Ionic Compound

Ionic compounds are basically defined as being compounds where two or more ions are held next to each other by electrical attraction

Ionic Compounds

This is a summary of the past and present nomenclature or naming conventions for ionic compounds

Naming Compounds

An ionic compound is one in which at least two of the elements or compounds in the group are oppositely-charged ions held together

Ionic Compounds

Ionic compounds generally are very hard and have very high melting points. They are solids at room temperature

Face Centered Cubic

When metals react with non-metals they form an ionic compound. Ions have a charge because electrons are lost or gained in forming an ionic bond.

Saturday, August 27, 2011

Binary is composed of substance...



Binary is composed of a substance whose molecules consist of atoms of two parts. Individual atoms, each molecule can vary, but must belong to only two elements, isotopes, even if the items are allowed. Binary compounds in the definition, some of the simplest compounds in all of nature, but also some of the principal as well as organic and inorganic chemicals. They are broadly classified as ionic or covalent, depending on the bonding between atoms. Several sub-groups and divisions of binary chemical compounds to identify the class and educational purposes.

A substance consisting of a metal and a nonmetallic element is a binary ionic compound. These compounds are formed when the positively charged ions bond with the negatively charged ions. Ionic bonds form the atoms are very strong and require a lot of energy to break. In most cases, the positively charged ions are atoms of the metal, and negatively charged ions from a metal no. Many compounds are salts such as common table salt which is composed of a sodium atom and a chlorine atom.

Another important type consists of a combination of atoms linked by covalent bonds. Covalent chemical bonds are not as strong as ionic bonds, ie the relatively low energy needed to break them. Hydrocarbons consist of only carbon and hydrogen atoms are of a type of binary covalent compound. Water is perhaps the most familiar. This compound covalently consists of two hydrogen atoms and one oxygen atom.

Chemists have developed a system for naming chemicals and other substances, and knowing little about the conventions of the system can help identify some binary compounds using their own names. The names of ionic compounds, which tend to be associated with a metal non-metal, is generally formulated with the name of the metal, followed by an abbreviation of the name of the non-metallic, with the suffix "-ide . 'For example, the sodium chloride salt, the "idea" to help identify it as a binary relation. Covalent compounds follow the same conventions, and binary compounds of two different period may have changed with a prefix, and describe more atoms of an element, such as carbon dioxide, which has two oxygen atoms. Other rules apply to certain other special cases, and sometimes, a substance do not follow the conventions at all.

Wednesday, August 17, 2011

Patterns of Chemical Bonding



Only a few elements on the periodic table are satisfied with their arrangement of electrons. This is due to an imbalance between the perceived positive and negative forces of attraction involved in the atom. Collage may be seen as a form of atoms undergo correction, resulting from the electronic configuration as stable as possible a full shell. This pattern is known Asthe octet rule. It is so called because the second row elements, and who need to fill eight valence electron shells. This is a golden rule, and there are many exceptions to this, but generally the elements combine in a way that results in that there are 8 valence electrons in their shells. An important exception is the closest orbital electron to the nucleus, this orbit requires only two electrons to fill it.


The electrons necessary for this purpose are not free, must come from somewhere. This is where the atomic bond This occurs when two atoms, dissatisfied with their electronic configurations meet to share / exchange of electrons to obtain a more stable configuration. There are two main types of atomic bonds:


A covalent bond where electrons are shared.


Bond ionic bonding that occurs after the transfer of electrons.


When you think of covalent bonds, always, always think about sharing. Atoms together and share electrons with each other in a sort of meshing model. This is the most common bond, and is completely non-metals.


Ionic bonds, however, occur when the attraction of one atom to another is sufficient to tear an electron-atom valence shell and make it part of them. Reception, or steal, the atom is the atom charge more positive than that, it takes between when the electron with negative charge more attractive the atom, was part of the first.


This change causes ionization, charge exchange of neutral atoms, both atoms. Exchange leads to a more stable configuration of the second atom, but what about the atom the electron has been taken in the first place? After that, and will deionize restabalize. Ionic bond forms when the positive charge (electron-deficient), the atom by atom is attracted to, the more negative charge (electron-rich). This attraction is not just the transfer of electrons. Thus the term "ionic bond" is a somewhat 'misleading. A more appropriate term would be "ionic attraction '


A "real life" alongside the covalent vs ionic dynamics of a pair of hand in front of a person being robbed, respectively. The couple shares a mutual attraction and covalent bonds are more stable than single, and there is a common link between them. A person who is being stolen and the thief closing (atom) and robbery (electrons) are more closely parallel the dynamics of ionic bond, because there is a common bond between the atoms, rather than an attraction.


You can ask how an ionic bond prefer a more stable configuration for the two atoms when one of them gets much the tree? For that, you believe that the elements are more attractive than others to electrons, called electro negativity, and it generally increases with the atom approaches a more stable configuration. If an atom with low electronegativity (such as sodium, which has an "extra" electrons), to something that has a high electronegativity (such as fluorine, which needs a more electrons to satisfy the byte), fluoride, sodium steal its electron to obtain a more stable configuration. Sodium is now slightly unfortunate, because now a more positive effect of the nucleus of a negative force of its electrons. It will have an equally mild attraction for the electron has been lost. This creates a situation that is lower in energy and more stable.


The molecule formed by this bond, in particular, is known as sodium fluoride, and is an excellent example of a salt. A salt is an ionic compound formed by bonds.Given the nature of their duties, the salts are very low and usually very soluble. Acids and bases are usually found in salt form (HCl and NaOH) for hydrogen (H) and hydronium (OH-) easily dissociate chlorine and sodium, respectively, in aqueous solution. All salts are called in this way, the first metal, nonmetal second and adds the suffix "IDE".

