ionic bonding puzzle

Ionic Bonding Puzzle Lab

Introduction

When metals and non-metals chemically react, the atoms will tend to form ions or charged atoms. Ions form because electrons are either gained or lost. Metals will generally form cations or positive ions, since they tend to donate electrons Non-metals will form anions or negative ions, since they tend to accept electrons.

Activity

In this activity you will create models of ionic compounds and observe the chemical formula of the binary molecules you have created. Your data will be recorded in a data table or chart, similar to the one below.

Cation name	Anion name	Chemical Formula	Name

Discussion/Conclusion (talk with your classmates and address in your write-up)

·         Notice the shape and charge of each cation model. Why do you think there are slots in the metal atoms? (TIP: How do the atoms become ions?)

·         Notice the shape and charge of the anion models. Why do you think there are tabs in the non-metal atoms?

·         If you were to make a neutral atom following the model, what would the shape be?

·         Group the ion models by family. What do you notice about the number of tabs or slots? What do you notice about the tabs or slots and charge of all ions? Is there a pattern? Why do you think the model is made that way?

·         In the compounds you formed, what do you notice about the ion charges, the net or final charge of the compound and how the charge relates to the chemical formula of the compound?

·         What do you notice about the names of the cations and anions on the cards. How do they compare with the name of the neutral atom or element. Do all metals have a number in parenthesis? Do the non-metals have anything in common about their name?

·         Is there a pattern between elements in a group or family and any numbers on the Periodic Table? (TIP: Think octet rule and how many electrons are involved to meet octet.)

Ionic Bonding Model Lab Scoring Rubric

4	Lab format follows the expected guidelines in the handout. Blank page on left for scores, Title, Purpose, Materials, Procedure, Data table, Discussion/Conclusion. Data is organized into a table with the names of cation, anion, chemical formula and compound name. Discussion and Conclusion addresses: Explain how the model relates to the ion; number and shape of slot, (ie. charge, cation, anion), what a neutral atom would look like in the model. Explain how elements are organized on the Periodic Table of Elements (i.e the category; metal or non-metal; and charge of the ion; amount of charge and position on the Periodic Table of Elements related to the valence electrons. Explain the connection between the ion charge and the ratio of atoms in the chemical formula for the ionic compound (the pieces fit together to balance charge) Identify the similarity in the name for all non-metal anions, similarity in the name for Alkai Metal and Alkaline Earth Metal cations; similarity in the name for all other metal cations.
3	Lab format follows the guidelines in the handout. Blank page on left for scores Data does not have 40 combinations, cation name, anion name, charge chemical symbol, and chemical name Missing some topics in the discussion or there is some incorrect information in parts of Discussion/Conclusion or data table.
2	Formatting problem Conceptual errors when writing chemical formula or name of compounds Missing or incorrect information in many parts of the Discussion/Conclusion
1	Major problems or conceptual errors.

Ionic Bonding Puzzle Lab Notes

The Model

Metals ___________ electrons and become positive ions or ______________.

Non-metals __________ electrons and become negative ions or _____________.

lose, cations, gain, anions

                     neutral atom                                                                    ions

                          metal                                    à

                       non-metal                               à

Using the same analogy for the atom, what would a +2 cation and a -2 anion look like?

Bonding and Predicting Chemical Formulas

Al₂O₃

The ______________ show the ___________ of each atom in the ________________.

subscripts, ratio, compound

For an ionic bond, the ________ need to balance _____________. The _____________ of each ion changes to make the compound _____________. The chemical ___________ shows how many of each ion are needed to _____________ the ____________ and make the compound neutral.

Ions, charge, number, neutral, formula, balance

What ratio will the +1 and -1 ions combine to balance the charge?

                                  +                                                        à

What ratio will the +2 and -1 ions combine to balance the charge?

                                  +                                                         à

 

Naming or Nomenclature

Use the name on the puzzle pieces to determine the name of each compound you created. TIP: In this lab if you create binary compounds you will save yourself time.

What do all of the Type II ions have in common?

What does the Roman Numeral show for a Type II ion?

Notice the Type ____ ions do not have a Roman Numeral. What are the charges of an ion formed from a Type I metal?

What do all ________ atomic non-metals or _______________ have in common?

mono-, anions

TIP: To make a subscript for a chemical formula, highlight the number and from the menu bar, select Format > Font > Subscript or A₂ on the Font Formatting Pallette

 

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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".

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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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