Download 2 - Castle High School

Chem I
Semester 2 Review
1
All of the following are general characteristics of a
substance in the liquid state except
a. definite volume.
c. not easily compressed.
b. able to flow.
d. definite shape.
1
In the chemical reaction iron plus oxygen →iron oxide,
a. iron oxide is a reactant.
b. iron is a reactant.
c. oxygen is a product.
d. iron is a product.
1
• Which term does not fit with the others listed?
• a. solid
c. gas
• b. reactant
d. liquid
1
The chemical symbol for sodium is
a. NA.
c. SO.
b. Na.
d. So.
1
A basketball has more mass than a golf ball because:
a. the basketball takes up more space.
b. the basketball contains more matter.
c. the golf ball contains a different kind of matter.
d. the golf ball has an indefinite composition.
1
A gas is a form of matter that
a. has a definite volume.
b. is generally a liquid or solid at room temperature.
c. takes the shape and volume of its container.
d. is difficult to compress.
1
Homogeneous mixtures
a. are always liquids.
b. consist of two or more phases.
c. have a composition that is fixed.
d. are known as solutions.
1
A compound
a. is a pure substance.
b. has a composition that varies.
c. can be physically separated into its elements.
d. has properties similar to those of its elements.
1
Physical properties of a substance include
a. color and odor.
c. malleability.
b. melting & boiling points.
d. all of the above.
1
When iron and oxygen combine to form iron oxide,
a. a physical change occurs.
b. a change of state occurs.
c. a change in mass occurs.
d. a chemical change occurs.
2
How many significant figures are in the
measurement 2103.2 g?
a. 2
c. 4
b. 3
d. 5
2
Which of these equalities is not correct?
a. 100 cg= 1 g
c. 1 cm3= 1 mL
b. 1000 mm= 1 m
d. 10 kg= 1 g
2
How many of the zeros in the measurement
040 200 m are significant?
a. 2
c. 7
b. 3
d. 8
0.000
2
How many milligrams are in 2.5 kg?
a. 2.5 x 106 mg
c. 2.5 x 104 mg
b. 25 mg
d. 2.5 x 102 mg
2
The closeness of a measurement to its true value is a
measure of its:
a. usefulness.
c. accuracy.
b. precision.
d. reproducibility.
2
Which of these measurements is expressed to three
significant figures?
a. 0.070 mm
c. 7007 mg
b. 7.30 x 107 km
d. 0.007 m
2
A metric unit of volume is the:
a. L.
c. km.
b. mg.
d. K.
2
The number of seconds in a 40-hour work week can be
calculated as follows:
2
The metric prefix kilo- means:
a. 100 times smaller.
c. 1000 times smaller.
b. 1000 times larger.
d. 100 times larger.
2
What is the volume of 60.0 g of ether if the density of
ether is 0.70 g/mL?
a. 86 mL
c. 2.4 x 102 mL
b. 1.2 x 102 mL
d. 42 mL
2
The temperature reading of -14C corresponds to a
Kelvin reading of:
a. 297.6 K.
c. 287 K.
b. -287 K.
d. 259 K.
2
Concentrated hydrochloric acid has a density of 1.19
g/mL. What is the mass, in grams, of 2.00 liters of
this acid?
a. 2.38 x 103 g
c. 4.20 x 10-4 g
b. 2.38 g
d. 4.20 x 104 g
2
A conversion factor:
a. is equal to 1.
b. is a ratio of equivalent measurements.
c. does not change the value of a measurement.
d. all of the above
2
Chlorine boils at 239 K. What is the boiling point of
chlorine expressed in degrees Celsius?
a. 93C
c. -61C
b. 34C
d. -34C
2
A student measures a volume as 25 mL, whereas the
correct volume is 23 mL. What is the percent error?
a. 0.087%
c. 0.92%
b. 8.7%
d. 8.0%
3
Which of the following is not a part of Dalton’s atomic
theory?
a. All elements are composed of atoms.
b. Atoms of the same element are alike.
c. Atoms are always in motion.
d. Atoms that combine do so in simple whole-number
ratios.
3
The nucleus of an atom is
a. negatively charged and has a low density.
b. negatively charged and has a high density.
c. positively charged and has a low density.
d. positively charged and has a high density.
3
Dalton theorized that atoms are indivisible and that all
atoms of an element are identical. Scientists now
know that
a. Dalton’s theories are completely correct.
b. atoms of an element can have different numbers of
protons.
c. atoms are all divisible.
d. all atoms of an element are not identical but they
all have the same mass.
3
The number of neutrons in the nucleus of an atom can
be calculated by
a. adding together the numbers of electrons and
protons.
b. subtracting the number of protons from the
number of electrons.
c. subtracting the number of protons from the mass
number.
d. adding the mass number to the number of protons.
