Chem- chapter 5 practice

The lattice energy of an ionic compound tends to _____ as ionic size increases and tends to _____ as the charge of one or both of the ions increases, although the arrangement of the ions in the solid also plays a role. NaCl will, therefore, have a _____ lattice energy than NaBr but a _____ lattice energy than Na2O.

decrease; increase; greater; lower

When an electron is removed from an atom the atomic radius decreases and when an electron is added the atomic radius increases. This is due in large part to changes in _____.

electron-electron repulsions

The amount of energy required to separate 1 mole of ions in a crystalline solid into separate gaseous ions is called _____ energy. This energy provides a measure of the strength of a(n) _____ bond, since the stronger the bond, the _____ the amount of energy required to break it.

lattice; ionic; greater

Which of the following options correctly describe the general trends followed by elements when they form ions? Select all that apply. •The charge of a main group cation is equal to its group number. •Metals generally form cations. •Noble gases do not usually form ions. •Nonmetals tend to lose electrons. •The charge of a main group anion is equal to (18 - group number).

•The charge of a main group cation is equal to its group number. •Metals generally form cations. •Noble gases do not usually form ions.

Which of the following factors affect the magnitude of the lattice energy for an ionic compound? •The number of valence electrons in the ions •The total number of positive and negative ions present in the sample •The size of the ions •The charges of the ions

•The size of the ions •The charges of the ions

What does it mean if two species are isoelectronic? Select all that apply. •They are in the same group in the periodic table. •They have the same electron configuration. •They have the same number of electrons. •They have the same charge.

•They have the same electron configuration. •They have the same number of electrons.

When the elements Mg and Cl form an ionic bond, Mg loses ______electron(s) from the 3s orbital to form the Mg2+ cation. Cl gains ______electron(s) in the 3p orbital to form the Cl- anion. Since the total number of electrons lost always equals the total number of electrons gained, the compound formed will contain_____Mg2+ ion(s) for every _____Cl- ion(s). Fill in the blanks with the appropriate numbers.

2 1 1 2

The bond typically observed when a metal bonds to a nonmetal is the _____ bond. The metal atom _____ one or more valence electrons while the nonmetal _____ electrons.

Ionic; Loses; Gains

Mg2+, Na+, and F- all have the same electron configuration as Ne, and are described as being _____ with Ne and with each other.

Isoelectronic

An ionic compound consists of a three-dimensional array of cations and anions called a(n)_______.

Lattice

Which of the following metal ion electron configurations is incorrect? •Mn4+ [Ar]4d3 •Fe3+ [Ar]3d5 •Cd2+ [Kr]4d10 •Ag+ [Kr]4d10 •Zr3+ [Kr]4d1

Mn4+ [Ar]4d3

A compound consists of atoms of ______or more different______ that are chemically bonded together.

Two; Elements

Select the correct electron configuration for Sn4+. •[Kr]5s24d8 •[Kr]5s24d65p2 •[Xe]4d10 •[Kr]4d10

[Kr]4d10

Arrange the following ions in increasing size with the smallest at the bottom. •H •H+ •H-

• H- • H • H+

A cation is smaller than its parent atom, whereas an anion is larger. Which of the following statements correctly explain this observation? Select all that apply. •A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. •The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell. •When an atom gains one or more electrons, its radius increases due to electron-electron repulsions. •When an anion is formed its radius increases because it gains an electronic energy level.

•A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. •The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell. •When an atom gains one or more electrons, its radius increases due to electron-electron repulsions.

Which of the following statements correctly describe compounds? Select all that apply. •A compound has a fixed mass ratio of its components. •A compound contains a fixed number of atoms in its formula. •The components of a compound can be separated physically. •A compound is a pure substance. •The properties of a compound are the same as the properties of its component elements.

•A compound has a fixed mass ratio of its components. •A compound contains a fixed number of atoms in its formula. •A compound is a pure substance.

