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Unit 1 Chemistry AS

Total questions: 125

Worksheet time: 3hrs 42mins

Name
Class
Date
1.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
2.
Which of the following is a compound?
a)
Co
b)
O2
c)
C
d)
CO2
3.
Which of the following is NOT an element?
a)
H2O
b)
H2
c)
O2
d)
Au
4.
When trying to identify an unknown element, a scientist determines what other elements the unknown element reacts with chemically. Which property of the unknown element determines the other elements it reacts with?
a)
The total number of neutrons in the unknown element
b)
The total number of particles in the nucleus of the unknown element
c)
The number of protons in the nucleus of the unknown element
d)
The number of valence electrons in the unknown element
5.
Which of these formulas contain equal numbers of nitrogen atoms?
a)
Formulas I and III
b)
Formulas I and IV
c)
Formulas II and III
d)
Formulas I, II, and V
6.
How many atoms are represented in the reactants of this equation?
a)
6
b)
12
c)
24
d)
36
7.

When 0.23 g of sodium, Na is added to water, the metal will react vigorously at the surface of the water, find the mass sodium hydroxide, NaOH produced.

RAM Na= 23, O= 16 , H= 1

a)

0.2g

b)

1.3g

c)

0.4g

d)

4.7g

8.

1.12 g of Iron burns completely in chlorine. What is the mass of the product. RAM [ Cl= 35.5, Fe = 56]

a)

0.38

b)

3.25

c)

4.88

d)

6.50

9.

3.84 g of magnesium was burnt in oxygen gas to produced magnesium oxide in a laboratory. Find the mass of magnesium oxide produced.

[Relative atomic mass: Mg, 24; O, 16]

a)

10.7g

b)

5g

c)

12.8g

d)

6.4 g

10.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
11.
How many  atom's of oxygen are in Al₂(SO₄)₃?
a)
4
b)
12
c)
7
d)
24
12.
How many atom's of Hydrogen are in 3(NH₄)₂CrO₄
a)
4
b)
2
c)
8
d)
24
13.
What is the name of the group that never reacts-- they are stable with a full outermost ring!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
14.
What coefficient should go in the blank space to balance the chemical equation? 
2Al  +  _____HCl   →    2AlCl3  +  3H2
a)
2
b)
4
c)
3
d)
6
15.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
16.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
17.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
18.
What is oxidation number of H in CaH2?
a)
+1
b)
-1
c)
0
d)
+2
19.

What is the precipitate formed when you mix silver nitrate with copper chloride?

a)

copper nitrate

b)

copper chloride

c)

silver chloride

d)

silver nitrate

20.
What is the precipitate formed between potassium bromide and ammonium sulfide
a)
potassium sulfide
b)
ammonium bromide
c)
potassium ammonium
d)
no ppt is formed
21.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
22.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
23.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
24.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
25.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
26.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
27.
How many neutrons does uranium-235 have?
a)
238
b)
92
c)
146
d)
143
28.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
29.
which explanation of this notation is correct?
a)
 12 is proton #
b)
6 tells you there are 6 neutrons
c)
6 tells you there are 6 protons
d)
12 is not a mass # here
30.
Barium atoms want to form...
a)
an anion
b)
a cation
c)
an onion
d)
a cuddly kitten friend
31.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
32.
What is the charge does a sodium ion have?
a)
+2
b)
+1
c)
-1
d)
-2
33.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
34.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
35.
Alpha particles.....
a)
a) are positively charged.
b)
b) consist of two protons and four neutrons.
c)
c) can penetrate any thickness of matter
d)
d) All of the above 
36.
The type of radioactive particle that can be stopped by a sheet of paper is the ____.
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
uranium
37.
The most penetrating type of radiation is the ____.  
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
38.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
39.
The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?
a)
100.0g
b)
50.0g
c)
12.5g
d)
8.5g
40.
After the third half-life, how much of the sample is left?
a)
1/2
b)
1/3
c)
1/16
d)
1/8
41.
Barium-122 has a half-life of 2 minutes. A fresh sample weighing 80 g was obtained. If it takes 10 minutes to set up an experiment using barium-122, how much barium-122 will be left when the experiment begins?
a)
0.25g
b)
2.5g
c)
25g
d)
80g
42.
Unstable isotopes undergo radioactive decay. What occurs during radioactive decay? 
a)
Unstable isotopes collapse in on themselves. 
b)
The electrons in unstable isotopes constantly move to higher energy levels within the electron cloud. 
c)
Unstable isotopes release charged particles. 
d)
 Unstable isotopes capture charged particles from other atoms
43.
What type of particle is released during beta decay? 
a)
Nucleus
b)
Neutron
c)
Proton
d)
Electron
44.
 For the following nuclear reaction, what was the beginning radionuclide (X)?
      X  →   86Rn222 + 2He4 
a)
Radium-222
b)
Radon-222
c)
Radon-226
d)
Radium-226
45.

