Download Chemistry I Honors Semester I FINAL EXAM REVIEW Atomic

Chemistry I Honors Semester I FINAL EXAM REVIEW Atomic Structure, P Table
Multiple Choice Identify the choice that best completes the statement or answers the question.
____ 1. Which of the following is an extensive property of matter?
a. melting point
b. boiling point
c. volume
d. density
____ 2. An atom is
a. the smallest unit of matter that maintains its chemical identity.
b. the smallest unit of a compound.
c. always made of carbon.
d. smaller than an electron.
____ 3. A measure of the quantity of matter is
a. density.
b. weight.
c. volume.
d. mass.
____ 4. Which of the following is not a physical change?
a. grinding
b. cutting
c. boiling
d. burning
____ 5. Which of the following is not a chemical change?
a. rusting
b. igniting
c. melting
d. burning
____ 6. A state of matter in which a material has no definite shape but has a definite volume is the ____ state.
a. gas
b. liquid
c. plasma
d. Solid
____ 7. Under ordinary conditions of temperature and pressure, the particles in a gas are
a. closely packed.
c. held in fixed positions.
b. very far from one another.
d. unevenly distributed.
____ 8. The solid state of matter can be described as
a. having definite shape and definite volume.
b. having neither a definite shape nor a definite volume.
c. having lost electrons owing to energy content.
d. having a definite volume but not a definite shape.
____ 9. A mixture is
a. a combination of pure substances bonded chemically.
b. any substance with a uniform composition.
c. a blend of any two or more kinds of matter, as long as each maintains its own unique
properties.
d. any group of elements that are chemically bonded to one another.
____ 10. If a mixture is not uniform throughout, it is called
a. homogeneous.
b. heterogeneous.
c. a compound
d. a solution.
____ 11. The vertical columns on the periodic table are called
a. periods.
b. rows.
c. groups.
d. elements.
____ 12. The horizontal rows on the periodic table are called
a. actinides.
b. families.
c. elements.
d. periods.
____ 13. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a
compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a. equal to
c. less than
b. greater than
d. either greater than or less than
____ 14. Experiments with cathode rays led to the discovery of the
a. proton.
b. nucleus.
c. neutron.
d. electron.
____ 15. An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
____ 16.
____ 17.
____ 18.
____ 19.
____ 20.
____ 21.
____ 22.
____ 23.
____ 24.
____ 25.
____ 26.
____ 27.
____ 28.
____ 29.
____ 30.
____ 31.
____ 32.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
The atomic number of oxygen, 8, indicates that there are eight
a. protons in the nucleus of an oxygen atom.
b. oxygen nuclides.
c. neutrons outside the oxygen atom's nucleus.
d. energy levels in the oxygen atom's nucleus.
The total number of protons and neutrons in the nucleus of an atom is its
a. atomic number.
c. mass number.
b. Avogadro number.
d. average atomic mass.
All atoms of the same element have the same
a. atomic mass.
b. # of neutrons.
c. mass number.
d. atomic number.
The average atomic mass of an element is the average of the atomic masses of its
a. naturally occurring isotopes.
c. radioactive isotopes.
b. two most abundant isotopes.
d. artificial isotopes.
An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a. 13.
b. 14.
c. 27.
d. 40.
Chlorine has atomic number 17 and mass number 35. It has
a. 17 protons, 17 electrons, 18 neutrons.
c. 17 protons, 17 electrons, 52 neutrons.
b. 35 protons, 35 electrons, 17 neutrons.
d. 18 protons, 18 electrons, 17 neutrons.
Neon-22 contains 12 neutrons. It also contains
a. 12 protons.
b. 22 protons.
c. 22 electrons.
d. 10 protons.