Monday, August 15, 2011

How ionic compounds Workstation


How ionic compounds Workstation


All ionic compounds are made up of tiny crystalline structures, which consist of positively charged particles called cations and negatively charged particles known as anions. In an ionic substance. Cations and anions to form a grid band that is very hard and brittle when you are in a solid state, ionic compounds are good electrical conductors because their ions can not move much. In an ionic liquid or substance which was dissolved in a polar solvent, however, is an ionic compound the ions are separated and allow electrons to move freely between them.

Applications

Ionic compounds have many uses. Table salt is an ionic compound. In fact, all forms of ionic salts. As a result, ionic compounds are mixed with other substances to produce different properties or divided in a solvent and used for their electrical conductivity or other purposes. Ionic compounds are also widely used in textile processing industry to remove stains from fabrics.

Benefits

Ionic compounds have several important advantages. They have very high melting and boiling points because their ions are linked together so well. Ionic compounds are very strong and are hard to break. Ionic compounds such as water, alcohol, acetone or other polar solvent dissolved provide high electrical conductivity. They are usually nontoxic, nonflammable, and can be produced from a number of different elements. Moreover, the ratio of cations and anions in an ionic compound can vary, causing different properties to be produced.

Disadvantages

Although ionic compounds are beneficial, but also have several disadvantages. For example, ionic solid compounds are very fragile and tend to break when broken. Ionic compounds have low thermal conductivity are usually solid at room temperature.

Tuesday, August 9, 2011

Examples of Covalent Bond



If we encounter the world, we have a huge lack of knowledge of the structures around the world in one easy movement unit aggregation is the difference between the atoms. Electromagnetic force to hold atoms together to form molecular compounds that come into an even larger molecules and polymers that are resistant as possible. This complexity reduction is likely that the electromagnetic forces between charged particles. Etching of atoms turns to pity, or to sell the source of electrons to create a network of molecules possible. Bond between the atoms can be covalent or ionic bond. They have two varieties of grass containing alkaline sizing. The purpose of this essay is an essay required of the alkaline-containing covalent attachment of the screen examples of the deposit.

What is a covalent bond?

We must first determine what is a covalent bond, before studying a few examples of this link. Because we have studied the theme of the covalent bond, we pretend we already know what an atom and has been reported with the atomic structure. Covalent atoms deposit is formed when you divide the unit, or calibration times between the electrons in the other. These shared electrons come from the span of money between the atoms, which keeps them together and only units that we chose to be a molecule. These shared electrons are the valence electrons of atoms spinning in their shells extreme.

Each atom, forming a covalent hand money to try to capture the courage, which has extremely filled electron orbitals of the atoms, which are still empty. As two atoms come together and share electrons, deposit, together with the electromagnetic force to conquer that between atomic nuclei and electrons within the municipality. In addition, the force between the combs of the electrons orbiting the two atoms, which causes the proton to get distorted. While the two atomic nuclei are excited about the town of electrons arc, a deposit is connected between the two atoms.

Depending on the similarities in the nucleus or Electronegativity (tendency to capture electrons from atoms), a single span Similarly, the electrons may or may not be evenly distributed. If they were distributed unevenly, the proton becomes "Polar" in the sense that the imbalance in spending towards the interior. Let's look at some examples of covalent payment in the next section. Understand the difference between covalent and ionic.

Examples of covalent

Initial Payment covalent atoms can exist between same or opposite. Here are some types of molecules covalently links including polar, nonpolar and coordinate covalent.

o Water (H2O): In this hydrogen protons to double share electrons with unique oxygen atoms that share electrons with their own double in return. This is an example of cold covalent bonds, which are combined since electronegativity of oxygen at altitude.

or hydrogen molecule (H2): This is a non-polar covalent intermediate as a period in the same nucleus is common between the two hydrogen atoms.

O ammonium chloride (NH4Cl): This is an example of coordinate covalent distribution, where the two electrons necessary for the fixation was assigned by the same atom. This is a special box with a covalent bond.

o hydrogen chloride (HCl): This is another one for the cold covalent deposit examples where the duration of heart from some closer to the chlorine atom has an electronegativity altitude.

Here is a list of inventory of refrigerated storage and non-polar covalent examples.

Examples of polar covalent nonpolar covalent bond Examples

Hydrofluoric acid (HF), nitrogen (N2)

Ozone (O3), methane (CH4)

Ammonia (NH3), carbon dioxide (CO2)

Hydrogen sulfide (H2S), chlorine (Cl2)

They were a little scholastic examples of covalent down payment, to be when we thought at the entrance of the kind that contains alkaline bond. As mentioned earlier, the pity of electrons between atoms, which inaugurates the proton is poorly by their electro negativity special. The few-more unbalanced electro-negativity, sometimes cool, they formed molecules. More on the electro-negativity, some more electrons are shared. Almost all organic molecules composed of CO bonded covalently linked. You will find plenty of examples of covalent deposit in organic chemistry.

The chemical binds to the investigation of a large-scale operation of the molecules from simple cuts similar to the oxygen molecules of the most formidable-like DNA (deoxyribonucleic acid). Each of these molecules are held together by covalent bonding between atoms base. We hope this test has simplified the process of covalent deposit for you. Study examples of covalent lowest paid in the retail, to absorb molecular-over settings.

Ion anhydrous barium chloride



Ion anhydrous barium chloride is the chemical compound with the formula BaCl2. He is one of the most important water-soluble salts of barium. Like other barium salts, is toxic and gives a flame yellow-green. It is also hygroscopic.


Anhydrous barium chloride in combination with other water-soluble barium is highly toxic. Sodium sulfate and magnesium sulfate are possible antidotes, because they form a solid insoluble BaSO4 Barium sulfate, which is not toxic.


