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MT Regents Review 2024

Total questions: 105

Worksheet time: 3hrs 59mins

Name
Class
Date
1.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

2.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

3.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

4.

What quantity is the same among atoms of the same element?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of nucleons

5.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

6.

Which elements have the most similar chemical properties?

a)

Ge, As, and Sb

b)

Mn, Fe, and Co

c)

S, Se, and Te

d)

P, S, and Cl

7.

In a bond between an atom of hydrogen and an atom of chlorine, the hydrogen atom has a

a)

weaker attraction for electrons

b)

stronger attraction for electrons

c)

smaller number of first-shell atoms

d)

larger number of first-shell atoms

8.

Which atom has the lowest electronegativity?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

9.

Which temperature is equal to 170 C?

a)

103 K

b)

443 K

c)

-103 K

d)

498 K

10.

Which statement accurately describes particles of an ideal gas, according to the kinetic molecular theory?

a)

The distance between the gas particles is much greater than the size of the particles

b)

As the gas particles collide, the total energy of the system increases

c)

The gas particles have strong intermolecular forces

d)

The gas particles move in a circular motion

11.

What is the overall charge of an ion that has 9 protons, 11 neutrons, and 10 electrons?

a)

+1

b)

-1

c)

+2

d)

-2

12.

Which electron configuration represents the atoms of a bromine atom in the excited state?

a)

2-8-18-7

b)

2-8-18-8

c)

2-8-17-8

d)

2-8-18-7-1

13.

Which formula represents a polar molecule?

a)

Cl2

b)

CH4

c)

HCl

d)

CO2

14.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

15.

When iron is mixed with sulfur, the iron

a)

becomes a covalent compound

b)

retains its magnetic properties

c)

loses its magnetic properties

d)

transfers its magnetic properties to sulfur

16.

As the elements in Group 2 in the periodic table are considered in order of increasing atomic number, there is a general increase in

a)

stability

b)

atomic radius

c)

electronegativity

d)

first ionization energy

17.

How many electron pairs are shared between the atoms in an N2 molecule?

a)

1

b)

2

c)

3

d)

4

18.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

19.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

20.

Under which conditions does a gas behave least like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and low pressure

d)

low temperature and high pressure

21.
What is length?
a)
the amount of matter in an object
b)
the amount of space an object takes up
c)
the distance between two points
d)
the amount of stuff in an object
22.
What is mass?
a)
the distance between two points
b)
the amount of matter (stuff) in an object
c)
the amount of space an object takes up
d)
the distance between three points
23.
What units do we use to measure length?
a)
meters (m)
b)
milliliters (mL)
c)
grams (g)
d)
cubic centimeters (cm3)
24.
What units do we use to measure mass?
a)
milliliters (mL)
b)
liters (L)
c)
centimeters (cm)
d)
grams (g)
25.
What is the length of the line?
a)
2.0 cm
b)
2.3 cm
c)
2.1 cm
d)
3.0 cm
26.
What is the volume of the liquid in this graduated cylinder?
a)
65ml
b)
65.5ml
c)
65.0ml
d)
64.7ml
27.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
28.
Which liquid is the least dense?
a)
oil
b)
water
c)
syrup 
d)
plastic bottle
29.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
30.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
31.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

32.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
33.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
34.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
35.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
36.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
37.
Discovered the nucleus of the atom through the Gold Foil Experiment
a)
Rutherford
b)
Chadwick
c)
Thomson
d)
Dalton
38.
Discovered the electron within the atom
a)
Thomson
b)
Chadwick 
c)
Schrodinger & Heisenberg
d)
Dalton
39.

What subatomic particle has a negative charge and is found outside of the nucleus?

a)

Electron

b)

Proton

c)

Nucleus

d)

Neutron

40.

The majority of an atom's mass exists where?

a)

In the nucleus

b)

In the electron cloud

c)

In the space between the nucleus and the electrons

d)

In the neutrons

41.

An atomic number of 8 means the atom has ________ protons.

a)

7

b)

8

c)

16

d)

88

42.

The mass # tells us the mass of the atom. Which two subatomic particles make up the mass of the atom?

a)

protons and electrons

b)

neutrons and electrons

c)

Kyrontrons and Kytrons

d)

protons and neutrons

43.

What can you do to find the number of neutrons in an atom?

a)

It's the same as the atomic #.

b)

Ask Sierra!

c)

Subtract the atomic # (protons) from the mass # (protons and neutrons)

d)

Multiply the mass # (protons and neutrons) and the atomic # (protons)

44.

The number of electrons is usually the same as the number of protons.

a)

True

b)

False

c)

Only Abraham knows...

45.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

46.

Which of the following is a representation of an ion?

a)

Li

b)

Na-22

c)

O-2

47.

What is the mass number of bromine?

a)

35

b)

45

c)

80

d)

79.904

48.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

49.

What type of atom is this?

a)

Neutral atom

b)

Cation

c)

Anion

d)

Isotope

50.

How does an atom become an ion?

a)

A change in the number of electrons

b)

A change in the number of protons

c)

A change in the number of neutrons

51.

Is this an atom or ion?

a)

atom

b)

Cation

c)

Anion

52.

Different numbers of neutrons causes there to be __________________ of the same elements

a)

ions

b)

mixtures

c)

isotopes

d)

atoms

53.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
54.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
55.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
56.

Which of the following elements LOSES 1 electron in order to attain an octet?

