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Unit 2 Review

Total questions: 72

Worksheet time: 1hrs 10mins

Name
Class
Date
1.

Which group of the periodic table is composed of inert (not reactive) gases with 8 valence electrons?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

2.

period

a)

Elements that occur in vertical columns on the periodic table.

b)

A horizontal row of elements in the periodic table

c)

Found in group two of the periodic table; highly reactive

d)

A subatomic particle that has a negative charge

3.

not able to conduct heat or electricity, little to no metallic luster

a)

Non-metals

b)

noble gases

c)

atomic mass

d)

Neutron

4.

Halogens (Group 17)

a)

gas at room temperature, low boiling point.

b)

most reactive nonmetals

c)

The electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds

d)

Number of protons and neutrons

5.

metalloids (semimetals)

a)

Elements that occur in vertical columns on the periodic table.

b)

an element that has both metallic and nonmetallic properties

c)

not able to conduct heat or electricity, little to no metallic luster

d)

found in group one of the periodic table; highly reactive

6.
What element is will have the most similar physical and chemical properties to the element Sulfur (S)?
a)
Carbon (C)
b)
Phosphorous (P)
c)
Oxygen (O)
d)
Neon (Ne
7.

This element has two valence electrons and two energy levels?

a)

Beryllium (Be)

b)

Lithium (Li)

c)

Zinc (Zn)

8.

How many valence electrons and energy levels does (Pb) lead have?

a)

4 valence electrons and 6 energy levels (orbitals)

b)

6 valence electrons and 4 energy levels (orbitals)

c)

5 valence electrons and 5 energy levels (orbitals)

d)

5 valence electrons and 10 energy levels (orbitals)

9.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
10.
Which of the following is the most metallic element in period 3?
a)
Boron (B)
b)
Sodium (Na)
c)
Argon (Ar)
d)
Silicon (Si)
11.
Pure forms of these elements are stored in oil so they won't react with oxygen and water in the air.
a)
Alkali Metals
b)
Alkaline-earth metals
c)
Halogens
d)
Noble Gases
12.
All of the actinides are ___________.
a)
stable
b)
radioactive
c)
shiny
d)
named after scientists
13.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
14.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
15.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
16.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

17.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

18.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

19.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

20.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

21.

who discovered the first scientific and systematic periodic table

a)

Henry Mosley

b)

Dmitri Mendeleev

c)

John Dalton

d)

sir Isaac Newton

22.

D block elements are known as .............

a)

Actinides

b)

Transition elements

c)

Lanthanides

d)

Noble gases

23.

choose the wrong statement

a)

Na is more active than Li

b)

O is more active than S

c)

Mg is more active than Al

d)

Cl is more active than F

24.

a grouping of elements based on similar properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

25.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
26.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
27.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
28.

Which element is the most abundant in the earths atmosphere?

a)

Oxygen

b)

argon

c)

phosphorus

d)

nitrogen

29.

Which of the following are allotropes of carbon? Select all that are correct

a)

diamond

b)

cardboard

c)

graphite

d)

coal

30.

Which of the following elements would most likely produce colorful compounds? Select all that are correct

a)

lithium

b)

copper

c)

nickel

d)

aluminum

e)

silicon

31.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
32.
Electronegativity is...
a)
how good an atom is at attracting 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. 
33.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
34.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
35.

As you move down a group, atomic radius increases because -

a)

there is a lower Zeff

b)

there is a higher Zeff

c)

there is more electron shielding

d)

you add more atomic mass

36.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
37.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
38.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
39.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
40.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
41.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
42.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
43.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
44.
Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium
a)
Strontium, Indium, Aluminum
b)
Strontium, Aluminum, Indium
c)
Indium, Aluminum, Strontium
d)
Aluminum, Indium, Strontium
45.

The electronegativity of Cl is the highest in Period 3. Why?

a)

Cl is the largest and has the greatest effective nuclear charge

b)

Cl is the smallest and has the lowest effective nuclear charge

c)

Cl is the largest and has the lowest effective nuclear charge

d)

Cl is the smallest and has the greatest effective nuclear charge

46.

The proper pair of the l value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

47.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

48.

Which of the following is incorrect about the quantum variable m, or ml?

a)

m = -l...l

b)

the value for p is -1, 0, 1

c)

when l is 2, there are 5 values for m

d)

the value is either +1/2 or -1/2

49.

Which set of Quantum numbers is not allowed

a)

(3,1,1,-1/2)

b)

(2,1,-2,+1/2)

c)

(4,2,-1,-1/2)

50.

If n = 2, what are the allowed values of l? Tick all that apply:

a)

0

b)

1

c)

2

d)

3

51.

For l = 2, tick the possible values of ml

a)

-2

b)

-1

c)

0

d)

1

e)

2

52.
Electormagnetic radiation travels through a vacuum at a speed of 
a)
186,000 m/s.
b)
125 m/s
c)
3.00 x 108 m/s
d)
It depends on the wavelength
53.

Light acts like

a)

a wave.

b)

a particle.

c)

Both a wave and a particle

d)

neither a wave nor a particle.

54.

This image is an illustration of

a)

photoelectric effect

b)

diffraction effect

c)

particle interference effect

d)

wave interference effect

55.

The ‘Photoelectric effect’ is where electrons, called photoelectrons are emitted from a metal’s surface when light of a certain frequency, or higher shines on it.

a)

True

b)

False

56.

 Calculate the wavelength of light that has a frequency of 5.2 x 1012 1/s. The speed of of light is 3.0x 108 m/s.

a)
5.8 x 10 -5 m
b)
5.8 x 10 -7 m
c)
5.19 x 10 14 m
d)
1.56 x 10 23 m
57.

If an AM radio station broadcasts at

9.95 x 105 Hz, what is the wavelength of this radiation?

a)

6.59 x 10-28 m

b)

1.01 x 10-6 m

c)

3.32 x 10-3 m

d)

302 m

58.

The energy of a photon having a frequency of 4.62 x 1014 s-1 is

a)

1.43 x10-48 J

b)

3.06 x 10-19 J

c)

6.79 x 1058J

d)

3.06 x 10-18J

59.

Blue light has a wavelength of 440 nm. How much energy does a photon of blue light have?

a)

9.72 x 10-49J

b)

4.51 x 10-17J

c)

4.51 x 10-18J

d)

4.51 x 10-19J

60.

What is the decrease in the attraction between an electron and the nucleus in an atom with more than one electron level?

a)

shielding effect

b)

effective nuclear charge

c)

ionization energy

d)

electronegativity

61.

What is this element?  1s22s22p63s23p64s23d104p6

a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
62.

What atom matches this electron configuration?

[Xe] 6s1 4f14 5d10

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

63.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
64.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
65.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
66.

Which electron configuration belongs to Copper (Cu)?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s1 3d10

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

67.
How many valence electrons does Calcium have? How many energy levels does Calcium have?
a)
2 valence: 4 energy levels 
b)
20 valence:  4 energy levels 
c)
4 valence: 2 energy levels 
d)
2 valence: 3 energy levels 
68.

Ca forms ions with a charge of _______.

a)

+1

b)

+2

c)

-1

d)

-2

69.

N forms ion with a charge of _______.

a)

+3

b)

-3

c)

+2

d)

-2

70.

S has ____ valence electrons and form ions with a charge of _______.

a)

6, -2

b)

6, -1

c)

7, +1

d)

6, +2

71.

F has _____ valence electrons and form ions with a charge of ________.

a)

6, -2

b)

7, -1

c)

1, +1

d)

2, +2

72.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

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