Final Review Part Two

Final Review Part Two

Multiple Choice

Identify the choice that best completes the statement or answers the question.

____1.Which hypothesis led to the discovery of the proton?

a. / When a neutral hydrogen atom loses an electron, a positively-charged particle should remain.
b. / A proton should be 1840 times heavier than an electron.
c. / Cathode rays should be attracted to a positively-charged plate.
d. / The nucleus of an atom should contain neutrons.

____2.Which of the following is correct concerning subatomic particles?

a. / The electron was discovered by Goldstein in 1886.
b. / The neutron was discovered by Chadwick in 1932.
c. / The proton was discovered by Thomson in 1880.
d. / Cathode rays were found to be made of protons.

____3.All atoms are ____.

a. / positively charged, with the number of protons exceeding the number of electrons
b. / negatively charged, with the number of electrons exceeding the number of protons
c. / neutral, with the number of protons equaling the number of electrons
d. / neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons

____4.Which of the following sets of symbols represents isotopes of the same element?

a. / J J J / c. / M M M
b. / L L L / d. / Q Q Q

____5.How do the isotopes hydrogen-1 and hydrogen-2 differ?

a. / Hydrogen-2 has one more electron than hydrogen-1.
b. / Hydrogen-2 has one neutron; hydrogen-1 has none.
c. / Hydrogen-2 has two protons; hydrogen-1 has one.
d. / Hydrogen-2 has one proton; hydrogen-1 has none.

____6.Which of the following isotopes has the same number of neutrons as phosphorus-31?

a. / P / c. / Si
b. / S / d. / Si

____7.What is the maximum number of electrons in the second principal energy level?

a. / 2 / c. / 18
b. / 8 / d. / 32

____8.When an electron moves from a lower to a higher energy level, the electron ____.

a. / always doubles its energy
b. / absorbs a continuously variable amount of energy
c. / absorbs a quantum of energy
d. / moves closer to the nucleus

____9.If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?

a. / one electron in each orbital
b. / two electrons in one orbital, one in another, none in the third
c. / three in one orbital, none in the other two
d. / Three electrons cannot fill three empty 2p atomic orbitals.

____10.How many unpaired electrons are in a sulfur atom (atomic number 16)?

a. / 0 / c. / 2
b. / 1 / d. / 3

____11.How many half-filled orbitals are in a bromine atom?

a. / 1 / c. / 3
b. / 2 / d. / 4

____12.Which of the following electron configurations of outer sublevels is the most stable?

a. / 4d5s / c. / 4d5s
b. / 4d5s / d. / 4d5s

____13.What is the wavelength of an electromagnetic wave that travels at 3 10 m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)

a. /
b. / 60 MHz  300,000,000 m/s
c. /
d. / No answer can be determined from the information given.

____14.Which variable is directly proportional to frequency?

a. / wavelength / c. / position
b. / velocity / d. / energy

____15.How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom?

a. / They are greater in magnitude than those between lower energy levels.
b. / They are smaller in magnitude than those between lower energy levels.
c. / There is no significant difference in the magnitudes of these differences.
d. / No answer can be determined from the information given.

____16.In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend on ____.

a. / a quantum mechanical model / c. / the Schrodinger equation
b. / direction with respect to the nucleus / d. / the electron energy sublevel

____17.To what category of elements does an element belong if it is a poor conductor of electricity?

a. / transition elements / c. / nonmetals
b. / metalloids / d. / metals

____18.Of the elements Fe, Hg, U, and Te, which is a representative element?

a. / Fe / c. / U
b. / Hg / d. / Te

____19.Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?

a. / more shielding of the electrons by the highest occupied energy level
b. / an increase in size of the nucleus
c. / an increase in number of protons
d. / fewer electrons in the highest occupied energy level

____20.Which of the following elements has the smallest atomic radius?

a. / sulfur / c. / selenium
b. / chlorine / d. / bromine

____21.In which of the following sets are the charges given correctly for all the ions?

a. / Na, Mg, Al / c. / Rb, Ba, P
b. / K, Sr, O / d. / N, O, F

____22.In which of the following groups of ions are the charges all shown correctly?

a. / Li, O, S / c. / K, F, Mg
b. / Ca, Al, Br / d. / Na, I, Rb

____23.Which of the following factors contributes to the increase in ionization energy from left to right across a period?

a. / an increase in the shielding effect
b. / an increase in the size of the nucleus
c. / an increase in the number of protons
d. / fewer electrons in the highest occupied energy level