First, let's look at their peril:


Eye contact may cause conjunctivitis l


Contact with skin causes irritation of the skin. Prolonged skin, especially if the skin is wet or damp, causing necrosis.


the case of accidental ingestion, causing kidney damage. Barium ion is a poison that causes muscle stimulation, and paralysis. The initial symptoms are gastrointestinal, including nausea, vomiting, colic and diarrhea, followed by myocardial and general muscular stimulation, tingling in the limbs.


Provided that the above condition occurs, what can we do to protect ourselves? I think the following is possible: Eye contact, you can wash eyes with plenty of water for at least 15 minutes, occasionally lifting the upper and lower eyelids. Get medical help as the skin, you should get medical care. Rinse skin with plenty of water for at least 15 minutes while removing contaminated clothing. Wash clothing before re-use, enjoy, then it is not possible to induce vomiting. If the victim is conscious and alert, give 2-4 cups of milk or water. Never give anything by mouth to an unconscious person. Get medical help immediately.

Saturday, August 6, 2011

Organometallic compounds



Organometallic compounds are highly reactive metals are used in basic and reducing agents. The key to understanding the chemical bond in compounds isoball principle is used. Organometallics plays an important role in other areas such as chemical and biological analysis. Depending on the nature of the organic compound, the nature of the link may vary depending on the type of ionic or covalent. There are also a number of complex linkages that characterize the coordination of the metal and organic binders, organic binders such as must always bind the metal through a heteroatom such as nitrogen and oxygen, and such compounds are then considered as coordination compounds. But if any of the ligands form a direct metal-carbon bonds, and therefore should generally be regarded as organometallic compounds. These compounds may also find practical applications, such as stoichiometric and catalytic active compounds, such as the use of ferrocene in place of tetraethyl lead as an anti knock.


Many organic compounds of coordination that occur in nature, such as hemoglobin that contains only one iron center is coordinated to nitrogen atoms.


It combines infrared data aspects of inorganic chemistry with organic chemistry, for which these compounds are also known as organo-inorganic compounds. The study of such inorganic compounds known as bioinorganic chemistry. If the fat-soluble alkoxides, and metal is defined as metalorganics. The second is based on organometallic compounds of titanium called Ziegler-Natta catalyst for producing polyethylene and other polymers. In addition, Wacker process for oxidation of olefins. So organic compounds that are linked to sodium ion is, while glued to the lead or tin, and are usually associated with lithium may be covalent bonds between the properties. Monsanto, the rhodium-carbonyl complex process used to produce acetic acid industrially. Includes all conventional metals, lanthanides, actinides, and semi-metals are considered to form organometallic compounds. These compounds may vary depending on the nature of the anionic portion, and can not generally be regarded as organometallic. Superbases work in organic synthesis, but reduce the flammability of their use by the industry seriously. NMR and infrared spectroscopy techniques are commonly used to determine the structure and bonding.

Friday, August 5, 2011

Classification of Crystals



The crystals are classified into four types:

(I) atomic crystals

(Ii) ionic crystals

(Iii) covalent crystals

(Iv) molecular crystals

This classification is based on the nature of forces and bonds between atoms, ions or molecules constituting the crystal.

(I) atomic crystals

Examples of these crystals are metals, so they are also called metal crystals. They are made of atoms packed and held together by metallic bonds. In metals, the valence electrons move freely in the crystal lattice and said that from an electron gas, where the positive ions are immersed. These crystals are characterized by: (a) Lustre (b) the high melting point (c) the electrical and thermal conductivity (d) ductility (drawing paper) (e) ductility (from to son).

(Ii) ionic crystals

These crystals consist of positively and negatively charged ions, held together by electrostatic forces of attraction. Individual ions

has no identity. They are characterized by: (a) The high melting point (b) of the conduction of electricity in the molten state and in solution. (C), accuracy and hardness (d) crystal growth without restriction until it is broken or has stopped growing.

(Iii) covalent crystals

These crystals are composed of atoms linked by covalent bonds. Covalent bonds are very strong. They need large amounts of energy to break them. Examples of covalent crystals are: graphite, diamond, silica and carborundum. In diamond, each carbon atom is connected to four other carbon atoms at an angle of 109 degrees, called the tetrahedral angle. Because of the close packing of atoms and the large number of covalent bonds, the diamond is very hard and has a high melting point.

In graphite, each carbon atom is connected to three carbon atoms at an angle of 120 degrees, forming layers of hexagons. Areheld adjacent layers together by weak Vander Waals forces. Due to the space between layers of flexible graphite layers slide easily over each other to

Graphite is a greasy texture. Graphite conducts electricity by air layers, because each carbon is one of the free electron. Covalent crystals are characterized by:

(A), high melting point (b) LD (c) the high refractive index

(Iv) in molecular crystals

These crystals are composed of molecules, such as ice, I <sub>2,</sub> CO <sub>2</sub> molecules are held together by forces following:

Hydrogen bonding (a) (which is a force of electrostatic attraction between a partially positive hydrogen atom of a molecule and an electronegative atom other molecules).

(B) A weak Vander Waal forces (due to the attraction between the atomic nuclei and electrons from one molecule to other molecules). Such

crystals are characterized by:

(A) The low melting point (b) no - the conduction of heat and electricity.

