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Unit 4 Test Review 7th Grade Chem

Total questions: 50

Worksheet time: 25mins

Name
Class
Date
1.

0.007980 kg has how many sig figs?

a)

6

b)

5

c)

4

d)

3

2.

6.02 g- 6.000 g= ? use sig figs

a)

0.002 g

b)

0.1g

c)

0.02 g

d)

0.00 g

3.

17 m X 0.00458 m=? use sig figs

a)

0.0078 m

b)

0.07786 m

c)

0.077 m

d)

0.0779 m

4.

Gases can be

a)

compressed

b)

no definite volume

c)

take the shape of anything

d)

high energy

e)

all of the above

5.

This is an example of a physical change

a)

a nail rusts

b)

water changes states

c)

fire cracker exploades

d)

a color forms when mixing two acids

6.

Which of these is NOT a sign that a chemical change has occured?

a)

Solid forms

b)

Color changes

c)

change in states

d)

Bubbles and a smell form

7.

Which is not a physical property

a)

luster

b)

malleability

c)

melting point

d)

reactivity

8.

In an exothermic reaction

a)

heat is absorbed in the form of energy

b)

energy is released in the form of heat

c)

temperature stays the same

d)

no energy is needed

9.

This is an example of

a)

a mixture of compounds

b)

a mixture of elements

c)

a mixture of pure substances

d)

a compound

10.

I am an element and I have 72 protons. Who am I?

a)

Ta

b)

Hf

c)

Rf

d)

Ge

11.

What is the mass number of Tungsten-186

a)

184

b)

183.84

c)

74

d)

186

12.

How many electrons does 114Be2+ have?

a)

2

b)

4

c)

11

d)

7

13.

How many neutrons does 114Be2+ have?

a)

2

b)

4

c)

11

d)

7

14.

Which group has 7 valence electrons?

a)

Alkali metals

b)

Alkaline earth metas

c)

Oxygen Family

d)

Halogens

15.

Elements in period___ have 86 core electrons

a)

4

b)

5

c)

6

d)

7

16.

Which group of elements contain the most reactive metals

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

lanthanides

17.

This picture represents what orbital?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

18.

Which electron configuration accurately represents Silicon?

a)

1s22s22p63s23p3

b)

1s22s22p63s23p2

c)

1s22s22p63s23d3

d)

1s22s22p63s13p2

19.

1s22s22p63s23p64s23d3

a)

Ti

b)

Cr

c)

V

d)

P

20.

An element with the electron configuration [Xe]6s1 belongs to what family?

a)

alkali metals

b)

alkali earth metals

c)

transition metals

d)

noble gases

21.

The d-orbital can hold a maximum of ___ electrons

a)

2

b)

6

c)

10

d)

14

22.

Hunds rule tells us

a)

You have to fill each orbital with two electrons before you go to the next one

b)

You have to fill every orbital with 1 electron before you fill it with a second

c)

The electrons have to be opposite spin

d)

Fill the electrons starting with the lowest energy orbital

23.

Which of these groups forms metal oxides?

a)

Alkaline earth metals

b)

noble gasses

c)

transition metals

d)

halogens

24.

[Rn]7s2 is the correct electron configuration for:

a)

Radium

b)

Radon

c)

Francium

d)

Lanthanum

25.

The electron configuration of an atom is 1s22s22p63s23p3. The atomic number of the atom is

a)

15

b)

11

c)

5

d)

3

26.

Of the orbitals shown, the one with the lowest energy is

a)

1d

b)

3s

c)

2s

d)

2p

27.

The third ionization energy would be ___ the first ionization energy.

a)

>

b)

<

c)

=

d)

≥

28.

Which atom has the lowest first ionization energy?

a)

Br

b)

At

c)

Cl

d)

I

29.

Which of the following elements has the largest atomic radius?

a)

O

b)

P

c)

Ge

d)

In

30.

Which ion is represented by the following electron configuration: 1s22s22p6?

a)

Ne

b)

Cl-

c)

F-

d)

K+

31.

Put the following in order of increasing ionization energy: Ne, Fr, S, As. And Ba.

a)

S,As, Ba, Fr, Ne

b)

Ne, S, As, Br, Fr

c)

Fr, Ba,As,S,Ne

d)

Ne, Fr, S, As,Ba

32.

Arrange the following elements in order of increasing electronegativity: S, Li, Zn, Xe, Cl

a)

Li, Zn, S, Cl, Xe

b)

Xe, Li, Zn, S, Cl

c)

Cl, Xe, Zn, Li, S

d)

Zn, Li, S, Cl, Xe

33.

Metals typically have _____ 1st ionixation energyies.

a)

No

b)

High

c)

Negative

d)

Low

34.

Rank the following elements in order of increasing atomic radius: Al, C, N

a)

Al < C < N

b)

C< Al < N

c)

C < N < Al

d)

N < C < Al

35.

Which of the following atoms or ions has the largest radius?

a)

F

b)

O

c)

S

d)

S2-

36.

Which of the following has the highest electronegativity value?

a)

F

b)

Br

c)

Cl

d)

I

37.

Group 17 elements form:

a)

2+ anions

b)

2- anions

c)

1+ anions

d)

1- anions

38.

The most nonmetallic metal is

a)

Aluminum

b)

Silicon

c)

Iron

d)

Zinc

39.

[Kr] 5s2 4d10 5p5 is the electron configuration for:

a)

Bromine

b)

Technetium

c)

Iodine

d)

Manganese

40.

Cations are __ the neutral element and anions are __ the neutral element.

a)

The same size as; larger than

b)

Smaller than; smaller than

c)

Larger than; smaller than

d)

smaller than; larger than

41.

Which of the following would have the largest ionic radii?

a)

Ba2+

b)

Li+

c)

F-

d)

Ca2+

42.

The number of electron shells:

a)

Decreases as you move down the groups and does not change across the periods

b)

Increases as you move down the groups and does not change across the periods

c)

Does not change as you move down the groups and increases across the periods

d)

Does not change as you move down the groups and decreases across the periods

43.

The correct electron configuration for Selenium is:

a)

[Ar] 4s23d104p4

b)

[Ar] 3d104s24p4

c)

1s22s22p63s23p63d104s24p4

d)

both a and c are correct

44.

A S2- ion has how many electrons?

a)

14

b)

16

c)

18

d)

30

45.

The equation Mg+(g)→Mg2+ (g) + e- best represents the:

a)

First ionization energy of magnesium

b)

Third ionization energy of magnesium

c)

Electronegativity reaction of magnesium

d)

Second ionization energy of magnesium

46.

Which of the sets of ions below has the same electron configuration as Neon

a)

Al3+, Li+, O2-

b)

S2-, Cl-, K+

c)

O2-, F-, Na+

d)

P3-, S2-, Mg2+

47.

An element has an atomic mass of 15.999g/mol. The element is:

a)

Potassium

b)

Lithium

c)

Oxygen

d)

Sulfur

48.

Aufbau's principal tells us...

a)

to fill each orbital with 2 electrons

b)

fill the orbitals starting with the lowest energy

c)

Opposite spin of electrons

d)

Fill each orbital with 1 electron and then a second

49.

Which group of elements are good catalysts?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Lanthanides

50.

Which group takes the 5f orbital?

a)

Transition metals

b)

noble gases

c)

Halogens

d)

Lanthanides

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