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WorksheetsChemistry Study Quiz
Total questions: 131
Worksheet time: 1hrs 25mins
All compounds containing carbon are organic compounds.
False
True
One of the following statements about the molecule shown below is incorrect:
CH3CH2CH2OCH2COOH
the molecule contains four oxygens
the molecule contains five carbons
the molecule contains eighteen atoms
the molecule contains ten hydrogens
If there is no subscript below a symbol, that means there is only one of that element being represented.
True
False
A monatomic anion is an atom with a -2 charge.
False
True
The Stock system is only used for cations.
True
False
A binary ionic compound
contains two types of atoms
can be a compound made of two nonmetals
can be a compound made of two metals
contains atoms combined in ratios of two
The overall charge of a binary ionic compound can vary.
False
True
The proper formula for potassium oxide is
K2O
KO
K2O3
KO2
The correct name for the CN- ion is
cyanide
cyanosis
cyanic
cyanate
The CO32− ion is known as the bicarbonate ion.
False
True
KBr
(a)
Na2S
(a)
CoCl2
(a)
copper(II) oxide
(a)
iron(III) bromate
(a)
Carbon dioxide consists of a central carbon atom bonded to two oxygen atoms.
True
False
Water is an ionic compound.
False
True
Binary molecular compounds are usually composed of
two nonmetals
three or more different elements
two metals
a metal and a non-metal
The nonmetal ___ would follow S when writing binary compound formulas
I
P
C
H
P2O5 is named phosphorus pentaoxide.
False
True
N and O can combine with each other in a variety of ratios.
True
False
CCl4 is the formula for carbon trichloride.
False
True
N2O5
(a)
SiO2
(a)
The formula for xenon hexachloride is
XeCl6
XeCl4
XeCl5
XeCl8
Boron trihydride has the following formula
BH3
B3H6
B2H6
B2H3
The formula for dinitrogen tetroxide is N2O2
False
True
arsenic triiodide
(a)
disilicon tetroxide
(a)
diboron hexahydride.
(a)
An acid produces ______ when dissolved in water.
hydrogen ions
hydroxide ions
OH+
electrons
What is the name for the PO3-4 ion?
phosphate
phosphite
phosphoric
phosphorous
HNO3
(a)
HMnO4
(a)
HClO3
(a)
If the anion ends in ite, the acid name ends in ______.
ous acid
ite acid
ate acid
ic acid
phosphoric acid
(a)
nitrous acid
(a)
hydroiodic acid
(a)
chlorous acid
(a)
The names of all bases end in
hydroxide
hydroxyl
hydride
hydronium
OH+ is the hydroxide ion.
False
True
Cu(OH)2
(a)
iron(II) hydroxide
(a)
lead(IV) hydroxide
(a)
The number of valence electrons for p-block elements is
group number minus 10
group number minus 12
group number minus 8
group number minus 6
The number of valence electrons for carbon is three.
False
True
Atoms of _____ elements tend to lose valence electrons to satisfy the octet rule.
metals
noble gases
halogens
gases
All elements obtain eight valence electrons, either by electron loss or electron gain.
False
True
Cations are formed when
atoms lose one or more electron
atoms add one electron
atoms lose all their electrons
atoms add electrons to fill the valence level
Beryllium can achieve a complete outermost principal energy level by losing four electrons.
False
True
carbon 4+
(a)
magnesium 2+
(a)
chlorine 1-
(a)
oxygen 2-
(a)
manganese 2+
(a)
Na+ and Cl- are isoelectronic.
False
True
The pseudo noble gas electron configuration for some transition elements has ____ electrons in the outermost principal energy level.
18
8
10
12
Zinc and copper ions have full d sublevels.
True
False
Scandium achieves a noble gas electron configuration by losing its two 4s electrons.
False
True
The strength of an ionic bond is directly dependent on
the magnitude of the charges
the size of the ion
the ionic polarities
the distance between the ions
A larger ion will form a stronger bond than a smaller ion.
False
True
The chlorine atom gains one electron to become an anion.
True
False
The formula unit for an ionic compound is
an empirical formula
a molecular formula
a diagram of the crystal structure
an indication of the number of individual ions in the crystal
The coordination number for an ionic compound is
the number of ions immediately surrounding an ion of opposite charge
the number of ions in the molecule
the number of ions in the crystal
the number of ions immediately surrounding an ion of like charge
Cs and Na have different coordination numbers because
the ion sizes are very different
the ionic charges are different
the chloride ion changes shape in contact with the two cations
solubilities of the two compounds are different
One formula unit of FeCl3 contains three Cl- for every Fe3+.
True
False
Coordination numbers are determined by ionic combinations.