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

57.

Which of the following elements LOSES 2 electrons in order to attain an octet?

a)

lithium

b)

magnesium

c)

helium

d)

sulfur

e)

bromine

58.
What determines the reactivity of an element?
a)
Size of its nucleus
b)
Number of total electrons
c)
Number of valence electrons
d)
Number of shells
59.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass
60.
What group of elements is stable?
a)
halogens
b)
noble gases
c)
alkali metals
d)
alkali earth metals
61.

Electron in the outermost energy level are called?

a)

Valence Electron

b)

Valence Proton

c)

Valence Neutron

62.

The majority of the elements in the periodic table are

a)

Non-Metals

b)

Metals

c)

Metalloids

63.

Elements in the same _________ have the same number of valence electrons.

a)

Period

b)

Group

64.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
65.
What property did Menedleev use to organize his first periodic table?
a)
atomic number
b)
atomic mass
c)
alphabetical order
d)
chemical properties
66.

The period number tells you the number of

a)

protons

b)

energy levels

c)

valence electrons

67.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
68.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
69.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
70.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
71.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
72.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
73.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
74.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
75.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
76.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
77.
What is the charge on an Aluminum ion?
a)
3
b)
+3
c)
+2
d)
+1
78.

What is the name of this instrument, which is used to measure atmospheric pressure?

a)

barometer

b)

thermometer

c)

anemometer

d)

voltmeter

79.

What is the Standard for Temperature and Pressure?

a)

273 K and 1 atm

b)

273 C and 1 kPa

c)

273 F and 1 mmHg

d)

273 K and 1 Torr

80.

What is the name of this instrument, which is used to measure atmospheric pressure?

a)

barometer

b)

thermometer

c)

anemometer

d)

voltmeter

81.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

82.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
83.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
84.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

85.

Absolute zero is

a)

0 K

b)

where there is no molecular movement

c)

the coldest temperature possible

d)

all of these

86.
If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be
a)
250 mL
b)
204 mL
c)
196 mL
d)
160 mL
87.

Which of the following is NOT a property of an ideal gas?

a)

Particles move in random, straight lines

b)

Particles have negligible volume

c)

Particles attract each other strongly

d)

Particles experience no intermolecular forces

88.

Which subatomic particle determines the identity of an element?

a)

Neutron

b)

Electron

c)

Proton

d)

Isotope

89.

Which of the following is NOT a property of metals?

a)

Good conductor of electricity

b)

Lustrous

c)

Malleable

d)

Brittle

90.

What is the atomic number of an element?

a)

The number of protons in the nucleus

b)

The number of electrons in the outer shell

c)

The number of neutrons in the nucleus

d)

The sum of protons and neutrons

91.

Which of the following elements is a halogen?

a)

Magnesium

b)

Neon

c)

Potassium

d)

Chlorine

92.

Which subatomic particle has no electrical charge?

a)

Proton

b)

Electron

c)

Neutron

d)

Positron

93.

What is the maximum number of electrons that can occupy the first energy level (shell) of an atom?

a)

18

b)

32

c)

2

d)

8

94.

Which scientist is credited with discovering the nucleus of the atom?

a)

Bohr

b)

Rutherford

c)

Dalton

d)

Thomson

95.

Which of the following is the best conductor of heat?

a)

Glass

b)

Plastic

c)

Copper

d)

Wood

96.

What is the process called when heat is transferred through direct contact between molecules?

a)

Convection

b)

Radiation

c)

Evaporation

d)

Conduction

97.

Which of the following is NOT a method of heat transfer?

a)

Conduction

b)

Convection

c)

Radiation

d)

Reflection

98.

How much heat is required to raise the temperature of 100 g of water by 10°C? (Specific heat of water = 4.18 J/g°C)

a)

1000 J

b)

4180 J

c)

41.8 J

d)

418 J

99.

Which of the following equations is used to calculate the amount of heat absorbed or released during a temperature change?

a)

Q = mL

b)

Q = nRT

c)

Q = PΔV

d)

Q = mcΔT

100.

If 250 g of a metal at 100°C is placed in 100 g of water at 20°C, which statement is true about the heat exchange?

a)

Both metal and water lose heat

b)

No heat is exchanged

c)

The metal loses heat and the water gains heat

d)

The water loses heat and the metal gains heat

101.

A 2.0 L container holds oxygen gas at 1.5 atm and 300 K. What will the pressure be if the volume is decreased to 1.0 L at constant temperature?

a)

6.0 atm

b)

0.75 atm

c)

3.0 atm

d)

1.5 atm

102.

If the temperature of a gas is doubled (in Kelvin) and the volume remains constant, what happens to the pressure?

a)

It becomes zero

b)

It is doubled

c)

It remains the same

d)

It is halved

103.

A gas occupies 2.5 L at 1.0 atm pressure. If the pressure is increased to 2.0 atm at constant temperature, what will be the new volume of the gas?

a)

0.5 L

b)

1.25 L

c)

2.5 L

d)

5.0 L

104.

A sample of gas occupies 3.0 L at 300 K. If the temperature is increased to 600 K at constant pressure, what will be the new volume?

a)

9.0 L

b)

6.0 L

c)

3.0 L

d)

1.5 L

105.

Which equation is used to relate pressure, volume, and temperature of a fixed amount of gas?

a)

Boyle's Law

b)

Charles' Law

c)

Combined Gas Law

d)

Avogadro's Law

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