Deck 4: Forces Between Particles

Question 1

When an ionic compound forms between sodium (Na)and bromine (Br)atoms, it is true that

A)a bromine atom donates an electron to a sodium atom.
B)both the bromine atoms and sodium atoms donate electrons to each other.
C)a sodium atom donates an electron to a bromine atom.
D)neither bromine nor sodium atoms donate electrons to each other.

Answer 1

a sodium atom donates an electron to a bromine atom.

Question 2

Which of the following has a noble gas electronic configuration?

A)Cl
B)O ⁻
C)Br ⁻
D)Cl⁺

Answer 2

Br ⁻

Question 3

The ionic compound that forms between magnesium (Mg)and oxygen (O)has the formula _____ .

A)Mg₂O
B)MgO
C)MgO₂
D)Mg₂O₃

Answer 3

MgO

Question 4

A correct Lewis structure for BrCl is _____ .

A)
B)
C)
D)

Question 5

Which of the following statements is correct with reference to covalent bonding?

A)Covalent bonds only form between like atoms.
B)The nonpolar covalent bond is the reason for hydrogen bonding.
C)Polyatomic compounds contain only covalent bonds.
D)None of these is a correct statement.

Question 6

Which of the following pairs of elements is most likely to form a covalent bond?

A)Fe H
B)Cs Br
C)Cl O
D)Zn S

Question 7

Which of the following electronic changes will cause a Group VA (15)element to achieve a noble gas configuration?

A)gain three electrons
B)gain two electrons
C)gain one electron
D)lose three electrons

Question 8

When magnesium forms an ion, it would be represented as _____ .

A)Mg ⁻
B)Mg^{2 −}
C)Mg⁺
D)Mg²⁺

Question 9

Which of the following would cause a calcium atom (Ca)to achieve a noble gas configuration?

A)lose one electron
B)lose two electrons
C)gain one electron
D)gain two electrons

Question 10

For some representative metals, two possible ions can be formed. Why?

A)s electrons can fill the next lower d orbital.
B)They can lose electrons to form a cation and gain electrons to form an anion.
C)They can lose the s electrons or all electrons in their outer shell.
D)They can lose just the p electrons or all electrons in their outer shell.

Question 11

If the electronegativity difference between A and B is 0.8, what type of bond is formed between the two elements?

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

Question 12

Some elements can display more than one charge. The most stable charge is

A)due to having 6 electrons in the outside orbit.
B)that charge produced by a loss of electrons, not a gain of electrons.
C)the charge produced by the noble gas configuration.
D)All are correct.

Question 13

The correct name for CeS is _____ .

A)cesium sulfate
B)cesium sulfide
C)cerium sulfate
D)cerium sulfide

Question 14

Which of the following is the correct Lewis structure for C₂H₄?

A)
B)
C)
D)

Question 15

The rigid three-dimensional arrangement assumed by the ions of ionic compounds is called a

A)molecule.
B)binary compound.
C)lattice site.
D)crystal lattice.

Question 16

Which of the following is a correct Lewis structure for a group IIIA(13)element M?

A)
B)
C)
D)

Question 17

Which of the following has the highest electronegativity?

A)O
B)N
C)Si
D)P

Question 18

Which of the following distinguishing electron configurations is characteristic of noble gases?

A)n f ¹⁴
B)n d ¹⁰
C)n p ⁶
D)n s ²

Question 19

A covalent bond results when

A)one atom gives up an electron to another atom.
B)one atom gives up two electrons to another atom.
C)two atoms share a pair of electrons.
D)two atoms share a single electron.

Question 20

Which of the following would you expect to be the most polar molecule?

A)CO₂
B)H₂S
C)KCl
D)SiH₄

Question 21

The correct name for BaCO₃ is _____ .

A)barium trioxide
B)barium monocarbon trioxide
C)barium carbonate
D)barium monocarbonate

Question 22

The correct formula for the ionic compound containing Al³⁺ and PO would be _____.