1s2 2s2 2p6 3s2 3p3


Atoms of an element, X, have the electronic con­figu­ration shown above. The compound most likely formed with magnesium, Mg, is:

a)

Mg3X2

b)

Mg2X

c)

MgX2

d)

MgX3

46.

Which atom below contains exactly two unpaired electrons?

a)

Ni

b)

Ca

c)

P

d)

I

47.

The table shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend?

a)

The atomic radius of oxygen is greater than the atomic radius of fluorine.

b)

The atomic radius of oxygen is less than the atomic radius of nitrogen.

c)

There is repulsion between paired electrons in oxygen’s 2p orbitals.

d)

There is attraction between paired electrons in oxygen’s 2p orbitals.

48.

The ionization energies for element X are listed in the table on the right. On the basis of the data, element X is most likely to be

a)

Be

b)

B

c)

C

d)

F

49.

For element X represented above, which of the following is the most likely explanation for the large difference between the second and third ionization energies?

a)

The effective nuclear charge decreases with successive ionizations.

b)

The shielding of outer electrons increases with successive ionizations.

c)

The electron removed during the third ionization is, on average, much closer to the nucleus than the first two electrons removed were.

d)

The ionic radius increases with successive ionizations.

50.

Which of these configurations correctly shows an atom in an excited state?

a)

1s2 2s2 2p6 3s2 3p6 4s3

b)

1s2 2s2 2p6 3s2 3p5

c)

1s2 2s2 2p6 3s1 3p6

d)

1s2 2s2 2p6 2d10

51.

What are the trends of electronegativity across the period and down the group?

a)

across the period = electronegativity decreases

down the group = electronegativity decreases

b)

across the period = electronegativity inreases

down the group = electronegativity increases

c)

across the period = electronegativity increases

down the group = electronegativity decreases

d)

across the period = electronegativity decreases

down the group = electronegativity increases

52.

It is even easier to pull away a second electron from a sodium atom compared to pulling away the first electron.

a)

true

b)

false

53.

Why do group 1 elements have the lowest first ionization energy?

a)

because they have the fewest shells

b)

because they are happy to lose their electron

c)

because they have the fewest protons

d)

because they are very happy to keep all their electrons

54.

What causes the decrease in the radius of an atom as we go across the period

a)

increase in number of electrons

b)

increase in number of neutrons

c)

increase in number of protons

d)

increase in number of shells

55.

Which of the following metals will be the most reactive (meaning that it is easiest to pull away its electron)

a)

Caesium (Cs)

b)

Sodium (Na)

c)

Rubidium (Rb)

d)

Lithium (Li)

