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MIDTERM EXAM CHGO15, CHEM1A

Total questions: 60

Worksheet time: 50mins

Name
Class
Date
1.

What branch of science deals with the study of matter and how matter changes?

a)

anatomy

b)

chemistry

c)

paleontology

d)

physics

2.

What is the basic particle that makes up an element?

a)

atom

b)

cell

c)

molecules

d)

particles

3.

What science resource lists all the elements?

a)

balance sheet

b)

microscope guide

c)

periodic table

4.

A scientist is working in the lab, with compounds containing carbon. She is most likely working in the field of?

a)

analytical

b)

biochemistry

c)

organic

d)

physical

5.

atomic number

a)

gas at room temperature, low boiling point

b)

a subatomic particle that has a negative charge

c)

number or protons and neutrons

d)

the number of protons in the nucleus of an atom

6.

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

7.

found in group one of the periodic table; highly reactive

a)

Non-metals

b)

Transition Metals (Groups 3-12)

c)

alkali metals (group 1)

d)

metalloids (semimetals)

8.

neutron

a)

A subatomic particle that has a positive charge and that is found in the nucleus of an atom

b)

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

c)

A subatomic particle that has a negative charge

d)

A small particle in the nucleus of the atom, with no electrical charge

9.

A subatomic particle that has a positive charge and that is found in the nucleus of an atom

a)

Proton

b)

elecrtron

c)

groups

d)

neutrons

10.

A subatomic particle that has a negative charge

a)

nobles gases

b)

protons

c)

electrons

d)

neutrons

11.

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

a)

Non-metals

b)

noble gases

c)

atomic mass

d)

Neutron

12.

Found in group two of the periodic table; highly reactive

a)

period

b)

Alkali Earth Metals (Group 2)

c)

metalloids (semimetals)

d)

alkali metals (group 1)

13.

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

a)

alkali metals (group 1)

b)

Halogens (Group 17)

c)

atomic number

d)

valence electrons

14.

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

15.

Number of protons and neutrons

a)

atomic number

b)

atomic mass

c)

noble gases

d)

Non-metals

16.

Elements that occur in vertical columns on the periodic table.

a)

Neutron

b)

metalloids (semimetals)

c)

groups

d)

Proton

17.

good thermal conductors, shiny, electric conductors, higher density and melting points than group

a)

alkali metals (group 1)

b)

Transition Metals (Groups 3-12)

c)

Non-metals

d)

metalloids (semimetals)

18.

gas at room temperature, low boiling point.

a)

atomic mass

b)

atomic number

c)

Non-metals

d)

noble gases

19.

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

20.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
21.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
22.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
23.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
24.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
25.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
26.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
27.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
28.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
29.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
30.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
31.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
32.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
33.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
34.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

35.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
36.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
37.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
38.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
39.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
40.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
41.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
42.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
43.
All chemical bonds involve two atoms sharing electrons.
a)
True
b)
False
44.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
45.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
46.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
47.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
48.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
49.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
50.
Which type of bond creates a "pool" of electrons between atoms?
a)
Ionic Bonds
b)
Covalent Bonds
c)
Metallic Bonds
d)
Saving Bonds
51.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

52.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

53.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

54.

The spin of an electron is represented by this variable:

a)

n

b)

m

c)

L

d)

s, ms

55.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

56.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

57.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

58.

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

a)

0; f

b)

3; p

c)

1; s

d)

2; d

59.

With each higher energy level, the electrons are

a)

lower in energy

b)

more stable

c)

weaker

d)

farther from the nucleus

60.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

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