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Worksheets2 Forces & Polarity
Total questions: 29
Worksheet time: 28mins
Name
Class
Date
1.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
2.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
3.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
4.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
5.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
6.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
7.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
8.
Covalent bond is equal sharing of electron. Polar covelent bond is
a)
unequal sharing of electrons
b)
different distribution of electrons
c)
presence of hydrogen bonding
d)
presence of polar atoms
9.
Define electronegativity
a)
ability to donate electron
b)
tendency to lose electron
c)
tendency to lose electron to its neighbor
d)
tendency of atom to attract shared electron to itself
10.
Polarity of a molecule is determined by
a)
shape and charge
b)
shape and difference in EN value
c)
difference in EN value and size
d)
difference in EN value and charges
11.
CCl4 has polar bonds but is a non polar molecule. Why?
a)
bond polarity exist between atoms
b)
bond polarity between atoms cancel
c)
dipole moment exist between atoms in molecule
d)
difference in EN between C and Cl
12.
HCCl3 is a polar molecule with polar bonds. Why?
a)
it has an asymmetrical shape
b)
bond polarity between atoms cancel
c)
net dipole moment exist between atoms in molecule
d)
difference in EN between C and Cl
13.
CO2 has polar bonds but is a NON POLAR molecule. Why?
a)
it has an asymmetrical shape
b)
bond polarity between C and O atoms cancel
c)
net dipole moment exist between atoms in molecule
d)
bond polarity exist between C+ and O-
14.
Which of the following is FALSE about intermolecular forces between molecules?
a)
It is also called London or Van Der Waals forces
b)
Dipole dipole attraction between molecule
c)
Also due to instantaneous dipole attraction between molecule
d)
Must have permanent dipole moment before it can exist
15.
The following statement is true for hydrogen bonding EXCEPT
a)
It is a dipole dipole forces of attraction
b)
Electronegative element like N, O and F must be present
c)
Hydogen bonding is stronger than covalent bonding
d)
ESF attraction bet H atom with lone pair electron from N,O,F
16.
Why BCI3 is non polar while NCI3 is polar?
a)
BCI3 is symmetrical and bond polarity exist
b)
BCI3 does not have polar bonds, while NCI3 does
c)
BCI3 is asymmetrical and bond polarity exist
d)
BCI3 is symmetrical and bond polarity cancel
17.
A substance made of two or more atoms that are joined together.
a)
molecule
b)
element
c)
meniscus
d)
atom
18.
HCN is a linear molecular geometry. What is the polarity of HCN molecule?
a)
Polar molecule
b)
Non-polar molecule
19.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
20.
True or False
Attractions between polar molecules are Weaker than attractions between nonpolar molecules.
a)
True
b)
False
21.
The two (2) factors that determine if a molecule is Polar or Non-polar:
a)
The atoms's ionization energy
b)
the type of atoms in the molecule
c)
The atom's oxidation number
d)
the shape of the molecule
22.
Which of the following statements correctly compares the behavior of a mixture of ethanol and water at STP?
a)
Water will evaporate first, because it has weaker intermolecular forces
b)
Ethanol will evaporate first, because it has weaker intermolecular forces
c)
Ethanol and water will evaporate simultaneously
d)
The aqueous solution will evaporate partially at a temperature between the boiling points of water and of ethanol
23.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
24.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
25.
Which phrase correctly describes the distribution of charge and the molecular polarity of ethane?
a)
symmetrical and polar
b)
asymmetrical and polar
c)
asymmetrical and nonpolar
d)
symmetrical and nonpolar
26.
Which statement correctly describes NaCl?
a)
Its charge is evenly distributed
b)
It is a polar molecule
c)
It is ionic, and its charges are distributed unevenly
27.
Which of the following geometries could be nonpolar?
a)
bent
b)
tetrahedral
c)
trigonal pyrimidal
d)
none of the above
28.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
29.
Which of the following molecules, based on the elements present, would be most polar?
a)
HF
b)
H2
c)
HCl
d)
HBr
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