Thursday, August 4, 2011

chemistry key terms, terminology


Key Concepts


Chapter 1

1. Alchemy - a pseudo-science that has sought to transform base metals such as lead, gold, medieval science, which aimed to find a universal cure for the disease, and the magic potion of immortality

Second Biochemistry - the study of chemicals extracted from plants and animals

3. Chemical science, which studies the composition and properties of matter

4th Experiences - a scientific approach to data collection and record observations in a controlled

5th Hypothesis - A tentative proposal for a scientific principle that attempts to explain the importance of a data set collected in an experiment

6th Inorganic Chemistry - the study of chemicals that do not contain carbon

7. Natural law - a proposal widely tested in a scientific principle that states a measurable relationship under different experimental conditions

8th Organic Chemistry - the study of chemicals that contain carbon

9. The scientific method - the method approach to explore the natural and logical explanations for the results

10th Theory - a proposal widely tested in a scientific principle that explains the behavior in the wild

Chapter 2

First centimeters or meters - a common metric unit of length

2. gram or a kilogram - a common metric units of mass

3. milliliters or liters - A unit of measurement of volume

4. mass - the amount of the target, was measured in the balance

5. Weight - The force of gravitational attraction between an object and the planet is measured.

Sixth significant digits - the digits of a measurement known with certainty, plus a number that is estimated.

7. scientific notation - a method to express very large or small by placing the comma after the first significant digit, and adjusting the size with a power of 10.

8th percentage - The ratio (times 100) of a single volume with respect to all volumes in a group and parts per hundred.

9. instrument - a recording of a measure such as length, mass or volume

10. measure - a numeric value and unit expressing a physical quantity such as length, mass or volume

11. nonsignificant digits - the numbers to an extent that exceeds the accuracy of the instrument

12. uncertainty - the degree of inaccuracy in measurement instruments

13. Method unit of analysis - a systematic procedure to solve the problems that some procereds response units conversion value reated

14. factor unit - a ration of two quantities that are equivalent and can be applied to convert from one unit to another, for example, an inch foot/12

Chapter 3

1. calories - the amount of heat required to Reais 1 gram of water 1 ° C

2. Celsius (° C) - the basic unit of temperature in the metric system

3. Density - the amount of mass in a unit volume

4. Degrees Fahrenheit (OF) - The basic unit of the temperature of the English system

5. Heat - A measure of the total energy in a system

6th International System (SI) - a comprehensive system of measurement for the seven basic units

7. Joule - a unit of energy is the SI system

8th unit Kelvin (K) - - the basic unit of temperature in the SI

9. metric - a decimal system of measurement with the basic units

10. seconds - - the basic unit of time in the metric system

11. specific gravity (sp gr) - the relationship between the density of a liquid compared to the density of water at 4 ° C

12. specific heat - the heat required to raise 1 g of substance 1 º C

13. Temperature - A measure of the average energy in a system, the average kinetic energy of molecules in motion

14. volume on the go - a technique for determining the volume of water displaced

15. absolute zero - the theoretical temperature at which the kinetic energy of a gas is equal to zero.


Chapter 4

1. League - a homogeneous mixture of two or more metals

2. Atomic number - a number that identifies a certain part of

3. chemical changes - changes in materials, which change the chemical composition of

4. chemical symbol - an abbreviation of the name of an element

5. compound - a substance that can be decomposed into simpler substances

6. deposit - a change of state of a gas derict a solid

7th ductile - belongs to a metal, which can be drawn into a wire

8th element - a substance that can not be decomposed by chemical reaction

Ninth law of conservation of energy - the law states that energy can not be created or destroyed

10th Law of conservation of mass and energy - the law is called the total mass and energy are constantly

11. malleable - the property of a metal that can be machined in one piece

12. Periodic Table - a table that organizes the elements according to their properties

13. physical changes - a feature that can not be obse4rved change the formula of the substance

14. The potential energy (PE) - energy stored in the field due to hold its position or composition of the

15. pure substance - issues with a clear composition and properties of Constance, for example, and the element or compound

16th fitness - Designates the status of a substance existing in solid, liquid or gas.

17th sublimation - direct change of state from a solid to a gas without forming a liquid

18. molecule - The smallest particle that represents a compound

19. The kinetic energy - the energy associated with the movement of molecules.

20. homogeneous material - the material to the standard configuration, a feature consistent and clear

21st element - a pure substance that can not be divided again by ordinary chemical reaction

22. compound - a pure substance that can be decomposed into two or more simpler substances by chemical reaction

23. heterogeneous mixture - Material that has a variable composition and properties of materials indeterminate consists of two or more substances which may be separated physically.

24. homogeneous mixture - issues associated with a variable composition, but a characteristic clear and consistent, are examples of natural gas, gasoline, and bronze.

25th atom - The smallest particle that represents an element

26th chemical formula - a symbolic representation of a complex indicates the number of atoms of each element

27. metal - an element that is usually shiny in appearance, has a high density and high melting point, and is a good conductor of heat and electricity

28. Non-metallic - an element that is usually boring in appearance, has a low density and low melting point, and is not a good conductor of heat and electricity

29. semimetal or metalloid - An element that is usually metal, as in the appearance and properties that are between a metal and nonmetallic.

30th law of constant composition or final - the principle that a compound that still contains the same elements in the same proportion by mass

31. Physical feature - a feature that can be detected without changing the chemical formula of the substance.

Chapter 5

1. atomic mass unit - a unit of mass equal to exactly 1.12 the mass of an atom of C-12

2. atomic notation - a symbolic method to express the composition of an atomic nucleus

3. electronic assembly - fast arrangement of electrons in the description of the authors' of the sublevels of the growing energy needs

4. spectrum of emission lines - a collection of narrow bands of light produced by the atoms of a particular element, releasing energy

5. sublevel energy - energy of electrons division level because of my energy level

Sixth orbital - a region around the nucleus, where it is very likely to find and electrons with a given energy

7. photon - a partical of radiant energy

8th quantum atom - a sophisticated model of the atom that describes the energy of an electron according to its probability of being found in a particular location around the nucleus

9. uncertainty principle - a statement that it is impossible to accurately measure the location and energy of a particle at the same time

10th Electron - A subatomic particle that has a negligible mass and charge of a relative minus

11. protons - subatomic particle with a mass of about 1 AMU and the equivalent for more than one

12. Neutron - a neutral particle in an atom, whose mass is about 1 amu

13. atomic nucleus - a region of high density in the center of the atom

14. Atomic number - number of the feature that indicates the number of protons in the heart of one of its atoms

15th lot of numbers - A number representing the total number of protons and neutrons in the nucleus of an atom

16. isotopes - atoms that have the same atomic number but different mass numbers. Atoms of the same element that have different numbers of neutrons in the nucleus.

