why is the boiling point of HF so much higher than that of HCl?

HF experiences hydrogen bonding

Which gas has the higher boiling point and why?

Neon because it has more electrons

have stable electron configurations

When drawing Lewis structures, some atoms may need to _______ in order to satisfy the octet rule.

share one or more pairs of electrons

What does VSEPR mean?

Outer electrons repel to move bonded atoms far away

Which of these two substances will have a higher boiling point?

Ethanol- it has hydrogen bonding

Ionic Bonds form because

one atom gives an electron to the other

What does VSEPR stand for?

Valence Shell Electron Pair Repulsion

determines the polarity of a polar bond

difference in electronegativity

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CHEMISTRY BJU Final Study Guide #3

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CH.7 BJU Chemistry : A #chemistry quiz to review #chemical bonds and #molecular #geometry BJU CH.6 Chemistry: BJU Chemistry 4th Edition Chapter 6 Chemical Bonding

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Questions 96

Answers

1
The attraction between opposite electrical charges is called
electron affinity.
ionization forces.
electronegativity.
electrostatic force.
2
number of electrons if there is a full s and a full p sublevel
2
10
8
6
3
diatomic molecules
bent polar
linear nonpolar
linear polar
bent nonpolar
4
why is the boiling point of HF so much higher than that of HCl?
HCl is a stronger acid
HCl experiences hydrogen bonding
Fluorine is lighter than chlorine
HF experiences hydrogen bonding
5
according to the VSEPR theory, what is the shape of a two-atom molecule
linear, bent, or pyramidal
always bent
linear or bent
always linear
6
Rank the boiling points from lowest to highest: N₂, O₂, NO
N2 > O2> NO
NO > O2 > N2
O2 > NO > N2
NO > N2 > O2
7
molecule that has more than an octet of electrons around the central atom
CH3Cl
CF6
H2O
NF4
8
The predominant type of bonding involved in Li₂O is
ionic
covalent
metallic
9
Shape of CF₂Cl₂
tetrahedral
pyramidal
trigonal planar
bent
10
Metallic bonding is characterized by a loose transfer of electrons between 2 atoms.
True
False
11
Shape of HCN
bent
linear
pyramidal
trigonal planar
12
Which gas has the higher boiling point and why?
Hydrogen because it can form hydrogen bonds
Hydrogen because it has a lower mass
Neon because it is a noble gas
Neon because it has more electrons
13
Molecules with higher boiling points will generally have ____ .
fewer atoms
dispersion forces
weaker intermolecular forces
stronger intermolecular forces
14
polar compound
CH4
CO2
Br2
NH3
15
Which of the following substances contains both ionic and covalent bonds?
ICl
NaOH
NH3
CH4
16
theory that states that the molecular shapes are largely determined by repulsion of electrons
VSEPR
MO
valence bond
electron sea
17
The symbols ς+ and ς- indicates
electron affinity.
partial charge.
electronegativity.
change.
18
Atoms with fewer than 4 valence electrons tend to gain electrons when bonding.
False
True
19
Noble gases
never form bonds.
bond readily with other Nobel gases.
have stable electron configurations
bond readily with other atoms
20
A full valence shell that allows atoms to maximize stability is known as
the triad rule.
Pauling's electronegativity rule.
the second law of thermodynamics.
the octet rule
21
Molecular compounds tend to have __ melting and boiling points than ionic compounds.
none of the above
the same
higher
lower
22
When drawing Lewis structures, some atoms may need to _______ in order to satisfy the octet rule.
share one or more pairs of electrons
share one or more pairs of protons.
gain one or more pairs of electrons
give up one or more pairs of electrons
23
According to VSEPR, three-atom molecules are
linear or bent
bent or pyramidal
always bent
linear or pyramidal
24
element that can be a central atom and hold less than 8 valence electrons
bromine
beryllium
bohrium
boron
25
