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Q#2 Chemistry Regents review

Total questions: 50

Worksheet time: 2hrs 57mins

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 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

7.

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

8.
The mass of a proton is approximately equal to the mass of
a)
an alpha particle
b)
a beta particle
c)
a neutron
d)
a positron
9.

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

10.

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

11.

An atom that has 8 protons and 10 neutrons and 6 electrons is an ion of the what element?

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

12.

What part of the atom determines the identity of an atom?

a)

Electrons

b)

Neutrons

c)

Protons

d)

Nucleus

13.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

14.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

15.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

16.
The most dangerous type of radiation is the ____. 
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
17.

What is the charge of a neutron?

a)

+1

b)

-1

c)

0

d)

+2

18.

Which scientist is known for the discovery of the nucleus?

a)

Bohr

b)

Rutherford

c)

Thomson

d)

Dalton

19.

An atom that has 7 protons, 7 neutrons and 10 electrons is an ion of what element?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

20.

The elements on the Periodic Table are arranged in

order of increasing

a)

atomic mass

b)

atomic number

c)

molar mass

d)

oxidation number

21.

Which term represents the strength of the attraction an

atom has for the electrons in a chemical bond?

a)

electrical conductivity

b)

electronegativity

c)

first ionization energy

d)

specific heat capacity

22.

Which term represents the amount of energy required

to remove the most loosely bound electron from an

atom in the gaseous state?

a)

atomic radius

b)

electronegativity

c)

First ionization energy

d)

electrical conductivity

23.

As the elements in Period 2 of the Periodic Table are

considered in order from left to right, which property

generally decreases?

a)

atomic radius

b)

electronegativity

c)

ionization energy

d)

nuclear charge

24.

Which sequence correctly places the elements in order

of increasing ionization energy?

a)

H -> Li -> Na -> K

b)

I -> Br -> Cl -> F

c)

O -> S -> Se -> Te

d)

H -> Be -> Al -> Ga

25.

In a given period of the Periodic Table, the element

with the lowest first ionization energy is always in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

26.

Which of these elements has physical and chemical

properties most similar to silicon (Si)?

a)

germanium (Ge)

b)

lead (Pb)

c)

phosphorus (P)

d)

chlorine (Cl)

27.

As the atomic number of elements within Group 2

increases, the metallic character of each successive

element

a)

decreases

b)

increases

c)

remains the same

28.

How much energy is required to remove the most

loosely bound electron from a neutral atom of neon

in the gaseous phase?

a)

363 kJ

b)

441 kJ

c)

1086 kJ

d)

2081 kJ

29.

Which atom has the greatest attraction for the

electrons in a chemical bond?

a)

hydrogen

b)

oxygen

c)

silicon

d)

sulfur

30.

Which element is a noble gas?

a)

Argon

b)

chlorine

c)

hydrogen

d)

magnesium

31.

The element helium is classified as a

a)

metal

b)

metalloid

c)

noble gas

32.

An atom of which element has the largest atomic

radius?

a)

Fe

b)

Mg

c)

Si

d)

Zn

33.
A nuclear reaction where a nucleus splits into two smaller nuclei is... 
a)
Fission
b)
Fusion
c)
Gamma decay
d)
Beta decay
34.
What would two different isotopes of an atom have in common?
a)
Number of neutrons 
b)
Number of protons
c)
Atomic weight 
d)
Atomic mass
35.
What happens when the number of protons in an atom changes? 
a)
The number of electrons changes too 
b)
Usually nothing happens, unless the atom is radioactive 
c)
The atomic nucleus explodes
d)
It becomes a completely different atom, with different properties 
36.
What element is the ?
a)
Ag-115
b)
Cd-115
c)
Pd-115
d)
Not Listed
37.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
38.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
39.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
40.
Negatively charged particles found outside of the nucleus are called
a)
electron
b)
protons
c)
neutrons
d)
nucleons
41.
Positively charged particles found in the nucleus of an atom are called
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
42.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Combustion
43.
When nuclei decay, massive amounts of __________ is released.
a)
energy
b)
jello
c)
protons
d)
neutrons
44.
What type of reaction is this?
a)
alpha
b)
beta
c)
gamma
d)
quiet
45.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

46.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

47.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

48.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

49.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

50.

Place the following atomic models in order, from earliest to latest:


A) Rutherford B) Thomson C) Dalton

a)

B, C, A

b)

C, A, B

c)

A, C, B

d)

C, B, A

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