A)Al₃(PO₄)₃
B)AlPO₄
C)Al₃(PO₄)₂
D)Al₂(PO₄)₃

Question 23

The molecular structure of water should be

A)linear because of the electron configuration of the oxygen atom.
B)flat triangular because water contains 3 atoms.
C)bent because of the unshared electrons on the molecule.
D)undetermined as there is no way to predict the shape of the water molecule.

Question 24

The shape of a BF₃ molecule is _____ .

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

Question 25

Which of the following covalent molecules contains polar bonds?

A)
B)
C)
D)more than one response is correct

Question 26

Which of the following correctly illustrates hydrogen bonding in water?

A)
B)
C)
D)

Question 27

The correct name for K₂SO₄ is _____ .

A)potassium sulfate
B)potassium sulfide
C)potassium sulfite
D)potassium tetrasulfoxygen

Question 28

Which of the following is the polyatomic ion call carbonate?

A)C₂Cl^{2 −}
B)ClO ⁻
C)CO
D)HCO

Question 29

The correct formula of an ionic compound containing Fe²⁺ and ClO is _____ .

A)FeClO₄
B)Fe₂(ClO₄)₃
C)Fe(ClO₄)₂
D)Fe₃(ClO₄)₂

Question 30

What single condition is required to insure that a molecule will be polar covalent?

A)a bond between like atoms
B)a bond between atoms that are different in electronegativity
C)a bond between atoms that are of widely different atomic weights
D)none of the choices

Question 31

Which of the following would be a polar molecule?

A)O₂
B)HCl
C)CH₄
D)F₂

Question 32

The correct formula for ammonium sulfate is _____ .

A)NH₄SO₄
B)(NH₄)₂SO₄
C)NH₄(SO₄)₂
D)(NH₄)₂(SO₄)₃

Question 33

The correct name for KHPO₄ is _____ .

A)potassium phosphate
B)monopotassium phosphate
C)potassium hydrogen phosphate
D)KHPO₄ is not a compound

Question 34

Which interparticle forces would you expect to find in a sample of the element lithium?

A)covalent
B)dispersion
C)ionic
D)metallic

Question 35

Hydrogen bonds form between the molecules of the hypothetical compound ABCH and do not form between DEFH molecules.

A)ABCH has a higher molecular weight than DEFH.
B)ABCH represents a compound that contains O, N, or F directly bonded to H.
C)ABCH tends to be a compound with color, but DEFH does not have color.
D)There is no significant difference between ABCH and DEFH.

Question 36

Which of the following molecular geometries would most likely give rise to a nonpolar compound?

A)
B)
C)
D)

Question 37

In describing the strength of interparticle forces, we discover that the weakest forces of bonds are _____ .

A)covalent
B)metallic
C)dipolar
D)dispersion

Question 38

The correct name for the covalent compound N₂O₄ is _____ .

A)dinitrogen tetroxide
B)nitrogen oxide
C)nitrogen quartoxide
D)dinitrogen quartoxide

Question 39

A polar molecule must have

A)polar bonds.
B)an unsymmetrical arrangement.
C)neither polar bonds nor an unsymmetrical arrangement.
D)both polar bonds and an unsymmetrical arrangement.

Question 40

Which type of interparticle forces leads to compounds with the lowest melting points?

A)covalent
B)dispersion
C)ionic
D)dipole-dipole

Question 41

The most common positive ion in human fluids is _____ .

A)Cl ⁻
B)PO
C)Na⁺
D)Fe²⁺

Question 42

What is the formula mass of the compound formed between Al³⁺ and Cl^-?

A)187.5 u
B)62.5 u
C)116.5 u
D)133.5 u

Question 43

NH₃ (ammonia)exhibits what type of structure?

A)triangle
B)pyramid with square base
C)pyramid with triangular base
D)none of these

Question 44

Which is the correct name for UF₆?

A)uranyl fluoride
B)uranium hexafluoride
C)uranium (VI)fluoride
D)uranium (IV)fluoride

Question 45

In what part of the human body is nitric oxide, NO, produced?

A)the brain
B)the heart
C)blood vessels
D)the skin

Question 46

Arrange the following bonds in order of increasing bond polarity.