True
False
All Group 1 cations will have the same packing arrangement.
False
True
High melting points of ionic compounds are due to
the presence of many ionic bonds
mixtures of metals in the crystals
the ordered crystal structure
various shapes of the crystals
Addition of NaCl to distilled water
causes conduction of an electrical current
generated electricity
increases negative ion movement
decreases the electrical conductivity
Ionic crystals break when struck because
ions of like charge are forced closer together and repel one another
the hammer forces all the ions together
ions of opposite charge set up an electrical current
a chemical reaction is initiated due to the pressure of the hammer
Distilled water can conduct an electric current.
False
True
What color is the mineral Azurite, Cu3(CO3)2(OH)2?
(a)
Solid NaCl at room temperature will conduct electricity
False
True
The points in a metal crystal lattice are occupied by
metal atoms
anions
cations
metal array
Electrons moving through the empty orbitals of the metal are called
delocalized
displaced
mobile
degenerate
All the atoms in a metallic crystal are identical.
True
False
In a metal, the positive ions migrate from one place to another.
False
True
Luster of a metal is due to electrons emitting light when they move to higher energy levels.
False
True
Ionic crystals are brittle because
like charges come too close together under force
electron flow increases under force
ionic bonds are weak
ions separate further under force
The malleability of a metal is due to
electrons blocking contact between adjacent cations
positive ions repelling one another
attraction between cations and anions
negative electrons repelling one another
Metals are malleable because the cations can move
False
True
__________ is the most efficient way to pack spherical objects
closest packing
hexagonal packing
linear packing
body-centered packing
One of the following is not a metallic crystal structure
hexagonal faced
cubic face centered
hexagonal
cubic body centered
The purpose for packing is to minimize empty space between atoms.
True
False
Bronze is an alloy of
copper and tin
tin and gold
copper and zinc
tin and aluminum
One of the following is not a constituent of steel
magnesium
molybdenum
carbon
manganese
The major constituent of steel is iron.
True
False
What would be a benefit of incorporating a small atom like carbon into the crystal structure of iron metal?
Defense between iron cations is enhanced, reducing the likelihood that iron atoms will repel each other and cause structural defects.
Interstitial alloy forms when smaller atoms such as carbon fit in between the larger atoms in the crystal packing arrangement increasing their strength, hardness, and resistance to corrosion.
One of the following is not a covalent compound
MgBr2
H2O
NH3
CO2
A covalent bond occurs when
two atoms share electrons
an atom donates an electron to another atom
two atoms donate electrons
two atoms lose an electron
A lower potential energy indicates a more stable system.
True
False
A covalent bond forms when
two singly occupied orbitals overlap
two pairs of electrons are shared
two full orbitals overlap
two electrons of the same spin overlap
A lone pair is a pair of electrons that are
not shared between atoms
shared more with one atom than the other
shared equally between two atoms
alternate between one atom and another
A double covalent bond is a bond shared between two pairs of atoms.
False
True
In a coordinate covalent bond
one atom provides both electrons
the electrons alternate between the two atoms
no electrons are shared
a double set of electrons are shared
A polyatomic ion
is a group of covalently bonded atoms with an overall charge
has more than one electrical charge
is a group of ions held together by an electrical charge
is a group of covalently bonded atoms with a distributed charge
One of the following is not a polyatomic ion
O2-
SO2-3
SO2-4
NH+4
A resonance structure
gives a partial idea of the actual structure
shows multiple electrons on the same compound
represents electron shifts among atoms
violates the octet rule
A “half-bond” in a resonance structure is shown by a dotted line.
True
False
One of the following is not an exception to the octet rule.
even-electron molecules
odd-electron molecules
incomplete octet
expanded octet
The d sublevel becomes important in covalent bonds for elements of the third period and beyond.
True
False
Which one of the following has the highest bond energy?
C=C
C-H
Cl-Cl
H-H
Why does aluminum not form complete octets of valence electrons when forming covalent compounds?
Aluminum has three valence electrons so it can only form three covalent bonds. When bonded with three other elements the compound will only have six valence electrons - not an octet. There have been stable compounds of aluminum with six valence electrons.
It is an ionic compound. Aluminum is a metallic with 3 valence electrons and coffee electron attraction. To acquire a solid octet, those valence electrons need to be lost (the preceding electricity stage has eight electrons).
Valence bond electrons are shown in Lewis structures.
True
False
PCl5 contains three Cl atoms with an ________ orientation.
equatorial
equilateral
equidistant
equimetric
Dotted line bonds project out of the page.
False
True
An octahedral shape would have seven sides.