When atoms bond, they will seek a lower, more stable energy state.
False
True
26
Shape of CH₂O
trigonal planar
linear
pyramidal
bent
27
Except for the transition and inner transition metals, the octet rule applies to all other elements.
False
True
28
δ- and δ+
partial charge
partial polarity
partial bond
partial orbital
29
What does VSEPR mean?
inner electrons repel to move the nucleus away
outer electrons bond with atoms
outer electrons share electrons
Outer electrons repel to move bonded atoms far away
30
The predominant type of bonding in CF₄ is
metallic
ionic
covalent
31
The luster or shine seen on most metals is thought to be caused by the movement of
electrons
gluons
protons
neutrons
32
Which of these two substances will have a higher boiling point?
Ethanol- it has hydrogen bonding
Dimethyl ether- it has dipole-dipole forces
33
Ionic compounds are bonds between
2 nonmetals
2 Metalloids
Metal and Nonmetal
2 metals
34
A mixture of atoms of a metal with another element where he mixtures has metallic properties is called a(n)
formula unit.
alloy.
polyatomic ion.
35
The mobile valence electrons in a metallic bond are said to be
locked in.
crystallized.
localized.
delocalized.
36
The orderly arrangement of ions in a three-dimensional pattern within a compound is called a(n)
crystal lattice
ion array
ionic network
formula unit
37
The compound most likely to be ionic is...
KF
CO2
ICl
CCl4
38
Metals
gain electrons
share electrons
lose electrons
39
What is the molecular geometry of XeF₄?
Square Planar
Trigonal Bipyramidal
Bent
Seesaw
40
The predominant type of bonding involved in Au is
ionic
covalent
metallic
41
Ionic Bonds form because
both atoms gain electrons
one atom gives an electron to the other
both atoms lose electrons
they share electrons, and sharing is caring
42
What does VSEPR stand for?
Valence Shell Electron Pair Reaction
Valence Shell Electron Pair Reponse
Valence Shell Electromagnetic Pair Reaction
Valence Shell Electron Pair Repulsion
43
A dash in a Lewis structure represents
three electrons
four electrons
two electrons
one electron
44
The predominant type of bonding in the electron-sea theory is
metallic
covalent
ionic
45
Atoms with a maximum electronegativity difference of what, form non-polar covalent bonds?
1.4
1.7
0.4
0.04
46
strongest bond
can't tell
double
triple
single
47
determines the polarity of a polar bond
difference in bond types
difference in electronegativity
difference in bond angles
difference in group numbers
48
Why would octane (C₈H₁₈) have a higher boiling point than water?
C
B
A
D
49
covalent bonds are formed when orbitals of different atoms overlap
VSEPR theory
valence bond theory
electron sea theory
MO theory
50
has 1 or more double covalent bonds
IBr
CO2
HCN
N2
51
The smaller the difference in electronegativity between 2 elements, the > the polarity of the resulting in molecule.
False
True
52
shape of PH₃
bent
trigonal planar
pyramidal
linear
53
shape that is always polar
tetrahedral
linear
bent (109.5°)
trigonal planar
54
Shape of HF
trigonal planar
bent
linear
pyramidal
55
Shape of OCl₂
bent
linear
trigonal planar
pyramidal
56
It is improper to refer to sodium chloride as a molecule.
True
False
57
The octet rule does not apply to
all of these.
the first five elements in the periodic table
inner transition metals
transition metals
58
Ionic bonds have ........... melting and boiling points.
Very High
High
Low
59
Electronegativity is..
Something that affects certain metals
An atom's ability to attract electrons
A Magnetic Pull
A property Unique to Francium
60
The electron-sea theory accounts for all of the following characteristics of metals except
conductivity
brittleness
malleability
luster
61
Define Covalent Bonds:
Bonds in which atoms share valence electrons.
Bonds in which molecules transfer valence electrons.
Bonds in which molecules share valence electrons.
Bonds in which atoms transfer valence electrons.
62
What is the molecular geometry of SbCl₅?
