Chemical Bonding

Question 1

Ionic bonding occurs between atoms with large differences in their tendencies to lose or gain electrons. Such differences occur between reactive metals (Grps 1A and 2A) and nonmetals (Grp 7A and the top of Grp 6A)

A. Nonmetal with nonmetal: electron sharing and covalent bonding
B. Metal with nonmetal: electron transfer and ionic bonding
C. Metal with metal: electron pooling and metallic bonding

Answer 1

A. Metal with nonmetal: electron transfer and ionic bonding

Question 2

A _____ (with low ionization energy or IE) loses its one or two valence electrons, and a nonmetal atom (with highly negative electron affinity or EA) gains the electron/s.

A. Acid Atom
B. Salt Atom
C. nonmetal atom
D. metal atom

Answer 2

D. metal atom

Question 3

_____________________________ occurs, and each atom forms an ion with a noble gas electron configuration. The electrostatic attractions between these positive ions (cations) and negative ions (anions) draw them into a three-dimensional array to form an ionic solid.

A. Electron transfer from nonmetal to metal
B. Electron configuration from nonmetal to metal
C. Electron transfer from metal to nonmetal
D. Electron configuration from metal to nonmetal

Answer 3

C. Electron transfer from metal to nonmetal

Question 4

Note that the chemical formula of an ionic compound is the ______ because it gives the cation-anion ratio

A. empirical formula
B. formula
C. molecular formula
D. molecule

Answer 4

A. empirical formula

Question 5

____ are written and named with the cation or positive ion first followed by the anion or negative ion.

A. Ionic mixture
B. Ionic bonding
C. Ionic formula
D. Ionic compounds

Answer 5

D. Ionic compounds

Question 6

When two atoms differ little, or not at all, in their tendencies to lose or gain electrons, we observe electron sharing and covalent bonding, which occurs most commonly between nonmetal atoms, as in O─H in H2O.

A. Nonmetal with nonmetal: electron sharing and covalent bonding
B. Metal with nonmetal: electron transfer and ionic bonding
C. Metal with metal: electron pooling and metallic bonding

Answer 6

A. Nonmetal with nonmetal: electron sharing and covalent bonding

Question 7

Note that the chemical formula of a covalent compound is the _____ because it gives the actual numbers of atoms in each molecule.

A. empirical formula
B. formula
C. molecular formula
D. molecule

Answer 7

C. molecular formula

Question 8

Metal atoms are relatively large, and their few outer electrons are well-shielded by filled inner levels (core electrons). Thus, they lose outer electrons easily (low ionization energy or IE) and do not gain them readily (slightly negative or positive electron affinity or EA). These properties lead metal atoms to share their valence electrons, but not by covalent bonding.

A. Nonmetal with nonmetal: electron sharing and covalent bonding
B. Metal with nonmetal: electron transfer and ionic bonding
C. Metal with metal: electron pooling and metallic bonding

Answer 8

C. Metal with metal: electron pooling and metallic bonding

Question 9

Unlike the localized electrons in covalent bonding, electrons in ____ are delocalized, moving freely throughout the entire piece of the metal.

A. ionic bonding
B. ionic formula
C. metallic bonding
D. metallic formula

Answer 9

C. metallic bonding

Question 10

gather together

a. loop/looping
b. pool/pooling
c. delocalized
d. Localized

Answer 10

b. pool/pooling

Question 11

just in one place

a. loop/looping
b. pool/pooling
c. delocalized
d. Localized

Answer 11

d. Localized

Question 12

can travel and move freely

a. loop/looping
b. pool/pooling
c. delocalized
d. Localized

Answer 12

c. delocalized

Question 13

In ______________, the element symbol represents the nucleus and inner electrons, and dots around the symbol represent the valence electrons. Note that the pattern of dots is the same for elements within a group.

A. the Octet Rule
B. the Polarity
C. the Covalent
D. the Lewis electron-dot symbol

Answer 13

D. the Lewis electron-dot symbol

Question 14

For a metal, the total number of dots is the number of electrons an atom loses to form a ____

A. polar bond
B. cation (+ ion)
C. nonpolar bond
D. anion (- ion)

Answer 14

B. cation (+ ion)

Question 15

For a nonmetal, the number of unpaired dots equals either the number of electrons an atom gains to form an______ or the number it shares to form covalent bonds.

A. polar bond
B. cation (+ ion)
C. nonpolar bond
D. anion (- ion)

Answer 15

D. anion (- ion)

Question 16

when atoms bond, they lose, gain, or share electrons to attain a filled outer level of eight electrons (or two, for H and Li).

A. Octet Rule
B. Polarity
C. Covalent
D. Lewis electron-dot symbol

Answer 16

A. Octet Rule

Question 17

formed due to the unequal electron sharing.