There are two naturally-occuring isotopes of an unknown element, X-35 and X-37. The percent abundance of
X-35 is 73%. The percent abundance of X-37 is 27%. What is the atomic mass of element X?
a. 35 amu
b. 37 amu
c. 35.5 amu
d. 36 amu
Explain why hydrogen’s atomic mass is 1.0079 amu, if there are 3 naturally occurring isotopes of hydrogen:
hydrogen-1, hydrogen-2, and hydrogen-3.
a. hydrogen-1 occurs most frequently
c. hydrogen’s atomic number is 1
b. hydrogen-1 is easier to use in calculations d. hydrogen-2 and hydrogen-3 are hard to
isolate
The idea of arranging the elements in the periodic table according to their chemical and physical properties is
attributed to
a. Mendeleev.
b. Moseley.
c. Bohr.
d. Ramsay.
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were
arranged in order of increasing
a. atomic number.
b. density.
c. reactivity.
d. atomic mass.
The person whose work led to a periodic table based on increasing atomic number was
a. Moseley.
b. Mendeleev.
c. Rutherford.
d. Cannizzaro.
What are the radioactive elements with atomic numbers from 90 to 103 called?
a. the noble gases
b. the lanthanides
c. the actinides
d. alkali metals
What are the elements with atomic numbers from 58 to 71 called?
a. lanthanides
b. noble gases
c. actinides
d. alkali metals
Argon, krypton, and xenon are
a. halogens
b. noble gases.
c. actinides.
d. lanthanides.
Identify the sublevels in a period that contains 32 elements.
____ 33.
____ 34.
____ 35.
____ 36.
____ 37.
____ 38.
____ 39.
____ 40.
____ 41.
____ 42.
____ 43.
____ 44.
____ 45.
a. s, f
b. s, p
c. s, p, d
d. s, p, d, f
Because the first energy level contains only the 1s sublevel, the number of elements in this period is
a. 1.
b. 2.
c. 4.
d. 8.
Calcium, atomic number 20, has the electron configuration that ends in 4s2. In what period is calcium?
a. Period 2
b. Period 4
c. Period 8
d. Period 20
The group of 14 f block elements in the sixth period is the
a. actinides.
b. lanthanides.
c. transition metals d. metalloids.
The elements in Group 1 are also known as the
a. alkali metals.
b. transition metals. c. Period 1.
d. actinide series.
A positive ion is known as a(n)
a. ionic radius.
b. electron.
c. cation.
d. anion
If electrons in an atom have the lowest possible energies, the atom is in the
a. ground state.
c. excited state.
b. inert state.
d. radiation-emitting state.
According to Bohr, electrons cannot reside at ____ in the figure below.
a. point A
b. point B
c. point C
d. point D
The letter designations for the first four sublevels with the maximum number of electrons that can be
accommodated in each sublevel are
a. s:2, p:4, d:6, and f:8.
c. s:2, p:6, d:10, and f:14.
b. s:1, p:3, d:5, and f:7.
d. s:1, p:2, d:3, and f:4.
The total number of orbitals that can exist at the second main energy level is
a. 2.
b. 3.
c. 4.
d. 8.
Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau
principle?
a. 1s 2s 2p 3s 4s 3p 3d 4p 5s
c. 1s 2s 2p 3s 3p 4s 4p 3d 4d
b. 1s 2s 2p 3s 3p 4s 3d 4p 5s
d. 1s 2s 2p 3s 3p 3d 4s 4p 5s
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a. Mg (Z = 12).
b. C (Z = 6).
c. S (Z = 16).
d. Si (Z = 14).
2
2
2
The electron configuration for the carbon atom (C) is 1s 2s 2p . The atomic number of carbon is
a. 3.
b. 6.
c. 11.
d. 12.
What is the electron configuration for nitrogen, atomic number 7?
a. 1s2 2s2 2p3
b. 1s2 2s3 2p2
c. 1s2 2s3 2p1
d. 1s2 2s2 2p2 3s1
Chemistry I Honors 2nd Six Weeks' PRACTICE Test (Ch 1, 3, 4, 5)
Answer Section
MULTIPLE CHOICE
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