17. Atomic mass - mass weighted average of the natural isotopes of the element.

18. Bohr atom - the atomic model of the images of the electron around the nucleus of specific orbital energy.

Chapter 6

1.

2. alkali metals - Group IA elements / 1, hydrogen is not

3. alkaline earth metals - Group II / 2 elements

4. Halogen - The Group of elements VIIA/17

5. noble gases - Group elements VIIIA/18

6. Group - A vertical column of the periodic table, a family of elements with similar properties.

7. period - a horizontal line on the periodic table, a series of elements with properties ranging from non-metallic metal.

8. Representative Elements - Group A elements (1,2,13-18) in the periodic table, also called main group elements.

9. transition elements - Group B (3-12) of the periodic table of elements.

10. Valence electrons - electrons that take the outermost atomic and sub sp, which are involved in chemical reactions

11. electrons points formula - a representation of an atom and its valence electrons, which shows the chemical symbol surrounded by a dot for each valence electron.

12th Ion - An atom that carries a charge due to gain or lose valence electrons

13. ionization energy - the amount of energy needed to remove the electron-neutral atom in a gaseous state

14. isoelectronic - refers to two or more of the ions with the same electronic configuration, for example, O2 and Mg 2 + each have 10 electrons, and their electron configurations are the same as the noble gas neon.

15th inner transition elements - the elements of the lanthanide series and actinide

16. lanthanide series - elements with atomic number 58-71

17. series actinides - elements with atomic number 90-103

Chapter 7

1. organic compound - any compound containing the element carbon.

2. inorganic compound - a compound does not contain the element carbon.

3. tion - a positively charged ion.

4. anion - a negatively charged ion.

5. formula units - the smallest particle of representative ionic compound.

6th aqueous solution - a substance dissolved in water

7. Binary acid - a slurry containing hydrogen and a nonmetal

8. ionic binary compound - a compound containing two nonmetals

9th IUPAC - the international system of rules for naming chemical compounds

10th Latin system - a system that means the tax on a cation with the suffix-ic or-UO

11. molecule - the only particle that represents a composite of non-metal atoms

12. monatomic ion - an atom that has a positive or negative charge

13. oxyanion - polyatomic anion that contains one or more elements combined with oxygen

14. polyatomic ion - a group of atoms bonded together with a positive or negative global charge

15th System images - a system that means the tax on a cation with Roman numerals

16. ionic ternary compound - a compound that contains three elements, including at least one metal

17. ternary oxyacid - combined with water, which contains hydrogen, nonmetal, and oxygen

Chapter 8

1. acid - hydrogen-containing compound that releases ions (H +) when dissolved in water.

Second base - A substance that releases hydroxide containing hydroxide ions (OH-) when dissolved in water.

3. an aqueous solution - a substance dissolved in water

4th chemical reaction - the process of undergoing a chemical change.

5. chemical equation - shorthand representation of formulas and symbols to describe the chemical changes.

6th reactive - A substance that undergoes chemical transformation.

7th product - a substance caused by a chemical change.

8. Catalyst - A substance that speeds up a reaction, but can be recovered without being changed forever.

9. exothermic reaction - a reaction that develops thermal energy.

10th endothermic reaction - a reaction that absorbs heat energy.

11. series of activities - a relative order of elements arranged by their ability to undergo reactions, also called electromotive series.

12. precipitate - an insoluble substance in the solution produced by a reaction.

13. combination of reaction - a reaction, in which the two substances produce a single compound.

14. decomposition reaction - a reaction in which two or more substances are produced from a single compound.

15th single replacement reaction - a reaction where a more active element displaces a less active for a solution or compound.

16. double displacement reaction - a reaction in which two different cations in ion exchange.

17. neutralization reaction - reaction of an acid and a base produces water and salt.

18th Salt - An ionic substance produced by an acid-base reaction, an ionic compound that does not contain hydroxide ions.

19. redox reaction - A chemical reaction in which electron transfer takes place.

20. coefficient - a figure in front of a chemical reaction that helps to balance a chemical equation

21. Index - a number in a chemical formula that represents the number of atoms or ions that appear on the substance

22. diatomic molecule - a particle composed of two nonmetal atoms

Chapter 9

1. Avogadro's Number (N) - the number of atoms, molecules or formula units, which form one mole of a substance, 6.02 x 1023 individual units.

2nd Mole - The amount of substance containing the same number of units as there are atoms in exactly 12 g of carbon-12.

Third molar mass - mass of a mole pure substance in grams, the mass of Avogadro's number of atoms, molecules or formula units.

4. empirical formula - The chemical formula of a compound that expresses the relationship simplest of atoms in a molecule or ion in a formula unit.

5th Molecular Formula - The chemical formula of a compound that expresses the actual number of atoms in a molecule.

6. molar volume - the volume of one mole of gas at standard temperature and pressure.

7. standard temperature and pressure or STP - A temperature of 0 ° C and atmospheric pressure arbitrarily chosen standard conditions

8. Avogadro's law - equal volumes of gas under the same conditions of temperature and pressure contain the same number of molecules.