Trigonal Planar
Tetrahedral
Trigonal Bipyramidal
See Saw
63
What does the solubility rule say?
Metallic can dissolve both nonmetal and metal.
Only molecules that are nonpolar can be dissolved.
Like dissolves like.
64
What is the molecular geometry of NH₃?
Bent
Distorted Tetrahedral
Trigonal Pyramidal
T-Shaped
65
Does water (H₂O) or methane (CH₄) have a higher boiling point?
Their boiling points are the same
Water
the horse's name is Friday
Methane
66
Silicates, diamonds, and quartz are examples of
metallic alloys
ionic cr;ystals.
polar covalent molecules.
network covalent substances.
67
trigonal planar molecule
BI3
NH3
PCl3
H2O
68
The predominant type of bonding in the attraction between oppositely charged ions is
ionic
covalent
metallic
69
The predominant type of bonding in RbCl is
metallic
ionic
covalent
70
The predominant type of bonding involved in Fe₃Al is
metallic
ionic
covalent
71
angle of bonds in a pure tetrahedral arrangement
180°
360°
120°
109.5°
72
Shape of O₃
trigonal planar
pyramidal
bent
linear
73
What type of bond would you expect in a compound of oxygen and potassium?
metallic
polar covalent
ionic
covalent
74
Which of the following does not exist as a diatomic molecule?
hydrogen
bromine
oxygen
krypton
75
Which of these is not a property of ionic compounds?
good electrical conductivity in water
high melting point
good heat conductivity
crystals easily split or cleaved
76
The element with the highest electronegativity is ..........
Cesium (Cs)
Astatine (At)
Hydrogen (H)
Fluorine (F)
77
How does VSEPR predict a compounds shape?
The repelling of electron pairs
Location of the electrons
Lewis Dot structures
Imagination
78
has only single covalent bonds
F2CO
Cl2O
SO2
ClCN
79
The measure of an atom's ability to attract electrons to itself in a chemical bond is called
electronegativity
ionization energy
polarity
electron affinity
80
Chemical bonds between atoms involve the rearranging of _____ to maximize stability.
protons
neutrons
electrons
81
The predominant type of bonding involved in I₂ is
ionic
covalent
metallic
82
What type of bond would you expect in a compound of oxygen and potassium?
ionic
polar covalent
covalent
polar covalent
83
The predominant type of bonding in PO₄^- is
covalent
ionic
metallic
84
Polyatomic ions often act as singled charged particles in chemical reactions and solutions and are made up of
three atoms.
two or more atoms.
single ions
85
Which of the following values for ΔEN would represent a bond that is mostly ionic?
2.0
0.9
3.2
2.6
86
The predominant type of bonding involved in electron sharing one or more pairs of electrons is
metallic
ionic
covalent
87
shape of H₂CO
pyramidal
tetrahedral
bent
trigonal planar
88
Atoms link with other atoms to form chemical bonds to
gain energy and lose stability
gain energy and stability.
release energy and gain stability.
release energy and lose stability.
89
Some covalent substances occur as relatively hard, brittle crystals with high melting points, glassy lusters, and
unusual thermal properties.
unusual electrical properties.
unusual lusters.
90
What is the molecular geometry?
Bent
Linear
Trigonal Planar
Tetrahedral
91
The ratio of cations to anions in an ionic compound is expressed in a chemical formula known as a(n)
formula unit.
polyatomic ion
diatomic molecue.
molecule.
92
Ionic compounds are ...
metals
carbonates
crisps
salts
93
The central atom in a Lewis structure is usually the atom
with the most unpaired electrons.
with the greatest electronegativity.
that is a metal.
with the most electrons.
94
bent molecule
OF2
CO2
NH3
Cl2CO
95
An atom becomes more stable by bonding with another atom if the resulting electron configuration is like what group?
noble gases
alkali metals
halogens
metalloids
96
The noble gases have _____________ boiling points.
approximately room temperature
higher than room temperature
varying temperature
lower than room temperature

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