56.
What are the steps of operation in the mass spectrometer?
a)
Accelerate, Deflect,Ionize, Detect
b)
Deflect,Ionize, Accelerate, Detect
c)
Ionize, Accelerate, Deflect, Detect
d)
Detect, Accelerate, Deflect, Ionize
57.
How many isotopes are shown in this mass spectrum?
a)
1
b)
84
c)
86
d)
4
58.
A sample of pure chlorine gas is analyzed in the MS. Which of the following is a correct interpretation?
a)
Chlorine has an isotope with a mass of 70 amu
b)
Chlorine has three known isotopes
c)
Chlorine is diatomic
d)
Chlorine is highly reactive
59.
Based on the mass spectrum, which isotope of chlorine is most abundant?
a)
35Cl
b)
37Cl
c)
70Cl
d)
72Cl
60.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
61.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
62.
How can you figure out how particles (atoms) there are in 2 moles?
a)
2
b)
2 x (6.02 x 1023)
c)
2 x (atomic mass)
d)
2 ÷ (6.02 x 1023)
63.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
64.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
65.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
66.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
67.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
68.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
69.
What do you do when you get a half in the ratio?
a)
add 2 to each element
add two to only the one with the half
b)
multiply the one with the half only by two
c)
multiply all of them by two
d)
add two to all of the ratios
70.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements. (keep two decimal places throughout calculations)
a)
SO
b)
SO2
c)
SO3
d)
SO4
71.
The ideal gas law is an equation that relates the  what  variables to a constant of R.
a)
volume, pressure, temperature
b)
volume, temperature, pressure, amount of gas particles
c)
volume, pressure
d)
volume, temperatue
72.
When using PV = nRT, it is important to use the units for pressure, volume and temperature as
a)
atm, L, K
b)
atm, ml, C
c)
mmHg, L, K
d)
mmHg, ml, K
73.
The amount of gas is measured in the units called
a)
grams
b)
quantities
c)
moles
d)
none of the above
74.
What is the volume in this burette?
a)
24.1mL
b)
24.3mL
c)
24.2L
d)
24.2mL
75.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
76.
What is the endpoint of a titration
a)
Where the amount of acid and base are equal as shown by a colour change 
b)
Where there is no base
c)
When the volume of base in the burette is used up 
d)
When there is no acid
77.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
78.
What are the products of the neutralization shown below?
Ca(OH)2  +  H2CO3  -->  
a)
H2O  +  Ca2CO3
b)
CaO +  CO3
c)
H2O  +  CaCO3
79.
Acid + Base ₋--> 
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
80.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
81.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
82.

What is shown by a half reaction

a)

neutralization of an ion or molecule

b)

oxidation or reduction of an element

c)

decomposition of an ion or molecule

d)

none of the abve

83.

Which element is the reducing agent in the following?

Na + KCl= NaCl + K

a)

None

b)

Na

c)

K

d)

Cl

84.

Who is the oxidizing agent in the following?

F2 + LiBr = LiF + Br2

a)

None

b)

F

c)

Li

d)

Br

85.

What is the oxidation number for P in H3PO4?

a)

3

b)

4

c)

5

d)

6

86.

Oxidation is

a)

lose of oxygen

b)

gaining electrons

c)

gaining Hydrogen

d)

losing electrons

87.

What is lost or gained in a redox reaction?

a)

atoms

b)

ions

c)

protons

d)

electrons

88.

Which of the following is a oxidation half-reaction.

a)

Fe+3 + e = Fe+2

b)

Cl2 + 2e = 2Cl-

c)

O2 + 4H+ + 4e = 2H2O

d)

Sn+2 = Sn+4 + 2e

89.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
90.
Which of the following is the balanced half -reaction for the oxidation of Cu to Cu+2?
a)
Cu   --> Cu+2
b)
Cu + 2 e-   --> Cu+2
c)
Cu  --> Cu+2  + 2 e-
d)
Cu - 2e-  --> Cu+2
91.
     In the reaction Zn + H2O → ZnO2 + H2
 which element, if any, is oxidized?
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
92.
Which are examples of reduction?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
93.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
94.
This electrode loses mass 
a)
anode
b)
cathode
95.
Reduction happens at the 
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
96.
What is formed when sodium reacts with water?
a)
sodium oxide and hydrogen
b)
sodium hydroxide and hydrogen
c)
sodium hydroxide and oxygen
d)
sodium hydroxide and carbon dioxide
97.
What is formed when sodium reacts with water?
a)
sodium oxide and hydrogen
b)
sodium hydroxide and hydrogen
c)
sodium hydroxide and oxygen
d)
sodium hydroxide and carbon dioxide
98.

...... is released when alkali metal react with water.

a)

Hydrogen

b)

Oxygen

c)

Metahne

d)

Carbon di oxide

99.

Alkali earth metals are found in which group of the periodic table?

a)

Group 1

b)

Group 2

c)

Group 7

d)

group 8

100.