9. gas density - the ratio of the mass per unit volume ofr a gas, in grams per liter

10th percentage composition - a list of the percentage mass of each element in a compound

Chapter 11

1. atmospheric pressure - The pressure exerted by gas molecules in the air at sea level this pressure is compatible with a column of 760 mm of mercury.

2. Barometric pressure - the pressure can be measured in the atmosphere.

3rd Torr - A unit of pressure equal to 1 mm Hg

4th vapor pressure - The pressure exerted by the molecules in gaseous form in dynamic equilibrium with the same type of molecules in a liquid state, for example, the water molecules of liquid water.

5. Boiling point - temperature at which the vapor pressure of the fluid is the same pressure.

6. Dalton is the partial pressure - pressure in the gas mixture is equal to the sum of the pressures exerted by each gas mixture.

7. partial pressure - The pressure exerted by a gas in a mixture of two or more gases.

8. vacuum - the volume, which contains none of the gas molecules.

9. Boyle's law - air temperature, pressure and volume of the gas are inversely proportional.

10. Avogadro's law - equal volumes of gas under the same conditions of temperature and pressure contain the same number of molecules.

11. standard temperature and pressure or STP - A temperature of 0 ° C and atmospheric pressure arbitrarily chosen standard conditions

12. Charles Law '- a constant temperature pressure, volume and Kelvin gas directly proportional.

13. ideal gas - a hypothetical gas that obeys the kinetic theory of perfect.

14. absolute zero - a temperature where the kinetic theory of gases is equal to zero.

15th ideal gas law - relationship PV = nRT for an ideal gas.

16. Combined Law - an indication that the pressure and the Kelvin temperature are directly proportional to the gas at constant pressure

17th Dalton law of partial pressure - a declaration that the pressure from a gas mixture is equal to the sum of the pressure of each gas

18. gas pressure - the pressure exerted by the molecules in the air

19. real gas - a real gas deviates from ideal behavior, which, under certain conditions

20. ideal gas constant - A constant principle of proportionality, the equation PV = nRT

Chapter 12

1. monatomic ion - a single atom, which is a positive or negative charge

2nd diatomic molecule - a particle that consists of two non-metal atoms

3. Valence electrons - electrons in atoms outer shell of energy that are available for bonding.

4th ionic bond - A chemical bond characterized by the attraction of a cation and an anion.

5. Covalent bond - a chemical bond characterized by sharing one or more pairs of valence electrons.

6. formula unit - the smallest body representative of a compound are held together by ionic bonds.

7th molecule - The smallest unit representing a compound held together by covalent bonds.

8th bonding electrons - the valence electrons in a molecule that is shared.

Nonbonding electrons 9th - the valence electrons in a molecule that is not shared.

10th Electron points formula - (.) A diagram of a molecule or polyatomic ion, where each atom is represented by its chemical symbol for each surrounded by a bonding or nonbonding electron, also called a Lewis structure.

11th structural formula - A diagram of a molecule of polyatomic ions, where each atom is represented by its chemical symbol associated with one row for each pair of bonding electrons.

12th Single Bond - A link consists of an electron appears as a unique link between them.

13. double bond - A bond consisting of two pairs of electrons showed that the two dashes between two atoms.

14th Triple Bond - A bond that consists of three pairs of electrons are represented by three lines between two atoms.

15. Electronegativity - the ability to split an atom to attract electrons in a pair of chemical bonding.

16th nonpolar covalent bond - A bond in which one or more pairs of electrons are shared equally.

17th Polar covalent bond - A bond in which one or more pairs of electrons are shared unequally.

18. Binding energy - the amount of energy needed to break the covalent bond two atoms

19. Bond length - distance from the nuclei of two atoms joined the covalent bond

20th chemical bond - the generic title of the attraction between two ions, or two atoms

21. molecular form - the geometric shape formed by atoms to the central atom in a molecule

22. Electron pair geometry - the geometric shape formed by the union and non-bonding electron pairs on the central atom of a molecule

23. VSEPR Theory - a model that explains the shapes of molecules as a result of the pairs of electrons on the central atom repel each other

24th octet rule - the claim that an atom tends to bind to acquire eight valence electrons

25. Delta notation - a method to indicate a partial negative charge and positive part in a chemical bond

26. polyatomic ions - a group of atoms bound together, and in general positive or negative charge

Chapter 13

1. vapor pressure - the pressure of gas molecules in a dynamic equilibrium of the same type of molecules in the liquid state, for example, water molecules in liquid water.

2. Viscosity - resistance of the fluid flow as a result of molecular attraction.

3. surface pressure - molecular attraction, which causes the liquid has a minimum area.

4. dispersion of forces - attraction of molecules based on the temporary dipoles of the molecules, also called London forces.

Fifth hydrogen bond - a bond that intermolecular between hydrogen and oxygen in both molecules have a polar group-OH.

6. heat of fusion - The heat required to convert a solid to a liquid at its melting point.

7. heat of vaporization - The heat required to convert a liquid into a gas at its boiling point.

8th hydrate - A substance that contains a number of water molecules per unit formula of a crystalline substance.

9. Anhydrous - means a compound that contains no water.

10. hard water - water that contains a variety of anions and cations such as Ca2 +, Mg2 +, Fe3 +, CO32-, SO42-, PO43.

