WorksheetsChapter 3: Chemical Bonding Unit Review Term 1
Total questions: 67
Worksheet time: 48mins
What is the correct formula for the molecule shown in the picture?
N3H
NH
NH3
NH4
Write the electron configuration for an oxygen atom.
Write like this: 1s2[space]2s2[space] (a)
In the correct Lewis structure for CH4,
how many unshared electron pairs surround the carbon?
(a)
In CO2, how many unshared pairs of electrons does each oxygen have?
1
2
4
6
When writing Lewis structures, only ____ electrons are involved.
inner shell
valence
stable
How many total valence electrons are participating in bonding in the image shown?
(a)
Three pairs of electrons are shared in a ___ .
single bond
double bond
triple bond
quadruple bond
How many electrons does each line indicate are shared?
1
2
3
4
How many electrons should Lithium have around its Lewis dot model?
1
2
3
4
How many electrons should Beryllium have around its Lewis dot model?
1
2
3
4
How many electrons should Boron have around its Lewis dot model?
1
3
5
7
How many electrons should Carbon have around its Lewis dot model?
2
4
6
8
How many electrons should Nitrogen have around its Lewis dot model?
1
3
5
7
How many electrons should Oxygen have around its Lewis dot model?
2
4
6
8
How many electrons should Fluorine have around its Lewis dot model?
2
3
5
7
giant (a) structure refers to a lattice of positive ions in a ‘sea’ of electrons.
The image shown is an example of displayed formula of a molecular compound. What is the name of this molecule?
(a)
The image shown is an example of a dot and cross diagram. What is the name of this molecule?
(a)
What is the group number of fluorine atom?
1
3
5
7
What is the group number of carbon atom in the periodic table?
1
2
3
4
What is the group number of lithium in the periodic table?
1
2
3
4
what is the group number of nitrogen atom in the periodic table?
1
3
5
7
What is the group number of oxygen in the periodic table?
2
4
6
8
Write the electron configuration of sodium.
Write like this: 1s2[space]2s2[space] (a)
Write the electron configuration of fluorine.
Write like this: 1s2[space]2s2[space] (a)
Which statement does not describe the property of ionic compounds?
they have high melting points
they have low boiling points
they are often soluble
they conduct electricity when molten or dissolved in water
True or False: In metals, it is the delocalised electrons are able to move while Ionic substances will not conduct electricity as solids. This is due to the fact that ions are not free to move in a solid as they are arranged in an ionic lattice.
(a)
What holds sodium chloride together?
the electrostatic force of attraction between the oppositely charged ions
the electrostatic force between metal ions and delocalised electrons
when elements share electrons in a covalent bond to form molecules
What holds molecular compound together?
the electrostatic force of attraction between the oppositely charged ions
the electrostatic force between metal ions and delocalised electrons
the sharing of electrons in a covalent bond to form molecules
Is Nitrogen gas a single, double or triple type of covalent bond?
(a)
Is methane (a compound of hydrogen and carbon) a single, double or triple type of covalent bond?
(a)
Is carbon dioxide a single, double or triple type of covalent bond?
(a)
What elements generally make an ionic bond?
none of these
metal and nonmetal
metal
two nonmetals
What elements generally make a covalent bond?
none of these
metal and nonmetal
metal
two nonmetals
Predict the bond that will form between Be and F.
Ionic
Covalent
Metallic
What happens when an atom loses an electron?
It stays the same.
It becomes Negatively Charged
It becomes Positively Charged
Predict the bond that is formed between Phosophorus and Chlorine?
Ionic
Covalent
Metallic
TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.
(a)
How do covalent bonds form?
Sharing valence e- between atoms.
Donating & receiving valence e- between atoms.
Opposite slight charges attract each other between compounds.
Which of these is NOT an alloy?
brass
bronze
copper
stainless steel
What is the basis of a metallic bond?
the attraction between protons and neutrons.
the attraction between positive metal ions and interlocking electrons.
the attraction between positive metal ions and free floating electrons.
the attraction of neutral metal atoms.
The ability of a material to be shaped in all directions
without cracking or breaking.
conductivity
malleability
ductility
hardness
Examine the image: How many bonds are formed looking at the model of the compound? And also idetify what type of bond is formed.
2 bonds; ionic
2 bonds; covalent
4 bonds; covalent
4 bonds; metallic
Predict the bond: Fe2S3
Ionic
Covalent
Metallic
Predict the bond: CF4
Ionic
Covalent
Metallic
What type of forces hold on an ionic lattice together?
Metallic bond
Electrostatic attraction forces
Covalent bond
Ionic compounds conduct electricity when dissolved in water.
Which statement below best explains the property?
Bonds are strong.
Ions are free to move.
Electrons are free to move.
There are weak intermolecular forces of attraction.
All solids at room temperature
Ionic compound
Molecular compound
Molten compound conducts electricity.
Ionic compound
Molecular compound
Molten compound does NOT conduct electricity.
Ionic compound
Molecular compound
When dissolved in water, the solution does NOT conduct electricity.
Ionic compound
Molecular compound
Which forms ions in a solution?
Ionic compound
Molecular compound
What is a cation's charge?
(a)
What is an anion's charge?
(a)
What is the chemical formula of the following covalent substance?
CO
CH4
CH3
CO2
Determine the non bonding pairs of Fluorine in HF.
1
2
3
4
Which elements have 1 valence electron?
period 1
group 1
group 2
period 2
which elements have 4 valence electrons?
group 3
group 14 or 4
group 5 or 15
group 2
groups on the periodic table tell you
the number of energy levels (rings)
the number of valence electrons
the elements identity
the number of protons
periods on the periodic table tell you
the number of energy levels
the number of valence electrons
the elements identity
the number of protons
What group number is Mg?
(a)
What group number is P?
(a)
What group number is K?
(a)
What period number is K?
(a)
What period number is P?
(a)
What period number is Mg?
(a)
What period number is F?
(a)