Which of the following statements correctly describe the structure of an ionic compound? •An ionic compound consists of a three-dimensional array of cations and anions. •The three-dimensional arrangement of cations and anions is called a lattice. •All ionic compounds have the same spatial arrangement of cations and anions. •The ratio of cations to anions is such that the compound is electrically neutral overall. •Each cation in the compound is associated with a particular anion.

•An ionic compound consists of a three-dimensional array of cations and anions. •The three-dimensional arrangement of cations and anions is called a lattice. •The ratio of cations to anions is such that the compound is electrically neutral overall.

Arrange the following ionic compounds in order of increasing lattice energy (increasing strength of the ionic bond) based on general trends in lattice energy. Start with the compound that has the lowest lattice energy at the top of the list. •MgCl2 •CaBr2 •Li2O

•CaBr2 •MgCl2 •Li2O

Match each type of ion with the correct description of its size relative to its parent atom.

•Cation - smaller than its parent atom •Anion - larger than its parent atom

List the following species in order of increasing radius, with the species with the smallest radius at the top of the list. F, O2-, F-, N3-

•F •F- •O2- •N3-

Which of the following monatomic ions have the electron configuration 1s22s22p6? Select all that apply. •F- •Li+ •O2- •S2- •Na+

•F- •O2- •Na+

Which of the following statements correctly describe ionic bonding? •Ionic bonding involves the transfer of electrons from the metal to the nonmetal. •Positive and negative ions combine in individual units of two or three ions each. •An ionic bond is the electrostatic attraction between two oppositely charged ions. •Ionic bonding is typically observed when two nonmetals bond.

•Ionic bonding involves the transfer of electrons from the metal to the nonmetal. •An ionic bond is the electrostatic attraction between two oppositely charged ions.

Which of the following statements correctly describe the trends in ionic size? Select all that apply. •Cations are smaller than their parent atom because of an increase in electron-electron repulsion. •Ionic size increases down a group on the periodic table. •For cations of the same element, cation size increases with increasing charge. •Anions are larger than their parent atom.

•Ionic size increases down a group on the periodic table. •Anions are larger than their parent atom.

Match each of the following elements with the correct number of electrons lost or gained to form its most common ion •K •Cl •Mg •S

•K - loses 1 electron •Cl- Gains 1 electron •Mg- loses 2 electron •S- gains 2 electrons

Consider the formation of an ionic bond between the elements potassium (K) and chlorine (Cl). Which of the following statements describe this process correctly? •Cl gains two electrons to form the Cl- anion. •K loses one electron from its 4s orbital to form a K+ cation. •The formation of this bond requires two K atoms for every one Cl atom. •The total number of electrons lost equals the total number of electrons gained. •Both the K+ and Cl- ions have full outer shells containing 8 electrons.

•K loses one electron from its 4s orbital to form a K+ cation. •The total number of electrons lost equals the total number of electrons gained. •Both the K+ and Cl- ions have full outer shells containing 8 electrons.

Which of the following options correctly describe lattice energy? •Lattice energy is the energy required to separate 1 mol of an ionic solid into gaseous ions. •Lattice energy is the energy required to arrange the ions of an ionic solid in a regular lattice. •Lattice energy is the energy required to force gaseous ions together to form 1 mol of an ionic solid. •Lattice energy provides a measure of the strength of an ionic bond. •Lattice energy decreases as the attraction between the ions increases.

•Lattice energy is the energy required to separate 1 mol of an ionic solid into gaseous ions. •Lattice energy provides a measure of the strength of an ionic bond.

Arrange the following ionic compounds in order of decreasing lattice energy (decreasing strength of the ionic bond) based on general periodic trends. Start by placing the compound with the highest lattice energy at the top of the list. •KBr •MgO •Na2O

•MgO •Na2O •KBr

List the following species in order of increasing size, starting with the atom/ion with the smallest radius on top to the largest at the bottom. •Br- •Kr •Se2- •Rb+

•Rb+ •Kr •Br- •Se2-

Predict the arrangement of the following isoelectronic ions in increasing size (with the smallest at the bottom). •Sc3+ •K+ •S2- •Ca2+

•S2- •K+ •Ca2+ •Sc3+