3
The sum of the protons and neutrons in an atom equals
the
a. atomic number.
c. atomic mass.
b. number of electrons. d. mass number.
3
• All atoms of the same element have the same:
• a. number of protons.
c. mass number.
• b. number of neutrons.
d. mass.
3
•
•
•
•
•
Which of these statements is false?
a. Electrons have a negative charge.
b. Electrons have a mass of 1 amu.
c. The nucleus of an atom is positively charged.
d. The neutron is found in the nucleus of an atom.
3
• An atom of an element with atomic number 48 and
mass number 120 contains
• a. 48 protons, 48 electrons, and 72 neutrons.
• b. 72 protons, 48 electrons, and 48 neutrons.
• c. 120 protons, 48 electrons, and 72 neutrons.
• d. 72 protons, 72 electrons, and 48 neutrons.
3
•
•
•
•
•
The number 80 in the name bromine-80 represents
a. the atomic number.
b. the mass number.
c. the sum of protons and electrons.
d. none of the above
3
• Which of these statements is not true?
• a. Atoms of the same elements can have different
masses.
• b. The nucleus of an atom has a positive charge.
• c. Atoms of isotopes of an element have different
numbers of protons.
• d. Atoms are mostly empty space.
3
• Relative atomic masses are measured in
• a. nanograms.
c. angstroms.
• b. grams.
d. amus.
3
• If E is the symbol for an element, which two of the
following symbols represent isotopes of the same
element?
4
• The fourth principal energy level has
• a. 4 orbitals.
c. 32 orbitals.
• b. 16 orbitals.
d. 9 orbitals.
4
• If the electron configuration of an element is
1s22s22p63s23p5, the element is
• a. iron.
c. chlorine.
• b. bromine.
d. phosphorus.
4
•
•
•
•
•
The electron configuration of calcium is
a. 1s22s22p23s23p34s2.
b. 1s22s22p103s23p4.
c. 1s22s23s23p6 3d8.
d. 1s22s22p63s23p64s2.
4
• The maximum number of electrons that can occupy
the third principal energy level is
• a. 18.
c. 2.
• b. 32.
d. 8.
4
•
•
•
•
•
As the frequency of light increases, the wavelength
a. increases.
b. remains the same.
c. decreases.
d. approaches the speed of light.
4
• In order to occupy the same orbital, two electrons
must have
• a. the same direction of spin.
• b. low energy.
• c. opposite charge.
• d. opposite spin.
4
•
•
•
•
•
Stable electron configurations are likely to contain
a. high-energy electrons.
b. unfilled s orbitals.
c. fewer electrons than unstable configurations.
d. filled energy sublevels.
4
• According to Hund’s rule, when electrons occupy
orbitals of equal energy, one electron enters each
orbit until
• a. all the orbitals contain one electron, with spins
parallel.
• b. all the orbitals contain one electron, with
opposite spins.
• c. there are two electrons in each orbital.
• d. electron velocities become constant.
5
• In the periodic table, there is a periodic pattern in
the physical and chemical properties of elements
when they are arranged in order of
• a. increasing atomic mass.
• b. increasing electronegativity.
• c. increasing atomic radius.
• d. increasing atomic number.
5
• Which sublevel corresponds to the transition metals
in the periodic table?
• a. s
c. d
• b. p
d. f
5
• Which of the following elements is a metalloid?
• a. As
c. Br
• b. Se
d. Kr
5
•
•
•
•
•
The element iodine, I, is a
a. period 5 alkali metal.
b. period 4 halogen.
c. period 5 halogen.
d. period 5 transition metal.
5
• The subatomic particle that plays the greatest role in
determining the physical and chemical properties of
an element is the
• a. proton.
c. electron.
• b. neutron.
d. photon.
5
• Which of the following atoms would you expect to
have the largest atomic radius?
• a. I
c. Ca
• b. K
d. Rb
5
• From left to right across the second period of the
periodic table,
• a. first ionization energy increases.
• b. atomic radii increase.
• c. electronegativity decreases.
• d. atomic mass decreases.
5
• The category of elements that is characterized by the
filling of f orbitals is the
• a. inner transition metals.
• b. alkali metals.
• c. alkali earth metals.
• d. transition metals.
5
• Electronegativity
• a. generally decreases from left to right across a
period.
• b. is the energy change that accompanies the loss of
an electron from a gaseous atom.
• c. generally decreases from top to bottom within a
group.
• d. is generally higher for metals than for nonmetals.
5
•
•
•
•
•
Atomic size generally
a. increases from left to right across a period.
b. decreases from top to bottom within a group.
c. remains constant within a period.
d. decreases from left to right across a period.
5
• The alkali metals do not include
• a. Li.
c. Na.
• b. Ca.
d. Rb.