A. polar bond
B. cation (+ ion)
C. nonpolar bond
D. anion (- ion)

Answer 17

A. polar bond

Question 18

formed due to the equal electron sharing

A. polar bond
B. cation (+ ion)
C. nonpolar bond
D. anion (- ion)

Answer 18

C. nonpolar bond

Question 19

refers to the number of electron pairs being shared by a given pair of atoms

A. BOND ANGLE
B. BOND ORDER
C. BOND LENGTH
D. BOND ENERGY

Answer 19

B. BOND ORDER

Question 20

The most common bond consists of one bonding pair of electrons. Thus, a single bond has a bond order of 1.

A. Single bond
B. Double bond
C. Triple Bond
D. Bond

Answer 20

A. Single bond

Question 21

consists of two bonding electron pairs, four electrons are shared between two atoms, so the bond order is 2. Examples are O═O or O2

A. Single bond
B. Double bond
C. Triple Bond
D. Bond

Answer 21

B. Double Bond

Question 22

consists of three shared pairs; two atoms have six electrons, so the bond order is 3. Examples are N≡N or N2

A. Single bond
B. Double bond
C. Triple Bond
D. Bond

Answer 22

C. Triple bond

Question 23

the energy needed to overcome this attraction and is defined as the standard enthalpy change for breaking the bond in 1 mol of gaseous molecules.

A. BOND ANGLE
B. BOND ORDER
C. BOND LENGTH
D. BOND ENERGY

Answer 23

D. BOND ENERGY

Question 24

the distance between the nuclei of two bonded atoms.

A. BOND ANGLE
B. BOND ORDER
C. BOND LENGTH
C. HYBRIDIZATION

Answer 24

C. BOND LENGTH

Question 25

a _______ results in a shorter bond length and a higher bond energy or a stronger bond. A. significant bond order B. large bond order C. stronger bond order D. higher bond order

Answer 25

D. higher bond order

Question 26

the angle formed by the nuclei of surrounding atoms with the nucleus of the central atom at the vertex. A. BOND ANGLE B. BOND ORDER C. BOND LENGTH C. HYBRIDIZATION

Answer 26

A. BOND ANGLE

Question 27

Its basic principle is that, to minimize repulsions, each group of valence electrons around a central atom is located as far as possible from the others. A. Valence-electron Pair Repulsion (VEPR) Theory B. Valence-Shell Electron-Pair Repulsion (VSEPR) Theory C. Valence-Shell Electron-Polar Repulsion (VSEPR) Theory D. Valence-Shell Energy-Pair Repulsion (VSEPR) Theory

Answer 27

B. Valence-Shell Electron-Pair Repulsion (VSEPR) Theory

Question 28

A ______ of electron is any number that occupies a localized region around an atom: single bond, double bond, triple bond, lone pair, or even lone electron. A. group B. bond C. configuration D. geometry

Answer 28

A. group

Question 29

This is the three-dimensional arrangement of nuclei joined by the bonding groups. A. Molecular Shape or Configuration B. Molecular Shape or Arrangement C. Molecular Shape or Geometry D. Molecular Shape or Group

Answer 29

C. Molecular Shape or Geometry

Question 30

Molecular shape with two electron groups A. Tetrahedral Arrangement B. Octahedral Arrangement C. Linear Arrangement D. Trigonal Planar Arrangement E. Trigonal Bipyramidial Arrangement

Answer 30

C. Linear Arrangement

Question 31

_____________ attached to a central atom point in opposite directions (AX2). This linear arrangement of electron groups in a molecule with a linear shape and a bond angle of 180°. A. Four electron groups B. One electron groups C. Seven electron groups D. Two electron groups

Answer 31

D. Two electron groups

Question 32

Molecular shapes with four electron groups A. Tetrahedral Arrangement B. Octahedral Arrangement C. Linear Arrangement D. Trigonal Planar Arrangement E. Trigonal Bipyramidial Arrangement

Answer 32

A. Tetrahedral Arrangement

Question 33

In tetrahedral arrangement, the four electron groups lie at the corners of a tetrahedron, a polyhedron with four faces made of equilateral triangles, giving bond angles of______ A. 180° B. 110° C. 109.6° D. 90°

Answer 33

109.5°

Question 34

Molecular shapes with five electron groups A. Tetrahedral Arrangement B. Octahedral Arrangement C. Linear Arrangement D. Trigonal Planar Arrangement E. Trigonal Bipyramidial Arrangement

Answer 34

E. Trigonal Bipyramidal Arrangement

Question 35

Five mutually repelling ______ form the trigonal bipyramidal arrangement, in which two trigonal pyramids share a common base. A. electron configuration B. electron formula C. electron molecule D. electron groups

Answer 35

D. electron groups

Question 36

Molecular Shapes with six electron groups A. Tetrahedral Arrangement B. Octahedral Arrangement C. Linear Arrangement D. Trigonal Planar Arrangement E. Trigonal Bipyramidial Arrangement

Answer 36

B. Octahedral Arrangement

Question 37

_________ form the octahedral arrangement. A. Ten electron groups B. Eight electron groups C. Seven electron groups D. Six electron groups

Answer 37

D. Six electron groups