____24.As you move from left to right across the second period of the periodic table ____.

a. / ionization energy increases / c. / electronegativity decreases
b. / atomic radii increase / d. / atomic mass decreases

____25.Of the following elements, which one has the smallest first ionization energy?

a. / boron / c. / aluminum
b. / carbon / d. / silicon

____26.Which of the following pairs of elements is most likely to form an ionic compound?

a. / magnesium and fluorine
b. / nitrogen and sulfur
c. / oxygen and chlorine
d. / sodium and aluminum

____27.Which elements can form diatomic molecules joined by a single covalent bond?

a. / hydrogen only
b. / halogens only
c. / halogens and members of the oxygen group only
d. / hydrogen and the halogens only

____28.Which of the following electron configurations gives the correct arrangement of the four valence electrons of the carbon atom in the molecule methane (CH)?

a. / 2s2p / c. / 2s2p3s
b. / 2s2p3s / d. / 2s2p

____29.Which of the following covalent bonds is the most polar?

a. / H—F / c. / H—H
b. / H—C / d. / H—N

____30.When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the ____.

a. / hydrogen region of the molecule / c. / H—O—H plane of the molecule
b. / geometric center of the molecule / d. / oxygen region of the molecule

____31.Which polyatomic ion forms a neutral compound when combined with a group 1A monatomic ion in a 1:1 ratio?

a. / ammonium / c. / nitrate
b. / carbonate / d. / phosphate

____32.Consider a mystery compound having the formula MT. If the compound is not an acid, if it contains only two elements, and if M is not a metal, which of the following is true about the compound?

a. / It contains a polyatomic ion. / c. / Its name ends in -ic.
b. / Its name ends in -ite or -ate. / d. / It is a binary molecular compound.

____33.What is the formula for hydrosulfuric acid?

a. / HS / c. / HSO
b. / HSO / d. / HS

____34.What is the correct formula for barium chlorate?

a. / Ba(ClO) / c. / Ba(ClO)
b. / Ba(ClO) / d. / BaCl

____35.What is the correct formula for calcium dihydrogen phosphate?

a. / CaHPO / c. / Ca(HPO)
b. / CaHPO / d. / Ca(HHPO)

____36.What is the correct name for Sn(PO)?

a. / tritin diphosphate / c. / tin(III) phosphate
b. / tin(II) phosphate / d. / tin(IV) phosphate

____37.Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 10 atoms of hydrogen, what is the subscript for the hydrogen atom in CHO?

a. / 1 / c. / 6
b. / 10 / d. / 8

____38.Which of the following gas samples would have the largest number of representative particles at STP?

a. / 12.0 L He / c. / 0.10 L Xe
b. / 7.0 L O / d. / 0.007 L SO

____39.Given 1.00 mole of each of the following gases at STP, which gas would have the greatest volume?

a. / He / c. / SO
b. / O / d. / All would have the same volume.

____40.If the density of a noble gas is 1.783 g/L at STP, that gas is ____.

a. / Kr / c. / Ar
b. / Xe / d. / He

____41.Which of the following compounds has the lowest percent gold content by weight?

a. / AuOH / c. / AuCl
b. / Au(OH) / d. / AuI

____42.Which of the following compounds has the highest oxygen content, by weight?

a. / NaO / c. / BaO
b. / CO / d. / HO

____43.The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar mass is 280 g?

a. / CHO / c. / CHO
b. / CHO / d. / CHO

____44.Who was the man who lived from 460B.C.–370B.C. and was among the first to suggest the idea of atoms?

a. / Atomos / c. / Democritus
b. / Dalton / d. / Thomson

____45.Which of the following was NOT among Democritus’s ideas?

a. / Matter consists of tiny particles called atoms.
b. / Atoms are indivisible.
c. / Atoms retain their identity in a chemical reaction.
d. / Atoms are indestructible.

____46.Dalton's atomic theory included which idea?

a. / All atoms of all elements are the same size.
b. / Atoms of different elements always combine in one-to-one ratios.
c. / Atoms of the same element are always identical.
d. / Individual atoms can be seen with a microscope.

____47.Which of the following is NOT a part of Dalton's atomic theory?

a. / All elements are composed of atoms.
b. / Atoms are always in motion.
c. / Atoms of the same element are identical.
d. / Atoms that combine do so in simple whole-number ratios.

