Deck 7: Chemical Bonds

Question 1

How many valence electrons does the representative element with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁵ possess?

A) 5
B) 3
C) 6
D) 7

Answer 1

7

Question 2

Elements in groups IIA and VA of the periodic table possess, respectively, how many valence electrons?

A) 2 and 2
B) 2 and 6
C) 3 and 4
D) 2 and 5

Answer 2

2 and 5

Question 3

Which of the following is the correct Lewis symbol diagram for carbon?

A)
B)
C)
D)

Answer 3

Question 4

Determine the number of valence electrons in an atom of antimony.

A) 1
B) 2
C) 4
D) 5

Question 5

Which of the following statements about the noble gases is incorrect?

A) All exist in nature as individual atoms rather than molecular form.
B) They are the most reactive of all gases.
C) All have very stable electron arrangements.
D) All have 8 valence electrons.

Question 6

Which option will correctly fill in the blank to define the octet rule? Atoms will ________ electrons so each atom involved will have a noble gas configuration.

A) share
B) lose
C) lose or gain
D) lose, gain, or share

Question 7

The notation Y^3- denotes a Y atom that has ________.

A) lost 3 electrons
B) lost 3 protons
C) gained 3 electrons
D) gained 3 protons

Question 8

Which of the following ions would not possess an "octet of electrons?"

A) P^2-
B) Be²⁺
C) K⁺
D) S^2-

Question 9

Which statement is incorrect?

A) An anion is a negatively charged ion.
B) Ions have different chemical properties than its corresponding atom.
C) Ionic bond is the attractive force between positively and negatively charged ions.
D) Ions are electrically neutral.

Question 10

Which is the electron configuration for a Sc³⁺ ion?

A) 1s² 2s² 2p⁶ 3s² 3p⁶
B) 1s² 2s² 2p⁶
C) 1s² 2s² 2p 3s²
D) 1s² 2s² 2p⁶ 3s² 3p³

Question 11

Which of the following represents the electron configuration of a selenium ion in its common oxidation state?

A) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁴
B) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶
D) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p²

Question 12

Elements in groups IIA and VIA of the periodic table would, respectively, be expected to form ions with charges of ________.

A) +1 and +7
B) -1 and -5
C) +1 and -1
D) +2 and-2

Question 13

The electron configuration for a Al³⁺ ion is ________.

A) 1s² 2s² 2p⁶
B) 1s² 2s² 2p⁶ 3s² 3p¹
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4 p⁶
D) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

Question 14

The electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ fits all of the following species except one. The exception is ________.

A) F^-
B) Ca²⁺
C) S^2-
D) P^3-

Question 15

Which of the following compounds contains an ion with a 3+ charge?

A) KCl
B) AlP
C) BeF₂
D) BaO

Question 16

What behavior is expected from an atom with the electronic configuration of

A) gain of 2 electrons
B) loss of 2 electrons
C) gain of 4 electrons
D) loss of 4 electrons

Question 17

Which ion is isoelectronic with Kr?

A) Cl^-
B) O^2-
C) Rb⁺
D) Ba²⁺

Question 18

Which of the following is not isoelectronic with a noble gas?

A) Li⁺
B) Ba²⁺
C) S^-
D) F^-

Question 19

Which one of the following sets contains species that are all isoelectronic?

A) O, F, Ne
B) C⁺⁴, N^-3, O^-2
C) P^-3, S^-2, Ar
D) Na, Mg, Al

Question 20

Which of the following compounds contains an ion with a 2- charge?

A) AlP
B) MgS
C) KBr
D) BaCl₂

Question 21

In the formation of the ionic compound CaBr₂ the number of electrons transferred from one Ca atom to two Br atoms, per formula unit, is ________.

A) 1
B) 2
C) 3
D) 4

Question 22

In the process of forming sodium nitride, Na₃N, each sodium atom ________ electron(s) and each nitride atom ________ electron(s).

A) loses one; gains two
B) loses three; gains one
C) loses three; gains three
D) loses one; gains three

Question 23

In which of the following pairings is the formula not consistent with the ions shown?

A) K₂O (K⁺ and O^-)
B) BaF₂ (Ba²⁺ and F^-)
C) Co₂S₃ (Co⁺³ and S^-2)
D) Na₃P (Na⁺ and P^3-)

Question 24

The correct formula for the ionic compound containing Ni²⁺ and NO^3? ions is ________.

A) NiNO₃
B) Ni₂NO₃
C) Ni(NO₃)₃
D) Ni(NO₃)₂

Question 25

The correct formula for the ionic compound formed between Ca and I is ________.

A) Ca₂I
B) CaI₂
C) Ca₂I₃
D) Ca₃I₂

Question 26

An ionic bond forms between two atoms through ________.

