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All about the Electron

Total questions: 62

Worksheet time: 54mins

Name
Class
Date
1.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
2.
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
3.
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
4.
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)
5.
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. 
6.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
7.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
8.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
9.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
10.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
11.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

12.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

13.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
14.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
15.

Boron has 3 valence electrons but it wants a full shell, what charge does it like to form?

a)

3-

b)

3+

c)

5-

d)

5+

16.

Oxygen has 6 valence electrons but wants a full shell. What charge does nitrogen tend to form?

a)

6+

b)

2-

c)

6-

d)

2+

17.

This is a correct dot diagram for oxygen (O)?

a)

true

b)

false

18.

What element does this Lewis Dot Digram represent?

a)

Li

b)

Al

c)

C

d)

Be

19.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
20.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
21.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
22.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
23.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
24.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
25.
 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
26.

Ionic bonding involves

a)

transfer of electrons

b)

sharing of electrons

c)

holding onto electrons

d)

electrons are not involved

27.

What do atoms that form positive ions tend to do?

a)

lose electrons

b)

gain electrons

c)

lose protons

d)

gain protons

28.

What usually forms a positive ion?

a)

metal

b)

nonmetal

c)

metalloid

d)

there is no way to tell

29.

Covalent compounds

a)

contain a sea of electrons

b)

share electrons

c)

transfer electrons

d)

conduct electricity

30.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

31.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

32.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

33.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

34.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

35.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

36.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

37.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

38.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

39.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
40.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
41.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
42.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
43.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
44.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
45.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
46.
Diatomic elements are defined as IDENTICAL elements that bond with each other (i.e. Oxygen with Oxygen).  What type of bond should they form?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals force
47.

In a polar covalent bond, electrons are shared:

a)

equally

b)

unequally

c)

between two metals

d)

between a metal and a non-metal

48.

Classify the following molecule.

a)

polar

b)

nonpolar

49.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
50.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
51.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
52.
 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
53.

Which type of molecular shape is shown by this molecule?

a)

trigonal pyramidal

b)

tetrahedral

c)

bent

d)

trigonal planar

54.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
55.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

56.

Which intramolecular force has the greatest strength?

a)

ionic bond

b)

nonpolar covalent

c)

polar covalent

d)

metallic

57.

Which of these is the weakest intermolecular force?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

58.

Which intermolecular force do all molecules have?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

59.

Which intermolecular force is characterized by partially oppositely charged ions?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

60.

Which type of intermolecular force does this molecular drawing best represent?

a)

dipole-dipole

b)

hydrogen bonding

c)

London dispersion forces

61.

Which of these molecules are polar? (You may choose multiple answers)

a)

a

b)

b

c)

c

d)

d

62.

One of these molecules is polar. Predict which molecule would have Dipole-dipole forces.

a)

a

b)

b

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