6
• How many valence electrons does an atom of any
element in Group 6A
• have?
• a. 2
c. 6
• b. 4
d. 8
6
• The electron dot structure for an atom of
phosphorus is
6
• Metals are good conductors of electricity because
they
• a. form crystal lattices.
• b. contain positive ions.
• c. contain mobile valence electrons.
• d. form ionic bonds.
6
• When an aluminum atom loses its valence electrons,
what is the charge on the resulting ion?
• a. 2+
c. 3+
• b. 2d. 1+
6
•
•
•
•
•
The electron configuration of a fluoride ion, F-, is
a. 1s2 2s2 2p5.
b. the same as that of the neon atom.
c. 1s2 2s2 2p6 3s1.
d. the same as that of a potassium ion.
6
•
•
•
•
•
In forming chemical bonds, atoms tend to attain
a. a state of higher energy.
b. the electron configuration of noble gas atoms.
c. the electron configuration of halogen atoms.
d. all of the above
6
•
•
•
•
•
An ionic compound is
a. electrically neutral.
b. held together by ionic bonds.
c. composed of anions and cations.
d. all of the above
6
• Which element when combined with chlorine would
most likely form an ionic compound?
• a. lithium
c. phosphorus
• b. carbon
d. bromine
6
•
•
•
•
•
A cation is any atom or group of atoms with
a. a positive charge.
b. no charge.
c. a negative charge.
d. more electrons than the corresponding atoms.
6
•
•
•
•
•
The cation Fe3+ is formed when
a. an atom of iron loses two electrons.
b. an atom of zinc loses two electrons.
c. an atom of iron loses three electrons.
d. an atom of iron gains three electrons.
6
• Which of these elements does not exist as a diatomic
molecule?
• a. I
c. H
• b. F
d. He
6
• Which one of the following compounds is not
covalent?
• a. SCl2
c. HCl
• b. KCl
d. S2Cl2
6
• How many valence electrons does an atom of any
halogen have?
• a. 1
c. 4
• b. 2
d. 7
6
• If a bonding pair of electrons is unequally shared
between two atoms, the bond is
• a. ionic.
c. coordinate covalent.
• b. nonpolar covalent.
d. polar covalent.
6
•
•
•
•
•
A covalent bond forms
a. when an element becomes a noble gas.
b. when atoms share electrons.
c. between metals and nonmetals.
d. when electrons are transferred from one atom to
another.
6
• Which of the following is the weakest?
• a. hydrogen bond
c. dipole interaction
• b. polar covalent bond
d. ionic bond
7
• The correct name for the N3- ion is the:
• a. nitrate ion.
c. nitride ion.
• b. nitric ion.
d. nitrite ion.
7
• What is the ionic charge on the chromium ion in the
ionic compound that has the formula Cr2O3?
• a. 3+
c. 5• b. 2d. 5+
7
• What is the formula for calcium hydrogen
phosphate?
• a. CaHPO4
c. Ca(H2PO4)2
• b. Ca2HPO4
d. Ca(HPO4)2
7
•
•
•
•
A molecular formula:
a. gives information about molecular geometry.
b. can be written for ionic compounds.
c. shows the number and kinds of atoms in a
molecule of a compound.
• d. uses superscripts to show the number of atoms
of each kind.
7
• The metals in Groups 1A, 2A, and 3A:
• a. gain electrons when they form ions.
• b. form ions with a charge found by subtracting 8
from the group number.
• c. all form ions with a 1 charge.
• d. lose electrons when they form ions.
7
• When naming an ion of a transition metal that has
more than one common ionic charge, the numerical
value of the charge is indicated by a:
• a. prefix.
• b. suffix.
• c. Roman numeral following the name.
• d. superscript after the name.
7
• In naming a binary molecular compound, the
number of atoms of each element present in the
molecule is indicated by:
• a. Roman numerals.
c. prefixes.
• b. superscripts.
d. suffixes.
7
• What is the formula for sulfuric acid?
• a. H2S2
c. H2SO3
• b. H2SO4
d. H2S
7
• Which of the following is not an empirical
formula?
• a. Na2SO4
c. N2H4
• b. C6H5Cl
d. Sn3(PO4)4
7
• Which expression represents the percent by
mass of nitrogen in NH4NO3?
8
• Which of these expressions is an incorrect
interpretation of the balanced equation?
•
•
•
•
•
2S(s) +3O2(g) → 2SO3(g)
a. 2 atoms S + 3 molecules O2 →2 molecules SO3
b. 2 g S + 3 g O2 → 2 g SO3
c. 2 mol S + 3 mol O2 → 2 mol SO3
d. none of the above
8
• When the equation Fe + O2
Fe2O3 is
balanced, the coefficient for O2 is:
• a. 4
c. 2
• b. 3
d. 1
9
• How many hydrogen atoms are in 4 molecules of
isopropyl alcohol,
• C3H8O?