False
True
Name the following VSEPR shape around the central atom
phosphorus
trigonal bipyramidal
trigonal bipyramidal
Name the following VSEPR shape around the central atom
Carbon
tetrahedral
tetrahedral
Name the following VSEPR shape around the central atom
octahedral
Cobalt
octahedral
Lone pair electrons are ______ repulsive than bonding pair electrons.
slightly more
much more
much less
slightly less
A distorted tetrahedron configuration is seen in the _______ molecule.
SF4
ClF3
Cl2F5
SF5
The H-O-H bond angle is 104.5°.
True
False
The ammonia molecule contains two lone pairs.
False
True
Use the diagram below to explain how the lone pair electrons influence the shape of the water molecule.
The two sets of lone pair electrons repel each other and also repel the H atoms.<In addition, the two H atoms repel each other.
The lone pair electrons make the shape a little more oddly shaped because the two are alone not with another like electron from another like atom.
Lone pair electrons use ______ than bonding pair electrons
more space
less space
variable space
the same amount of space
Lone pairs on the central atom are not considered in determining geometry.
False
True
The bromine pentafluoride molecule has a central bromine atom, five single bonds to fluorine atoms, and one lone pair.The six groups of electrons around the central atom give it an octahedral domain geometry:
If a fluorine is remove, it would form BrF4- with an expected molecular geometry in the form of AB4E2. What is this molecular geometry called?
Square Planar
BrF4- would most likely be square planar.<> Each F atom would repel all the others equally. There would now be two lone pairs repelling also. This means that the central atom will have a AB4E2 shape.
A non-polar covalent bond involves
equal sharing of electrons
unpaired electrons in orbitals
balanced charge distribution in the bond
strong attraction of electrons by one atom
The Greek letter δ represents
partial charge
change in state
partial bond energy
rate of reaction
The C-O bond is
polar covalent
partially covalent
mostly ionic
mostly covalent
Arrange the following bonds in terms of increasing polarity, beginning with the lowest polarity (Show the ∆EN calculation for each for full marks) (2 Marks) :a) Pb-Ib) Si-Clc) Al-Cld) Cu-Bre) O-P
(lowest) Pb-I, Cu-Br, O-P, Si-Cl, Al-Cl (highest) a, d, e, b, cPb-I ∆EN = 2.66 - 2.33 = 0.33Cu-Br ∆EN = 2.96 - 1.90 = 1.06>>O-P ∆EN = 3.44 - 2.19 = 1.25Si-Cl ∆EN = 3.16 - 1.90 = 1.26Al-Cl ∆EN = 3.16 - 1.61 = 1.55
a) 2.5-1.9=.6
b) 3.0-1.8=1.2
c) 3.0-1.5=1.5
d) 2.8-1.9=.9
e) 3.5-2.1=1.4
Answer: a) PB-I, d) Cu-Br, b) Si-Cl, e) O-P, c) Al-Cl
A dipole has
two poles
two like charges
two diffuse charges
two negative poles
Why is BF3 non-polar?
BF3 is nonpolar in nature due to the fact it's far exceptionally symmetric in shape. Vector sum of the dipole moments of 3 polar bonds of every B-F bond is 0 due to the trigonal planar shape of boron trifluoride.
The three dipoles all lie in the same plane and cancel each other out.
What would be the effect on the polarity of the molecule formed when CCl4 has one Cl replaced by an H? Explain why.
Answer: Polarized.
Description: See the photograph below. I understand it sucks, however allow me explain: ΔE is electronegativity. The better the ΔE of a substance, the greater electrons it is able to attract. Cl has better electronegativity than C and H. But of direction there's some other Cl with the identical amount. Therefore, if we've a tetrahedral spatial configuration as withinside the left figure, all Cl cancel different electrostatic forces. However, changing Cl with H offers a dipole second pointing to Cl going through hydrogen as the suitable pull. The look of the ensuing dipole suggests the presence of polar compounds.
CCl4 is non-polar because all four dipoles are equal and cancel each other.Introduction of a H would give<rise to three identical dipoles that are not aligned in such a way to cancel each other so it would become polar.
London dispersion forces
are due to random motions of electrons
are due to random motions of molecules
are seen between polar atoms
are a result of differing electronegativities between two atoms
Dispersion forces are a form of van der Waals interactions.
True
False
Why would London dispersion forces be so weak?
London dispersion forces are intermolecular forces that occur between all atoms and molecules due to the random motion of electrons. This forms a weak and temporary dipole. They are fluctuating at all times and do not exist in a static form,>so they are not permanent.
Electrons in adjacent molecules "run away" when they repel each other, thus redistributing the electron density of one molecule in the vicinity of another.
At room temperature, molecular compounds can be solid, liquid, or gas.
True
False