____48.Which of the following was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?

a. / Atoms are tiny indivisible particles.
b. / Atoms of the same element are identical.
c. / Compounds are made by combining atoms.
d. / Atoms of different elements can combine with one another in simple whole number ratios.

____49.The comparison of the number of atoms in a copper coin the size of a penny with the number of people on Earth is made to illustrate which of the following?

a. / that atoms are indivisible
b. / that atoms are very small
c. / that atoms are very large
d. / that in a copper penny, there is one atom for every person on Earth

____50.The range in size of most atomic radii is approximately ____.

a. / 2 to 5 cm / c. / 5 10 m to 2 10 m
b. / 2 to 5 nm / d. / 5 10 m to 2 10 m

____51.Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?

a. / Cathode rays are negatively-charged particles.
b. / Cathode rays can be deflected by magnets.
c. / An electron is 2000 times lighter than a hydrogen atom.
d. / Charge-to-mass ratio of electrons was the same, regardless of the gas used.

____52.Which of the following is true about subatomic particles?

a. / Electrons are negatively charged and are the heaviest subatomic particle.
b. / Protons are positively charged and the lightest subatomic particle.
c. / Neutrons have no charge and are the lightest subatomic particle.
d. / The mass of a neutron nearly equals the mass of a proton.

____53.Who conducted experiments to determine the quantity of charge carried by an electron?

a. / Rutherford / c. / Dalton
b. / Millikan / d. / Thomson

____54.What is the relative mass of an electron?

a. / 1/1840 the mass of a hydrogen atom / c. / 1/1840 the mass of a C-12 atom
b. / 1/1840 the mass of a neutron + proton / d. / 1/1840 the mass of an alpha particle

____55.The particles that are found in the nucleus of an atom are ____.

a. / neutrons and electrons / c. / protons and neutrons
b. / electrons only / d. / protons and electrons

____56.As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?

a. / Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.
b. / The nucleus is made of protons, electrons, and neutrons.
c. / Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
d. / The nucleus is made of electrons and protons.

____57.The nucleus of an atom is ____.

a. / the central core and is composed of protons and neutrons
b. / positively charged and has more protons than neutrons
c. / negatively charged and has a high density
d. / negatively charged and has a low density

____58.In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a. / In, 49 protons, 49 electrons / c. / Cs, 55 protons, 132.9 electrons
b. / Zn, 30 protons, 60 electrons / d. / F, 19 protons, 19 electrons

____59.The mass number of an element is equal to ____.

a. / the total number of electrons in the nucleus
b. / the total number of protons and neutrons in the nucleus
c. / less than twice the atomic number
d. / a constant number for the lighter elements

____60.Using the periodic table, determine the number of neutrons in O.

a. / 4 / c. / 16
b. / 8 / d. / 24

____61.How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?

a. / 50 protons, 50 electrons, 75 neutrons / c. / 120 neutrons, 50 protons, 75 electrons
b. / 75 electrons, 50 protons, 50 neutrons / d. / 70 neutrons, 75 protons, 50 electrons

____62.Which of the following statements is NOT true?

a. / Atoms of the same element can have different masses.
b. / Atoms of isotopes of an element have different numbers of protons.
c. / The nucleus of an atom has a positive charge.
d. / Atoms are mostly empty space.

____63.If E is the symbol for an element, which two of the following symbols represent isotopes of the same element?

1. E / 2. E / 3. E / 4. E
a. / 1 and 2 / c. / 1 and 4
b. / 3 and 4 / d. / 2 and 3

____64.Select the correct symbol for an atom of tritium.

a. / n / c. / H
b. / H / d. / H

____65.How is the number of neutrons in the nucleus of an atom calculated?

a. / Add the number of electrons and protons together.
b. / Subtract the number of electrons from the number of protons.
c. / Subtract the number of protons from the mass number.
d. / Add the mass number to the number of electrons.

____66.In which of the following is the number of neutrons correctly represented?

a. / F has 0 neutrons. / c. / Mg has 24 neutrons.
b. / As has 108 neutrons. / d. / U has 146 neutrons.

____67.Which of the following statements is NOT true?

a. / Protons have a positive charge.
b. / Electrons are negatively charged and have a mass of 1 amu.
c. / The nucleus of an atom is positively charged.
d. / Neutrons are located in the nucleus of an atom.

____68.Why do chemists use relative masses of atoms compared to a reference isotope rather than the actual masses of the atoms?

a. / The actual mass of an electron is very large compared to the actual mass of a proton.
b. / The actual masses of atoms are very small and difficult to work with.
c. / The number of subatomic particles in atoms of different elements varies.
d. / The actual masses of protons, electrons, and neutrons are not known.