• a. 4 x (6.02 x 1023)
c. 32
• b. 4
d. 32 x (6.02 x 1023)
9
• The mass of a mole of NaCl is its:
• a. molar mass.
c. gram atomic mass.
• b. empirical formula.
d. atomic mass.
9
• The chemical formula of aspirin is C9H8O4. What is
the mass of 0.200 mol of aspirin?
• a. 22.5 g
c. 80 g
• b. 5.4 g
d. 36.0 g
9
• How many moles of SO3 are in 2.4 x 1024 molecules
of SO3?
• a. 0.25
c. 4.0
• b. 3.4 x 1022
d. 2.9 x 1023
9
3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(s) + 2NO(g) +4H2O(l)
• How many grams of Cu would be needed to
react with 2.0 mol HNO3?
• a. 95.3 g
c. 47.6 g
• b. 63.5 g
d. 1.50 g
10
• The high surface tension of water is due to
the:
• a. small size of water molecules.
• b. low mass of water molecules.
• c. hydrogen bonding between water
molecules.
• d. covalent bonds in water molecules.
10
• The density of ice is less than the density of
water because:
• a. ice has a lower molecular mass than water.
• b. the same mass occupies a smaller volume.
• c. the molecules are more closely packed.
• d. hydrogen bonding in ice produces an open
framework.
11
• What is the volume (in liters at STP) of 2.50 mol of
carbon monoxide?
• a. 0.112 L
c. 56.0 L
• b. 3.10 L
d. 8.96 L
11
•
•
•
•
•
The molar mass of molecular oxygen is:
a. equal to the mass of one mole of oxygen atoms.
b. 16.0 g.
c. 32.0 g.
d. none of the above
11
•
•
•
•
•
The molar mass of a gas can be determined from:
a. the density of the gas at STP.
b. the volume of a mole of the gas.
c. Avogadro’s number.
d. none of the above
11
• How many liters of oxygen are required to
react completely with 1.2 liters of hydrogen to
form water?
•
2H2(g) O2(g) → 2H2(g)
• a. 1.2 L
c. 2.4 L
• b. 0.6 L
d. 4.8 L
11
• As the temperature of a fixed volume of gas
increases, the pressure will
• a. vary inversely. c. be unchanged.
• b. decrease.
d. increase.
11
• The volume of a gas is doubled while the
temperature is held constant. The pressure of
the gas
• a. remains unchanged.
• b. is reduced by one half.
• c. is doubled.
• d. depends on the kind of gas.
11
• A box with a volume of 22.4 L contains 1.0 mol of
nitrogen and 2.0 mol of hydrogen at 0C. Which of the
following statements is true?
• a. The total pressure in the box is 202.6 kPa.
• b. The partial pressure of N2 and H2 are equal.
• c. The total pressure is 101.3 kPa.
• d. The partial pressure of N2 is 101.3 kPa.
12
• What is the molarity of a 200-mL solution in
which 0.2 mole of sodium bromide is
dissolved?
• a. 0.20M
c. 0.40M
• b. 1.0M
d. 4.0M
12
• What is the percent by mass of a water
solution that contains 60 g of calcium chloride,
CaCl2, and that has a mass of 400 g?
• a. 15%
c. 24%
• b. 1.35%
d. 6.7%
14
• In the reaction NH4 + H2O → 1NH3 + H3O, water
is acting as a(n)
a. Arrhenius acid.
c. Brønsted acid.
b. Brønsted base.
d. Arrhenius base.
14
• Which of these is an Arrhenius base?
• a. KOH
c. H2PO4
• b. NH3
d. CH3COOH
14
• Which of these acids is monoprotic?
• a. CH3COOH
c. H2SO4
• b. H2CO3
d. H3PO4
15
• A solution in which the hydroxide-ion
concentration is 1 x 10-5M is
• a. acidic.
c. neutral.
• b. basic.
d. none of the above
15
• In a neutral solution, the [H+] is
• a. 10-14.
c. 1 x 107M.
• b. zero.
d. equal to [OH-].
15
• What is the pH of a solution in which the [H]
1 x 1012?
• a. 1.0
c. 2.0
• b. 2.0
d. 12.0
15
•
•
•
•
•
A solution with a pH of 5.0
a. is basic.
b. has a hydrogen-ion concentration of 5.0M.
c. is neutral.
d. has a hydroxide -ion concentration of
1
x 10-9M.
14
• According to the Brønsted theory, water
• a. acts as a base when it accepts a hydrogen
ion.
• b. can be neither an acid nor a base.
• c. acts as an acid by accepting hydrogen ions.
• d. can accept but not donate hydrogen ions.