A)C–O < P–O < Cl–O
B)Cl–O < C–O < P–O
C)P–O < Cl–O < C–O
D)C–O < Cl–O < P–O

Question 47

Atoms or ions are considered isoelectronic if

A)they have similar electron configurations.
B)they have different number of electrons.
C)they have the same number of protons.
D)None of the choices.

Question 48

Which of the following reactions would not produce an octet of electrons in the ion product?

A)
B)
C)
D)

Question 49

The anion in an ionic compound whose name ends in "-ide" is

A)always a simple ion.
B)always a polyatomic ion.
C)either a simple or polyatomic ion.
D)a positive charge.

Question 50

Which of the following correctly represents the polarity of the bond?

A)
B)
C)
D)

Question 51

The lattice site in a crystal is

A)the general location of all particles in a crystal.
B)the individual location occupied by a particle.
C)the rigid three-dimensional arrangement of particles.
D)None of the choices.

Question 52

Which of the following Lewis structures depicts provides a reasonable representation of SO₂?

A)
B)
C)
D)

Question 53

Which pair of elements will be further apart in electronegativity?

A)Cl and F
B)Li and Cl
C)Mn and Se
D)U and Cs

Question 54

Consider the following geometric shapes.  Which one is a tetrahedral?

A)
B)
C)
D)

Question 55

Which of the following metals would not use a Roman Numeral as part of its name in a compound?

A)Cr
B)Mn
C)Co
D)Ca

Question 56

During the formation of an ionic bond between Na and N, which of the following reactions occurs?

A)
B)
C)
D)

Question 57

How many moles of K⁺ and P^3- ions are present in 2.00 moles of K₃P?

A)6.00 mol K⁺ and  2.00 mol P^3-
B)3.00 mol K⁺ and  1.00 mol P^3-
C)1.00 mol K⁺ and  3.00 mol P^3-
D)2.00 mol K⁺ and  6.00 mol P^3-

Question 58

What medicinal value does ZnO have?

A)sun screen
B)relieves diaper rash
C)relieves poison ivy
D)all of these

Question 59

What would be the proper name for the following binary ionic compound CaBr₂?

A)calcium dibromine
B)monocalcium bromine
C)monocalcium dibromide
D)calcium bromide

Question 60

Which of the following molecules would be classified as polar covalent?

A)NaCl
B)CH₃Cl
C)KCl
D)CaCl₂

Question 61

K⁺ and Cl ⁻ have the same electronic configuration as argon.

Question 62

Ammonia is a planar trigonal molecule.

Question 63

Metals gain electrons to become ions in ionic compounds.

Question 64

The outer shell of a noble gas always contains eight electrons.

Question 65

Fe²⁺ and Fe³⁺ are isoelectronic.

Question 66

Both bonding and non-bonding electron pairs can influence molecular shape.

Question 67

Oxygen must gain two electrons to achieve a noble gas configuration.

Question 68

Na⁺ and F ⁻ are isoelectronic.

Question 69

None of the noble gases make compounds.

Question 70

Which of the following would be considered as a rare earth?

A)cerium
B)cesium
C)curium
D)cadmium

Question 71

Only compounds containing hydrogen attached to an oxygen, nitrogen, or fluoride atom can exhibit hydrogen bonding.

Question 72

H₂O is a binary compound.

Question 73

CCl₄ has a tetrahedral structure.

Question 74

Carbon dioxide is a linear molecule.

Question 75

Eating foods rich in _____ has been shown to help reduce hypertension.

A)chloride
B)iron
C)sodium
D)potassium

Question 76

Dispersion forces are among the strongest interparticle forces.

Question 77

Nitrogen is more electronegative than oxygen.

Question 78

The water molecule has a bent structure.

Question 79

Knowing that indium is a member of group IIIA (13)and selenium is listed under group VIA (16), which of the following compounds should result from a reaction between these two elements?

A)InSe
B)In₂Se₃
C)In₅Se₃
D)Se₅In₃

Question 80

HCl and HBr can exhibit hydrogen bonding with each other.