The University of the State of New York
MOCK REGENTS HIGH SCHOOL EXAMINATION
You are to answer all questions in all parts of this examination according to the directions provided.
Record the number of your choice for each Part A and Part B–1 multiple-choice question on your separate answer sheet. Write your answers to the Part B–2 and
Part C questions in your answer booklet. You may use scrap paper to work out the answers to the questions, but be sure to record all your answers on your separate answer sheet and in your answer booklet.
Notice. . .
A four-function or scientific calculator and a copy of the Reference Tables for Physical
Setting/Chemistry must be available for your use while taking this examination.
Part A
Answer all questions in this part.
Directions (1–20) : For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry .
1.
Which statement best describes electrons?
(1) They are positive subatomic particles and
are found in the nucleus.
(2) They are positive subatomic particles and
are found surrounding the nucleus.
(3) They are negative subatomic particles and
are found in the nucleus.
(4) They are negative subatomic particles and
are found surrounding the nucleus.
5.
An increase in the average kinetic energy of a sample of copper atoms occurs with an increase in
(1) concentration
(2) temperature
(3) pressure
(4) volume
6.
The high electrical conductivity of metals is primarily due to
(1) high ionization energies
(2) filled energy levels
(3) mobile electrons
(4) high electronegativities 2.
Which Group of the Periodic Table contains atoms with a stable outer electron configuration?
(1) 1 (3) 16
(2) 8 (4) 18
7.
The atomic number of an atom is always equal to the number of its
(1) protons, only (3) neutrons, only
(2) protons plus neutrons (4) protons plus electrons 3.
What is the percent by mass of oxygen in
H
2
SO
4
? [formula mass = 98]
(1) 16%
(2) 33%
(3) 65%
(4) 98%
4.
The strength of an atom’s attraction for the electronsin a chemical bond is the atom’s
(1) electronegativity
(2) ionization energy
(3) heat of reaction
(4) heat of formation
8.
What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table?
(1) the number of neutrons in the atom
(2) the number of protons in the atom
(3) the number of valence electrons in the atom
(4) the total number of electrons in the atom

9.
Which is an empirical formula?
(1) P
2
O
5
(3) C
2
H
4
(2) P
4
O
6
(4) C
3
H
6
10.
The percent by mass of calcium in the compound calcium sulfate (CaSO
4
) is approximately
(1) 15%
(2) 29%
(3) 34%
(4) 47%
11.
Which type of chemical bond is formed between two atoms of bromine?
(1) metallic
(2) hydrogen
(3) ionic
(4) covalent
12.
The region that is the most probable location of an electron in an atom is
(1) the nucleus
(2) an orbital
(3) the excited state
(4) an ion
13.
Which of these formulas contains the most polar bond?
(1) H–Br
(2) H–Cl
(3) H–F
(4) H–I
14.
Which type of change must occur to form a compound?
(1) chemical
(2) physical
(3) nuclear
(4) phase
15.
Which formula correctly represents the composition of iron (III) oxide?
(1) FeO
3
(3) Fe
3
O
(2) Fe
2
O
3
(4) Fe
3
O
2
16.
Given the reaction:
PbCl
2
(aq) + Na
2
CrO
4
(aq)->PbCrO
4
(s) + 2 NaCl(aq)
What is the total number of moles of NaCl formed when 2 moles of Na
2
CrO
4 react completely?
(1) 1 mole
(2) 2 moles
(3) 3 moles
(4) 4 moles
17.
What is the total number of valence electrons in an atom of sulfur in the ground state?
(1) 6
(2) 8
(3) 3
(4) 4
18.
In which compound is the percent by mass of oxygen greatest?
(1) BeO
(2) MgO
(3) CaO
(4) SrO
19.
Which type of bond is formed when electrons are transferred from one atom to another?
(1) covalent
(2) ionic
(3) hydrogen
(4) metallic
20.
Which Lewis electron-dot structure is drawn correctly for the atom it represents?
21.
What occurs when an atom of chlorine forms a chloride ion?
(1) The chlorine atom gains an electron, and its
radius becomes smaller.
(2) The chlorine atom gains an electron, and its
radius becomes larger.
(3) The chlorine atom loses an electron, and its
radius becomes smaller.
(4) The chlorine atom loses an electron, and its
radius becomes larger.

22.
Which of the following solids has the highest melting point?
(1) H
2
O(s)
(2) Na
2
O(s)
(3) SO
2
(s)
(4) CO
2
(s)
23.
A student intended to make a salt solution with a concentration of 10.0 grams of solute per liter of solution. When the student’s solution was analyzed, it was found to contain 8.90 grams of solute per liter of solution. What was the percent error in the concentration of the solution?
(1) 1.10% (3) 11.0%
(2) 8.90% (4) 18.9%
24.
Given the equation:
2 C
2
H
2
(g) + 5 O
2
(g)

4 CO
2
(g) + 2 H
2
O(g)
How many moles of oxygen are required to react completely with 1.0 mole of C
2
H
2
?
(1) 2.5
(2) 2.0
(3) 5.0
(4) 10
25.
Given the unbalanced equation:
__Fe
2
O
3
+ __CO

__Fe + __CO
2
When the equation is correctly balanced using the smallest whole-number coefficients, what is the coefficient of CO?
(1) 1
(2) 2
(3) 3
(4) 4
26.
The nucleus of an atom of K-42 contains
(1) 19 protons and 23 neutrons
(2) 19 protons and 42 neutrons
(3) 20 protons and 19 neutrons
(4) 23 protons and 19 neutrons
27.
What is the total number of electrons in a
Cu
+ ion?
(1) 28
(2) 29
(3) 30
(4) 36
Part B–1
Answer all questions in this part.
Directions (22–34) : For each statement or question, write the number of the word or expression that, of those given, best completes the statement or answers the question.
Some questions may require the use of the Reference Tables for Physical Setting/Chemistry .
28.
The freezing point of bromine is
(1) 539°C (3) 7°C
(2) –539°C (4) –7°C
29.
Which ion has the same electron configuration as an atom of He?
(1) H
–
(2) O
2–
(3) Na
(4) Ca
+
2+
30.
Which list of elements is arranged in order of increasing atomic radii?
(1) Li, Be, B, C (3) Sc, Ti, V, Cr
(2) Sr, Ca, Mg, Be (4) F, Cl, Br, I
31.
What is the molecular formula of a compound that has a molecular mass of 54 and the empirical formula C
2
H
3
?
(1) C
2
H
3
(2) C
4
H
6
(3) C
6
H
9
(4) C
8
H
12
32.
Given the balanced equation:
2 C
4
H
10
(g) + 13 O
2
(g)

8 CO
2
(g) + 10 H
2
O(g)
What is the total number of moles of O
2
(g) that must react completely with 5.00 moles of C
4
H
10
(g)?
(1) 10.0 (3) 26.5
(2) 20.0 (4) 32.5
33.
Which particle has the same electron configuration as a potassium ion?
(1) fluoride ion (3) neon atom
(2) sodium ion (4) argon atom
34.
Which is an electron configuration for an atom of chlorine in the excited state?
(1) 2–8–7
(2) 2–8–8
(3) 2–8–6–1
(4) 2–8–7–1