11. Boiling point - temperature at which the vapor pressure of the fluid is the same pressure

12. demineralized water - water purified by the removal of ions by an ion exchange method, also called demineralized water

13th dipole force - an intermolecular attraction based on the permanent dipoles

14th electrolysis - the chemical reaction produced by an electric current through an aqueous solution

15. heavy water - water molecule, with hydrogen atoms has been replaced by a hydrogen atom with a neutron

16. metal oxide - a compound that reacts with water to form a solution, also called oxide-based

17. net dipole - the general direction of a partial negative charge is a molecule with two or more dipoles

18. non-metallic oxide - a compound that reacts with water to form an acid solution, also known as acid oxide

19. freshwater - water contains sodium ions and anions other than

Chapter 14

1. net dipole - the general direction of a partial negative charge is a molecule with two or more dipoles

Second solution - a component that is dissolved in a solvent to form a solution.

3. solvent - in the solution, part of the largest concentrations occur, usually in a liquid in which the solute dissolves.

Fourth solution - a homogeneous mixture at the atomic scale, molecular and / or ion consisting of a solute (or solutes) dissolved in a solvent.

5. Henry's Law - the principle that the solubility of a gas in a liquid is proportional to the partial pressure of gas above the liquid.

6. miscible - refers to two liquids that are soluble in one another.

7. immiscible - refers to two liquids that are insoluble in the other, and if mixed, separated into two layers.

8. a saturated solution - A solution in which the dissolved and undissolved solute are in dynamic equilibrium. A solution containing solute as much as possible to a specific temperature.

9. supersaturated solution - a solution unstable, which contains more than the solvent-impregnated at the same temperature.

10th dipole - a region of a polar molecule with a partial negative charge and partially positive

11th that dissolves as a rule - the principle that the solubility is greater when the polarity of the solute is similar to that of the solvent

12th non-polar solvents - a solvent which is composed of nonpolar molecules

13. polar solvent - a liquid compound polar solvent molecules

14. Solubility - the maximum amount of solute that can dissolve in a solvent at a given temperature

15. solvent cage - a group of solvent molecules around a solute particle in a solution

16. Unsaturated solution - a solution that contains less than the maximum amount of solute that can dissolve at a given temperature

Chapter 15

1. acid-base indicator - a chemical that changes color depending on the pH of the solution.

2. Arrhenius acid - a substance that provides hydrogen ions dissolved in water.

Arrhenius third base - A substance that allows hydroxide ions when dissolved in water.

4. hydronium ion H3O + or - ion that best represents the hydrogen ion in aqueous solution.

5. dissociation - an ionic compound dissolves in water and separated into positive and negative ions, for example, NaOH is dissolved in water, so that sodium ions and hydroxide ions.

6. amphiprotic - a substance that can accept or donate a proton in an acid-base

7. The Brønsted-Lowry acid - a substance that gives a proton in an acid-base

8th Bronsted-Lowry Base - a substance that accepts a proton in an acid-base reaction

9. buffer - a solution that resists changes in pH when acid or base is added

10th test - the scene in a titration when the indicator changes color

11th ionization constant of water (KW) - a constant that is equal to the molar hydrogen ion concentration and the molar concentration of hydroxide ions

12. Net ionic equation - the equation representing the chemical reaction in the viewer after the ion-ion have been deleted

13. pH - hydrogen ion concentration expressed on a scale molecular exponential

14th proton acceptor - a term used interchangeably with the acceptor of hydrogen ions

15th proton donor - a term used interchangeably with the donor hydrogen-ion

16. salt - a product derived from the neutralization reaction, in addition to water

17th spectator ions - ions that are dissolved in water, but does not appear in the net ionic equations

18th standard solution - a solution whose concentration was determined accurately

19th strong electrolyte - an aqueous solution, it is a good conductor of electricity

20. weak electrolytes - aqueous solution, which is a poor conductor of electricity

21st assay - a procedure to deliver a measured amount of solution through a burette

22nd Total ionic equation - an equation that represents the chemical substances highly ionized ionic form and slightly ionized substances in ionic form,

Chapter 16

1. reversible reaction - a reaction that moves forward and to the products as well as in the opposite direction towards the reaction.

Second balance - a dynamic state of a reversible reaction, where the rate of reaction front and rear are equal.

Third solid electrolytes - An aqueous solution containing a substance that implements strong electric current, for example, strong acids, strong alkalis, soluble salts.

4th weak electrolyte - An aqueous solution containing a substance that causes an electric current easily, for example, weak acids, weak alkalis, easily soluble salts.

5. exothermic reaction - a reaction that evolves heat energy.

6. endothermic reaction - a reaction that absorbs heat energy.

7th Catalyst - a substance that gives a reaction go faster by lowering the activation energy.

8. Heat of reaction - the energy difference between reactants and products

9. reaction rate - the rate at which the concentrations decrease in response per unit of time

Chapter 17

First Oxidation - A chemical change in which a substance loses electrons or an increase in oxidation number occurs.

Second oxidation number - a value assigned to an atom in a molecule or ion to keep track of electrons gained or lost value can be positive or negative and is zero in the free form.

3. Reduction - A chemical change in which electrons substances increase or a decrease in oxidation number.

4th oxidant - essentially reduced to a redox reaction.

5. reducing agent - the substance is oxidized in a redox reaction.

6. electrochemical cell - a generic term for devices that contain two different solutions in different sectors of the electrodes connected to run the wire.

7. Anode - The electrode in an electrochemical cell where oxidation occurs.

8. cathode - electrode electrochemical cell, where the reduction takes place.

9. photovoltaic cells or batteries - A general term for any electrochemical cell which produces electricity spontaneously.

