Chapter 6-7: Ionic and Metallic Bonding

Question 1

What is the formula for lead(II) nitrate?

Answer 1

Pb(NO₃)₂

Question 1

What is the name of the compound Sr(NO₂)₂?

Answer 1

Strontium nitrite

Question 2

A regular, repeating, three dimensional array of atoms, molecules or ions that minimizes energy.

Answer 2

Crystal

Question 2

Using electron dot structures, predict the formula for rubidium phosphide.

Answer 2

Rb₃P

Question 2

What is the formula for nickel(III) sulfide?

Answer 2

Ni₂S₃

Question 3

A charged group of covalently bonded atoms.

Answer 3

A polyatomic ion

Question 4

Which of the following would you expect to have a higher melting point? Why?

KCl or CaCl₂

Answer 4

CaCl₂ should have the higher melting point. Calcium is a smaller ion than potassium, causing the charges to be closer together, and the lattice energy to be stronger. Additionally, the calcium ion has a +2 charge, but the potassium ion has only a +1 charge. Lattice energies (and thus melting points) are higher for ions having higher magnitude charges.

Question 4

A rule that states that atoms form compounds in order to achieve 8 valence electrons (a noble gas electron configuration).

Answer 4

The octet rule

Question 4

The collection of a metal’s delocalized valence electrons that move freely throughout the metal, shared by all of the metal’s cation cores.

Answer 4

Electron sea

Question 4

What is the name of the compound MgCl₂?

Answer 4

Magnesium chloride

Question 5

A compound composed of only 2 different elements; a monatomic cation and a monatomic anion. Their names always end in -ide.

Answer 5

Binary ionic compound

Question 6

How many total electrons are there in the phosphide ion, P^-3?

Answer 6

18

Question 8

A chemical bond that results from the electrical attraction between cations and anions.

Answer 8

Ionic bond

Question 9

What is the name of the compound KOH?

Answer 9

Potassium hydroxide

Question 10

The chemical bonding that results from the attraction between metal cation cores and the surrounding sea of electrons.

Answer 10

Metallic bonding

Question 10

The amount of energy as heat required to vaporize a metal. It is a measure of the strength of the bonds that hold the metal together.

Answer 10

Enthalpy of vaporization

Question 12

Which of the following would you expect to have a higher melting point? Why?

KF or KBr

Answer 12

KF should have a higher melting point than KBr. Fluoride and bromide ions have the same charge (-1), but the ionic radius of fluoride is much smaller than that of bromide. This results in a higher lattice energy since the positive and negative charges are closer together.

Question 13

A polyatomic ion containing oxygen.

Answer 13

Oxyanion (or oxoanion)

Question 15

A compound composed ot positive and negative ions (cations and anions) that are combined so that the numbers of positive and negative charges are equal.

Answer 15

An ionic compound

Question 16

The ability of a substance to be pulled into a wire.

Answer 16

Ductility

Question 17

What is the name of the compound V₂S₃?

Answer 17

Vanadium(III) sulfide

Question 18

Another term for an ionic compound.

Answer 18

Salt

Question 20

How many electrons are there in the zinc ion, Zn⁺²?

Answer 20

28 electrons. Metals lose valence electrons when forming ions. A +2 charge means there are two more positively charged protons than negatively charged electrons.

Question 21

Atoms or ions having the same electron configuration like Na⁺¹, Mg⁺², O^-2, F^-1, and Ar are….

Answer 21

Isoelectronic

Question 22

What is formula for zirconium oxide?

Answer 22

ZrO₂

Question 23

A substance that conducts electricty when melted or dissolved in water.

Answer 23

Electrolytes

Question 24

The ability of a substance to be hammered into thin sheets.

Answer 24

Malleability

Question 25

Adjective that describes the mobile valence electrons of a metal.

Answer 25

Delocalized

Question 26

What is the formula for ammonium phosphate?

Answer 26

(NH₄)₃PO₄

Question 28

The naming system that uses Roman numerals to indicate the charge of the ions of elements which can have multiple ions. For example: iron(III), copper(I), lead(IV).

Answer 28

Stock system

Question 29

Using electron dot structures, predict the formula for scandium flouride.

Answer 29

ScF₃

Question 30

An ion that results from either the gain or loss of one or more electrons by a single atom.

Answer 30

Monatomic ion

Question 31

Which substance would you expect to shatter when struck with a hammer? Why? Aluminum or aluminum oxide

Answer 31

Aluminum oxide would shatter. It is an ionic compound, It has a fixed crystal lattice. Striking it with a hammer would cause a shift in the ions that would put like-charged ions beside each other. The resulting repulsion would cause it to shatter. This is why ionic compounds are brittle. Aluminum metal simply dents when struck as the cation cores and sea of electrons simply shift in response to the impact.

Question 33

The energy released when one mole of ionic crystalline compound is formed from gaseous ions. or The change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase

Answer 33

Lattice energy

Question 34

The zinc ion's (Zn⁺²) electron configuration [Ar]3d¹⁰ illustrates what kind of stable electron configuration?

Answer 34

A pseudo noble gas electron configuration.

Question 35

What is the formula for sodium sulfate?

Answer 35

Na₂SO₄

Question 37

The lowest whole number ratio of cations to anions in an ionic compound. or The simplest collection of atoms from which an ionic compound's formual can be written.

Answer 37

Formula Unit

Question 38

What is the name of the compound SnO₂?

Answer 38

Tin(IV) oxide

Question 39

The formula for the iodate ion is IO₃^-1. What is the expected formula for the iodite ion?

Answer 39

IO₂^-1. Changing the suffix of a polyatomic ion from -ate to -ite involves removing an oxygen while keeping the charge the same.

Question 40

An ion that is formed as a result of a *single* atom either gaining or losing electrons?

Answer 40

A monatomic ion

Question 41

All monatomic ions have this ending.

Answer 41

-ide (like fluoride, telluride, oxide, bromide, etc...)