A) sharing of electron pairs
B) transferring of electrons from metallic atoms to nonmetallic atoms
C) transferring protons from the nucleus of the nonmetal to the nucleus of the metal
D) each atom acquiring a negative charge

Question 27

Which of the following pairs of elements would most likely form a covalent compound?

A) Na and Pb
B) F and S
C) Cu and Ar
D) Zn and K

Question 28

Which statement is incorrect?

A) Ionic compounds generally contain metal and nonmetal elements.
B) Formulas of ionic compounds are written with the anion first, then the cation.
C) Cations and anions combine in the simplest ratio which achieves electrical neutrality.
D) The number of electrons lost by the cation(s) must equal the number gained by anion(s) in an ionic compound.

Question 29

Which of the following formulas for an ionic compound is incorrect as written?

A) Al₂(CO₃)₃
B) Na₂S
C) Li₂SO₄
D) MgHCO₃

Question 30

Which of the following formulas for an ionic compound is incorrect as written?

A) Ca(SO₄)₂
B) KOH
C) MgS
D) NH₄ClO₄

Question 31

Which of the following statements is an accurate description of the structure of the ionic compound NaCl?

A) Alternating layers of Na and Cl molecules are present.
B) Alternating layers of Na⁺ and Cl^- ions are present.
C) Alternating rows of Na⁺ and Cl^- ions are present.
D) Each ion present is surrounded by six ions of opposite charge.

Question 32

A polyatomic ion is an ion that ________.

A) has a negative charge < -1
B) contains both a metal and a nonmetal
C) develops a charge as a result of the combination of two or more types of atoms
D) occurs alone as do molecules

Question 33

What is the correct chemical formula for a compound that contains K⁺ and CO₃^2- ions?

A) K₂CO₃
B) KCO₃
C) K(CO₃)₂
D) K₃(CO₃)₂

Question 34

What is the formula for the ionic compound which forms when Co³⁺ combines with SO₄^2-?

A) CoSO₄
B) Co₂(SO₄)₃
C) Co(SO₄)₂
D) Co₃(SO₄)₂

Question 35

For which of the following pairs of elements would "electron transfer" between atoms most likely occur?

A) Na and Cd
B) Ca and O
C) As and I
D) V and Li

Question 36

Which of the following pairs of elements would most likely form a polar covalent bond?

A) Se and Cl
B) Si and C
C) K and He
D) Ba and Ag

Question 37

Which of the following is the correct Lewis structure for OF₂?

A)
B)
C)
D)

Question 38

The total number of "shared electron pairs" in the molecule H₂S is ________.

A) 1
B) 2
C) 3
D) 4

Question 39

Indicate the total number of electrons which would be shown as "dots" in a correctly written Lewis structure for OF₂.

A) 18
B) 32
C) 26
D) 20

Question 40

Which of the following molecules contains a triple covalent bond?

A) Br₂
B) C₂H₂Cl₂
C) SO₂
D) HCN

Question 41

Which of the following general statements concerning covalent bond characteristics is incorrect?

A) Triple bonds are stronger than double bonds.
B) Double bonds are stronger than single bonds.
C) Double bonding can occur with Group VII A elements.
D) Triple bonding is possible when 3 or more electrons are needed to complete an octet.

Question 42

When drawing a Lewis structure, pairs of electrons that are not between atoms but are used to fill the octet of an atom are called ________.

A) bonding pairs
B) lone pairs
C) filled shells
D) excess electrons

Question 43

Which bonding is not possible for carbon with its 4 valence electrons?

A) 4 single bonds
B) 2 single bonds and 1 double bond
C) 1 single bond and 1 triple bond
D) 1 double bond and 1 triple bond

Question 44

One of the resonance structures for the polyatomic ion NO₃^- is:

How many other resonance structures are there for this ion?

A) 1
B) 2
C) 3
D) 4

Question 45

The following represents one of the resonance structures for the nitrite ion, NO₂^-.

How many additional resonance structures can be drawn for NO₂^-?

A) 0
B) 1
C) 2
D) 3

Question 46

How many resonance forms can be drawn for the CO₃^-2 ion?

A) 0
B) 1
C) 2
D) 3

Question 47

The Lewis structure for the SO₄^2- ion contains how many "bonding electrons"?

A) 2
B) 4
C) 8
D) 12

Question 48

In the Lewis structure of HCN, how many nonbonded electron pairs are present?

A) 3
B) 4
C) 2
D) 1

Question 49

In the Lewis structure, X represents a period 3 nonmetal. Identify the nonmetal.

A) aluminum
B) sulfur
C) chlorine
D) nitrogen

Question 50

Calculate the total number of electrons in the Lewis structure for the PH₄⁺ ion.

A) 9
B) 8
C) 10
D) 12

Question 51

Calculate the total number of electrons in the Lewis structure for the C₂H₃O₂^- ion.