____69.The atomic mass of an element is the ____.

a. / total number of subatomic particles in its nucleus
b. / weighted average of the masses of the isotopes of the element
c. / total mass of the isotopes of the element
d. / average of the mass number and the atomic number for the element

____70.The atomic mass of an element depends upon the ____.

a. / mass of each electron in that element
b. / mass of each isotope of that element
c. / relative abundance of protons in that element
d. / mass and relative abundance of each isotope of that element

____71.Which of the following is necessary to calculate the atomic mass of an element?

a. / the atomic mass of carbon-12
b. / the atomic number of the element
c. / the relative masses of the element’s protons and neutrons
d. / the masses of each isotope of the element

____72.The principal quantum number indicates what property of an electron?

a. / position / c. / energy level
b. / speed / d. / electron cloud shape

____73.Each period in the periodic table corresponds to ____.

a. / a principal energy level / c. / an orbital
b. / an energy sublevel / d. / a suborbital

____74.The modern periodic table is arranged in order of increasing atomic ____.

a. / mass / c. / number
b. / charge / d. / radius

____75.Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a. / Pt / c. / Li
b. / V / d. / Kr

____76.The atomic number of an element is the total number of which particles in the nucleus?

a. / neutrons / c. / electrons
b. / protons / d. / protons and electrons

____77.What element has the electron configuration 1s2s2p3s3p?

a. / nitrogen / c. / silicon
b. / selenium / d. / silver

____78.Which of the following is true about the electron configurations of the noble gases?

a. / The highest occupied s and p sublevels are completely filled.
b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.

____79.Elements that are characterized by the filling of p orbitals are classified as ____.

a. / groups 3A through 8A / c. / inner transition metals
b. / transition metals / d. / groups 1A and 2A

____80.Which of the following electron configurations is most likely to result in an element that is relatively inactive?

a. / a half-filled energy sublevel
b. / a filled energy sublevel
c. / one empty and one filled energy sublevel
d. / a filled highest occupied principal energy level

____81.Which subatomic particle plays the greatest part in determining the properties of an element?

a. / proton / c. / neutron
b. / electron / d. / none of the above

____82.Which of the following is true about the electron configurations of the representative elements?

a. / The highest occupied s and p sublevels are completely filled.
b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.

____83.What are the Group 1A and Group 7A elements examples of?

a. / representative elements / c. / noble gases
b. / transition elements / d. / nonmetallic elements

____84.How does atomic radius change from left to right across a period in the periodic table?

a. / It tends to decrease. / c. / It first increases, then decreases.
b. / It tends to increase. / d. / It first decreases, then increases.

____85.What causes the shielding effect to remain constant across a period?

a. / Electrons are added to the same principal energy level.
b. / Electrons are added to different principal energy levels.
c. / The charge on the nucleus is constant.
d. / The atomic radius increases.

____86.Atomic size generally ____.

a. / increases as you move from left to right across a period
b. / decreases as you move from top to bottom within a group
c. / remains constant within a period
d. / decreases as you move from left to right across a period

____87.What element in the second period has the largest atomic radius?

a. / carbon / c. / potassium
b. / lithium / d. / neon

____88.Which of the following statements is true about ions?

a. / Cations form when an atom gains electrons.
b. / Cations form when an atom loses electrons.
c. / Anions form when an atom gains protons.
d. / Anions form when an atom loses protons.

____89.The metals in Groups 1A, 2A, and 3A ____.

a. / gain electrons when they form ions / c. / all have ions with a 1 charge
b. / all form ions with a negative charge / d. / lose electrons when they form ions

____90.Which of the following statements is NOT true about ions?

a. / Cations are positively charged ions.
b. / Anions are common among nonmetals.
c. / Charges for ions are written as numbers followed by a plus or minus sign.
d. / When a cation forms, more electrons are transferred to it.

____91.Why is the second ionization energy greater than the first ionization energy?

a. / It is more difficult to remove a second electron from an atom.
b. / The size of atoms increases down a group.
c. / The size of anions decreases across a period.
d. / The nuclear attraction from protons in the nucleus decreases.

____92.Which of the following elements has the smallest ionic radius?

a. / Li / c. / O
b. / K / d. / S

____93.What is the energy required to remove an electron from an atom in the gaseous state called?