AnswersNY-Chemistry Term 1 HillcrestCumulative Exam

Cumulative Exam — Cumulative exam Answers

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1
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Which is a feature of a single replacement reaction?

A
Substance XYZ breaks down into X and YZ.
B
Substance G reacts with compound XY to form GY and X.
C
Substance X burns rapidly in the presence of oxygen.
D
Substance QR and GT exchange ions with each other.
2
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A teacher wants to perform a classroom demonstration that illustrates both chemical and physical changes. Which would be the best demonstration that she could use?

A
bending a piece of aluminum
B
breaking a matchstick
C
dissolving sugar in water
D
burning a candle
3

A single atom of an element has 21 neutrons, 20 electrons, and 20 protons. Which element is it?

A
K
B
Zr
C
Ca
D
Sc
4

Which of the following best describes a pair of elements that will form an ionic bond?

A
C and H: Hydrogen easily loses electrons, and carbon gains them.
B
Li and O: Oxygen easily loses electrons, and lithium gains them.
C
P and Cl: Phosphorus easily loses electrons, and chlorine gains them.
D
Ca and Br: Calcium easily loses electrons, and bromine gains them.
5

Consider the balanced equation below.N2H4 + 2H2O2 N2 + 4H2OWhat are the mole ratios of hydrazine (N2H4) to hydrogen peroxide (H2O2) and hydrazine to water?

Question illustration
A
1:2 and 1:4
B
1:3 and 1:4
C
1:2 and 3:5
D
1:3 and 3:5
6

A mixture of three noble gases has a total pressure of 1.25 atm. The individual pressures exerted by neon and argon are 0.68 atm and 0.35 atm, respectively. What is the partial pressure of the third gas, helium?Use .

Question illustration
A
0.22 atm
B
0.33 atm
C
1.03 atm
D
2.28 atm
7

The diagram below shows that the periodic table is divided into different blocks.Elements that have complete valence electron shells are mostly found in the

Question illustration
A
s block.
B
d block.
C
p block.
D
f block.
8

Consider the half reactions below for a chemical reaction.What is the overall equation for this chemical reaction?

Question illustration
A
Upper M g (s) plus 2 upper H superscript plus (a q) right arrow upper M g superscript 2 plus (a q) plus upper H subscript 2 (g).
Option A
B
Upper M g (s) plus 2 upper H superscript plus (a q) right arrow upper M g superscript 2 plus (a q) plus 2 e superscript minus.
Option B
C
Upper M g superscript 2 plus (a q) plus upper H subscript 2 (g) right arrow upper M g (s) plus 2 upper H superscript plus (a q).
Option C
D
Upper M g (s) plus 2 upper H right arrow upper M g (a q) plus upper H subscript 2 (g).
Option D
9

Consider the reaction below.2C6H14 + 19O2 12CO2 + 14H2OHow many moles of hexane (C6H14) must burn to form 18.4 mol of carbon dioxide?

Question illustration
A
1.53 mol
B
3.07 mol
C
110. mol
D
175. mol
10

The expression below was formed by combining different gas laws. Which law was used to determine the relationship between the volume and the number of moles in this equation?

Question illustration
A
Boyle’s law
B
Charles’s law
C
Avogadro’s law
D
Gay-Lussac’s law
11

Which element is likely to have a high thermal conductivity?

A
antimony
B
carbon
C
chlorine
D
sodium
12

Which diagram shows electrons violating the Pauli exclusion principle?

A
A box contains an up arrow.
Option A
B
A box contains an up and a down arrow.
Option B
C
A box contains an up and a down arrow.
Option C
D
A box contains an up and a down arrow.
Option D
13

A gas in a rigid container at 25°C has a pressure of 0.96 atm. A change in temperature causes the pressure to increase to 1.25 atm. What is the new temperature of the gas?Use .

Question illustration
A
–44.2°C
B
32.6°C
C
115°C
D
388°C
14

In the molecules below, areas that have a partial negative charge are pink and areas that have a partial positive charge are blue. The attractive force between these two molecules has most likely been produced by

Question illustration
A
covalent bonds.
B
dipole-dipole interactions.
C
dipole-induced dipole interactions.
D
London dispersion forces.
15

Based on the activity series provided, which reactants will form products?F > Cl > Br > I

A
CuI2 + Br2
Option A
B
Cl2 + AlF3
Option B
C
Br2 + NaCl
Option C
D
CuF2 + I2
Option D
16

Which statement is true about crystal lattice energy?

A
It increases as the size of the ions increases.
B
It increases as the charge on the ions decreases.
C
It is the energy that ions absorb when they form a crystal.
D
It is a measure of the strength of the bonds between ions.
17

When chemists convert ethene (C2H2) to ethanol (CH3CH2OH), they have a mixture of the two gaseous substances. Why do chemists then lower the temperature of the mixture?

A
to collect liquid ethene and leave ethanol as a gas because ethene has stronger dipole-dipole forces
B
to collect liquid ethene and leave ethanol as a gas because ethanol has stronger London dispersion forces
C
to collect liquid ethanol and leave ethene as a gas because ethanol has hydrogen bonds
D
to collect liquid ethanol and leave ethene as a gas because ethene has stronger London dispersion forces
18

What is the element Ar classified as in the periodic table?

A
a noble gas
B
a halogen
C
a metalloid
D
a metal
19

In which orbitals would the valence electrons for carbon (C) be placed?

A
s orbital and d orbitals
B
s orbital only
C
p orbitals only
D
s orbital and p orbitals
20

Which task most likely involves a calculation that uses moles?

A
measuring a sugar sample on a balance
B
counting the number of jellybeans in a jar
C
determining the number of atoms in a jar of liquid
D
finding the rate of expansion of a gas-filled balloon

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