What is the flame color of Barium metal or Barium containing compound when they are burned?

a)

Blue

b)

Red

c)

Green

d)

Yellow

101.
Water is polar because...
a)
The unequal sharing of electrons gives the water molecule a slight negative charge near its oxygen atom and a slight positive charge near its hydrogen atoms.
b)
The molecule has two poles, at which the it is colder than other regions of the molecule.
c)
The unequal sharing of electrons gives the water molecule a slight negative charge near its hydrogen atoms and a slight positive charge near its oxygen atom.
d)
The water molecule is neutral.
102.

Would carbon dioxide dissolve in water or carbon tetrachloride?

a)

water

b)

carbon tetrachloride

103.

Would methane, CH4, dissolve in water or carbon tetrachloride?

a)

water

b)

carbon tetrachloride

104.

Which "Halogen" can able to replace Chlorine in Sodium Chloride?

a)

Flourine

b)

Bromine

c)

Iodine

d)

Astatine

105.

which statement is true about halogens?

a)

form covalent compounds with other non-metallic elements

b)

A less reactive halogen will displace a more reactive element form its ionic salt

c)

Form ionic compound with hydrogen

d)

form negative ion of charge -2

106.

silver nitrate is added to an aqueous solution containing Br- to give a precipitate X, which is then tested for its solubility in concentrated ammonia. which of the following correctly describes the the colour of X and its solubility in ammonia.

a)

white insoluble

b)

cream slightly soluble

c)

white slightly soluble

d)

yellow insoluble

107.

An excess of aqueous solution of silver nitrate is added to an aqueous solution containing both potassium chloride and potassium bromide. the precipitate formed is the filtered off and washed with distilled water. The precipitate is then shaken with aqueous ammonia and filtered off again.which ion does the final filtrate contain?

a)

chloride

b)

silver

c)

iodide

d)

potassium

108.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
109.
What is the function of iron in the Haber process?
a)
It shifts the position of equilibrium towards the products.
b)
It decreases the rate of the reaction.
c)
It provides an alternative reaction pathway with a lower activation energy.
d)
It reduces the enthalpy change of the reaction.
110.
Which statement about chemical equilibria implies they are dynamic?
a)
The position of equilibrium constantly changes.
b)
The rates of forward and backward reactions change.
c)
The reactants and products continue to react.
d)
The concentrations of the reactants and products continue to change.
111.
What will happen when at a constant temperature, more iodide ions, I–, are added to the equilibrium below?
I2(s) + I–(aq) <-->  I3–(aq)
a)
The amount of solid iodine decreases and the equilibrium constant increases.
b)
The amount of solid iodine decreases and the equilibrium constant remains unchanged.
c)
The amount of solid iodine increases and the equilibrium constant decreases.
d)
The amount of solid iodine increases and the equilibrium constant remains unchanged.
112.
An increase in temperature increases the amount of chlorine present in the following equilibrium.
PCl5(s) <->  PCl3(l) + Cl2(g)
What is the best explanation for this?
a)
The higher temperature increases the rate of the forward reaction only.
b)
The higher temperature increases the rate of the reverse reaction only.
c)
The higher temperature increases the rate of both reactions but the forward reaction is affected more than the reverse.
d)
The higher temperature increases the rate of both reactions but the reverse reaction is affected more than the forward.
113.
Consider the following reversible reaction.
Cr2O72–(aq) + H2O(l) <-> 2CrO42–(aq) + 2H+(aq)
What will happen to the position of equilibrium and the value of Kc when more H+ ions are added at constant temperature?
a)
eqm shifts to the left and Kc decreases
b)
eqm shifts to the right and Kc increases
c)
eqm shifts to the right and Kc does not change
d)
eqm shifts to the left and Kc does not change
114.

True or false: a neutral solution has equal amounts of H+ and OH-.

a)

True

b)

False

115.
ammonia
a)
base
b)
acid
116.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
117.

What is the formula for nitric acid?

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

118.
BASE + ACID ----> SALT +?
a)
water
b)
oxygen
c)
hydrogen ion
d)
hydroxide ion
119.
The pH of a 0.001 M solution of HCl is 
a)
11
b)
3
c)
-3
d)
-11
120.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
121.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
122.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
123.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

124.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
125.

What is the endpoint of a titration

a)

Where the amount of acid and base are equal as shown by a color change

b)

Where there is no base

c)

When the volume of base in the burette is used up

d)

When there is no acid

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