A) 25
B) 32
C) 28
D) 24

Question 52

The geometry associated with three pairs of bonded electrons and one pair of nonbonded electrons about a central atom in a molecule is ________.

A) tetrahedral
B) trigonal pyramidal
C) trigonal planar
D) angular

Question 53

The geometry of a molecule in which the central atom has 2 bonding electron pairs and 2 nonbonded electron pairs is ________.

A) linear
B) angular
C) trigonal planar
D) trigonal pyramidal

Question 54

The molecular shape (geometry) of a Cl₂CO molecule is ________.

A) linear
B) trigonal pyramidal
C) trigonal planar
D) tetrahedral

Question 55

The molecular shape (geometry) of a NCl₃ molecule is ________.

A) angular
B) trigonal planar
C) tetrahedral
D) trigonal pyramidal

Question 56

Which one of the following molecules is tetrahedral in shape?

A) XeF₄
B) CF₄
C) BF₃
D) NH₃

Question 57

What is the molecular geometry of CO₂?

A) linear
B) trigonal planar
C) tetrahedral
D) angular

Question 58

The ability of an atom to attract electrons to itself in a molecule is called ________.

A) electron affinity
B) electronegativity
C) ionization energy
D) paramagnetism

Question 59

Which of the following sets of elements is arranged in order of increasing electronegativity?

A) Cl, S, Se, Te
B) F, B, O, Li
C) Br, Cl, S, P
D) Fr, Mg, Si, F

Question 60

Which statement about electronegativity is incorrect?

A) Fluorine is the most electronegative atom of all the elements.
B) Metals generally have higher electronegativity values than nonmetals.
C) Within a periodic table row, electronegativity increases from left to right.
D) Within a periodic table group, electronegativity increases from bottom to top.

Question 61

Which atom is the most electronegative?

A) Li
B) Cs
C) P
D) As

Question 62

Which atom is the least electronegative?

A) F
B) Si
C) Rb
D) Ca

Question 63

If the electronegativity difference between two elements X and Y is 0.2, the bond between the two elements would be ________.

A) ionic
B) nonpolar covalent
C) polar covalent
D) coordinate covalent

Question 64

Which of the following diatomic molecules contains the bond of greatest polarity?

A) P₄
B) Cl-F
C) BrI
D) Te-F

Question 65

Which of the following is the best notation for the bonding in the formula unit NaF?

A) ^{+ 11eec96d_5bf8_46d2_b236_e5ca71510896_TB10281_11-}
Na-F
B) ^{11eec96d_5bf8_46d2_b236_e5ca71510896_TB10281_11- 11eec96d_5bf8_46d2_b236_e5ca71510896_TB10281_11+}
Na-F
C) Na-F
D) Na⁺ F^-

Question 66

Which bond has the greatest percent covalent character?

A) O - F
B) Be - N
C) Cu - N
D) Li - Cl

Question 67

For which of the bonds is the direction of polarity incorrect?

A) Bond I
B) Bond II
C) Bond III
D) Bond IV

Question 68

Which of the following bonds is the most polar?

A) As-Cl
B) N-F
C) I-Br
D) O-Si

Question 69

Which of the following is a nonpolar molecule containing polar bonds?

A) H - H
B) CH₄
C) F - Be - F
D) It is not possible for a molecule to be nonpolar while containing polar bonds.

Question 70

Which of the following statements concerning molecular polarity is incorrect?

A) All A-B molecules are polar.
B) All linear X-A-X molecules are nonpolar.
C) All angular A-B-C molecules are nonpolar.
D) All symmetrical AX₄ molecules are nonpolar.

Question 71

Which molecule is not a polar molecule?

A) HCN
B) CHCl₃
C) NH₃
D) BCl₃

Question 72

Which of the following molecules is polar?

A) BeCl₂
B) BF₃
C) CBr₄
D) NCl₃

Question 73

How many valence electrons do atoms with the following electron configurations have?
-1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴

Question 74

How many valence electrons do atoms with the following electron configurations have?
-1s²2s²2p⁶3s²

Question 75

How many valence electrons do atoms with the following electron configurations have?
-1s²2s²2p⁶3s²3p⁶4s¹

Question 76

How many valence electrons do atoms with the following electron configurations have?
-1s²2s²2p⁵

Question 77

Determine the formula for the compound formed between the following pairs of elements and/or ions.
-Cs and P₄

Question 78

Determine the formula for the compound formed between the following pairs of elements and/or ions.
-As and Cl₂

Question 79

Determine the formula for the compound formed between the following pairs of elements and/or ions.
-OH⁻ and Fe³⁺

Question 80

Determine the formula for the compound formed between the following pairs of elements and/or ions.
-O₂ and F₂