10th redox reaction - a chemical reaction in which electron transfer takes place

11. electrochemistry - the study of the interconversion of chemical and electrical energy

12th electrolysis - it supplies electricity to a redox process nonspontaneous to provoke a reaction

Chapter 18

1. activity - the number of radioactive nuclei during the break in tha sample pieces to give time, for example, 500 dpm

2. alpha particles - nuclear radiation identical to helium-4 nuclear

Third atomic number (Z)-value indicating the number of protons in a nucleus

4. Beta particles - radioactive radiation, identical to that of the electron

5. chain reaction - nuclear fission reaction in which neutrons released to initiate a second reaction, which in turn, starts the third reaction, and so on

6. a critical mass - the minimum mass of fissile nuclide necessary to maintain a reaction chiain

7. Deuterium - hydrogen nuclide is a neutron

8. electron capture (EC) - a nuclear reaction in which a large nuclide is based on its inner core electrons in the nucleus

9th gamma rays - a nuclear radiation, similar to the light of high energy

10. The half-life - the amount of time required for 50% of the radioactive nuclei in a sample of corruption

11. mass number - the value indicating the number of protons and neutrons in a nucleus

12. the nuclear equation - with shorthand representation of the atomic notation to describe the nuclear reaction

13th Nuclear fission - a nuclear reaction in which a nucleus divides into two or more lighter nuclei

14. nuclear fusion - the nuclear reaction in which two light nuclei combine into a single core

15. nuclear reaction - a change that involves high-energy core

16. nuclide - the atom, which has a number of protons and neutrons

17. positrons - Identical to nuclear radiation byt the same opposite to the electron

18. Radiation - emission of particles or nuclear energy in an unstable

19th Transmutation - the conversion of one element to another by a nuclear reaction

20. tritium - the nuclide of hydrogen with two neutrons

Chapter 19

First hydrocarbon - an organic compound containing hydrogen and carbon.

Second alkane or saturated hydrocarbons - a hydrocarbon that contains only a single bond.

3rd unsaturated hydrocarbon - a hydrocarbon containing a double or triple bond.

4th aromatic hydrocarbons - a hydrocarbon containing a benzene ring.

Fifth structural formula - a chemical formula that shows the actual arrangement of atoms in a molecule.

6. Structural isomers - compounds with the same molecular formula but different structural formula.

7. combustion reaction - a chemical reaction with the hydrocarbon burns and is oxidized into carbon dioxide and water.

8th Polymer - A high molecular compound is composed of small repeating chemical units.

9. monomer - The chemical repeating unit in a compound of high molecular weight.

10th Polyester - A type of polymer formed by the reaction of a dicarboxylic acid and a dihydric alcohol.

11th polyamide - A type of polymer formed by the reaction of a dicarboxylic acid and diamine.

12th alkenes - a family of compounds consisting of unsaturated hydrocarbons containing a double bond

13th alkynes - a family of compounds consisting of unsaturated hydrocarbons having a triple bond

14th functional group - a family of drugs, where all members have the same structural characteristics

Chapter 20

1. Biochemistry - The study of biological compounds and their reactions.

2. polypeptide - a polymer of amino acids combined with organic amide.

3. amino acids - a biological compound contains both amino and carboxylic acid.

4. Peptide bond - amide link, which connects two amino acids.

Fifth enzyme - a biological compound that catalyzes a specific biochemical reaction.

6. carbohydrates - a biological compound, which is a polyhydroxy aldehyde or ketone.

7. monosaccharide - simple sugars such as glucose or fructose.

8th Lipid - A biological agent which is insoluble in water, such as a grease or oil.

9th fatty acids - a carboxylic acid with a long hydrocarbon chain.

10. fat - a lipid that consists mainly of saturated fats and fatty acids esterified to glycerol.

11th Oil - A lipid consisting mainly of unsaturated fatty acids esterified to glycerol.

12. nucleic acid - a polymer containing biological genetic information.

13. protein - a biological compound which is a polymer of amino acids


















Wednesday, August 3, 2011

Ionic bonding Vs. metallic bonding



Ionic bonding Vs. metallic bonding


As proposed by the American Chemical GNLewis, atoms are stable when they contain eight electrons in its valence shell. Most atoms have fewer than eight valence electrons in its shell (with the exception of noble gases in Group 18 of the periodic table), therefore are not stable. These atoms tend to react with each other to become stable. Thus, each atom can achieve a noble gas electron configuration. This can be done by forming ionic bonds, covalent or metallic.


Ionic bond


Atoms can gain or lose electrons and become positively or negatively charged particles, respectively. These particles are called ions. There are electrostatic interactions between ions. Ionic bond is the force of attraction between oppositely charged ions. The strength of the electrostatic interaction is largely influenced by the electronegativity of atoms in an ionic bond. Electronegativity is a measure of the affinity of the atoms of electrons. An atom with high electronegativity can attract the electrons of an atom with low electronegativity to form an ionic bond. For example, sodium chloride is an ionic bond between ions of sodium and chloride ion. Sodium is a metal, therefore, has a very low electronegativity (0.9) compared with chlorine (3.0). Because of this difference in electronegativity, the chlorine can attract an electron from the sodium form of Cl-and Na +. For this reason, the two atoms for stability, noble gas electron configuration.


Metallic bond


Metals are the atoms that can form cations by removing electrons. Group 1, Group 2 and transition elements are metals. Most metals are the time in the solid phase. The type of link between the shapes of the metal atoms is called metallic bonding. Metals release electrons in its outer layer, and these electrons are scattered among the metal cations. Therefore, they are known as a sea of ​​delocalized electrons. Electrostatic interactions between electrons and cations are called metallic bond. The number of electrons released in the sea, and the size of the cation determines the strength of the metal union. Size of the cations is inversely proportional to the strength of the union, and the number of electrons released is directly proportional to the strength of metal binding. The electrons can move, so that the metals have the ability to conduct electricity. Due to the metal union metals have an orderly structure.


Cl-and Na + are held together by electrostatic attractive forces, forming an ionic bond.


High melting points and boiling points of metals are also due to strong metal union. Metals are solid and not fragile, due to the strength of metallic bond.

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