Chapter 7 Review

How do positive ions and negative ions form?

positive ion forms when an atom loses one or more valence electron. To form a negative ion it must gain the electrons lost by the cation.

Discuss how an ionic compound is named.

An ionic compound is named by putting the metal first and then having the nonmetal and taking out the suffix of that metal in adding -ide

Explain how an anion of nitrogen forms.

N gains three electrons, forming N3-, which has the stable electron configuration of Ne.

Using oxidation numbers, explain why the formula NaF2 is incorrect

Na has 1 valence electron, and F has 7, you would need 2 Na to balance for 2 F

Which are correct formulas for ionic compounds? For those that are not correct, give the correct formula and justify your answer. c. BaOH2

. BaOH2 (no) - Ba(OH)2

In Figure 14, the element labeled B is barium. and the element labeled E is iodine. Explain why the compound formed between these elements will not be Bal

A +3, B + 2, C +1, D -3, G -2, E -2 F noble gas no change

Discuss the formation of ionic bonds.

A positive ion is attracted to a negative ion and lattice energy is released.

Discuss the formation of the barium ion.

A positive ion is attracted to a negative ion and lattice energy is released.

Which are correct formulas for ionic compounds? For those that are not correct, give the correct formula and justify your answer. a. AlCl

AlCl3; one Al3 ion bonds to three Cl ions

Explain how the iron atom can form both an iron 2 + ion and an iron 3 + ion.

Based off of the charge of the anion

Describe an ionic crystal, and explain why ionic crystals for different compounds might vary in shape.

Because of the size of the ions that are bonded as well as the number of each type of ion bonded together.

Give the formula for each ionic compound. a. calcium iodide b. silver bromide c. copper(II) chloride cl. potassium periodate e. silver acetate

CaI2 Ag(I)Br Cu(II)Cl2 KIO4 Ag(I)C2H3O2

Which of these compounds are not likely to occur caKr, Na2S, BaCl3, MgF? Explain your choices.

CaKr-Kr is a noble ga, Na2S-not balanced, BaCl3-not balanced, MgF-not balanced

Why are halogens and alkali metals likely to form ions?

Halogens in Alkali metals are likely to form ions because their ionization energy is very low because they only need to lose or gain one electron.

Explain why steel, an alloy of iron, is used to build the supporting structure of many buildings.

Iron forms a strong metallic bond, giving solid iron hardness and strength.

Write the formulas for all of the ionic compounds that can be formed by combining each of the cations with each of the anions listed in Table 15. Name each compound formed.

K2SO3, potassium sulfite; KI, potassium iodide; KNO3, potassium nitrate; (NH4)2SO3, ammonium sulfite; NH4I, ammonium iodide; NH4NO3, ammonium nitrate; Fe2(SO3)3, iron(III) sulfite; FeI3, iron(III) iodide; Fe(NO3)3, iron(III) nitrate

Which has the greater lattice energy, CsCl or KCl? K20 or CaO? Explain your choices.

KCl, CaO

Which are correct formulas for ionic compounds? For those that are not correct, give the correct formula and justify your answer. b. Na3SO4

Na2SO4; two Na ions bond to SO4

Explain why potassium does not bond with neon to form a compound.

Neon already has an octet in its outer energy level; it is already stable.

Explain why noble gases are not likely to form chemical bonds.

Noble gases have a stable octet and are not likely to form a chemical bond. They have a low electron affinity.

Discuss the formation of a 3+ scandium ion orbital notation, shown in Figure 16.

Scandium, [Ar]4s23d1, loses both the 4s2 electrons and the 3d1 electron to form the 3 ion in the stable [Ar] configuration.

Explain what the name chromium(ill) oxide means in terms of electrons lost and gained, and identify the correct formula. Scandium (III) implies the metal has a 3+ charge due to roman numerals, oxide is 02-

The correct formula would be Sc2(III)O3

When are subscripts used in formulas for ionic compounds?

The subscripts used in farming was for ionic compounds are to show that there is more than one of an element in the compound

What does the term electrically neutral mean when discussing ionic compounds?

The term electrically neutral in an ionic compound means that when the two ions combine they have a charge of zero

Chrome Chromium, a transition metal used in chrome plating, forms both the Cr2+ and CrH ions. Write the formulas for the ionic compounds formed when these ions react with fluorine ions and with oxygen ions.

With fluorine they form: CrF2 and CrF3 With oxygen they form: CrO and Cr2O3

Discuss the formation of an ionic bond between zinc and oxygen.

Zn will lose its outer 4s electrons, forming Zn 2+ . Oxygen will gain the two electrons forming O 2- .Zn 2+ attracts O 2- and ZnO forms.

Which are correct formulas for ionic compounds? For those that are not correct, give the correct formula and justify your answer. d. Fe2O

a

Give the number of valence electrons in an atom of each element. a. Cesium d. Zinc b. Rubidium e. Strontium c. gallium

a. Cesium 1 d. Zinc 2 b. Rubidium 1 e. Strontium 2 c. gallium 3

Name each of the following ionic compounds. a. K20 b. CaCl2 c. Mg3N2 d. NaClO e. KN03

a. K20 potassium oxide b. CaCl2 Calcium chlorine c. Mg3N2 magnesium nitrogen d. NaClO sodium hypochlorite e. KN03 Potassium nitrogen

Predict the reactivity of each atom based on its electron configuration. a. Potassium b. Fluorine c. neon

a. Potassium ([Ar] 4s1) will lose one outer electron and form a 1+ ion. b. Fluorine ([He] 2s2 2p5) will gain one more electron and form a 1- ion. c. neon (1s2 2s2 2p6) will not react because it already has eight electrons in its outer energy level.

Determine the ratio of cations to anions in each a. potassium chloride, a salt substitute b. calcium fluoride, used in the steel industry c. calcium oxide, used to remove sulfur dioxide from power-plant exhaust d. strontium chloride, used in fireworks

a. potassium chloride, a salt substitute 1:1 b. calcium fluoride, used in the steel industry 1:2 c. calcium oxide, used to remove sulfur dioxide from power-plant exhaust 1:1 d. strontium chloride, used in fireworks 1:2

The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or fluorine? Explain.

fluorine since it has 7 valence electrons

Explain how a metallic bond is similar to an ionic bond.

here is an attraction between particles of unlike charges. a lattice structure is formed in the solid state: from 8 to 12 atoms/ions surround each atom/ion.

How is a metallic bond different from an ionic bond?

in an ionic bond the valence electrons are transferred from the metal only to the neighboring nonmetal, but in metallic bonding the valence electrons of each atom/ion are free to move or float around within the entire metal solid. in an ionic bond there are positive and negative ions being formed, but in metallic bonding there are only positive ions being formed

Discuss the importance of electron affinity and ionization energy in the formation of ions.

ionization energy is how easily an atom can lose an electron. - Electron affinity indicates how much attraction and atom has for electrons. If an atom loses an electron it becomes a positively charged ion or cation, and if an atom gains an electron it becomes a negatively charged ion or anion

Describe a metallic bond.

the force of attraction between a positive metal ion and the valence electrons it shares with the other ions

What information do you need to write a correct chemical formula to represent an ionic compound?

the names of the elements and their ionic charge

Briefly describe how malleability and ductility of metals are explained by metallic bonding.

when force is applied to a metallic solid, the metal ions and valence electrons can move