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Chemical Bonding Flashcards

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1
Q

What is a compound?

A

A substance that is made up of two or more different elements, chemically combined.

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2
Q

How are atoms held together?

A

By chemical bonds

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3
Q

Describe noble gases

A

They contain 8 electrons in their outer shell and are generally unreactive.

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4
Q

What are the uses of helium?

A
  • Airships because it is not flammable.

- Balloons because it is lighter than air.

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5
Q

What are the uses of argon?

A

Used in lightbulbs to stop imploding.

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6
Q

What is the octet rule?

A

When bonding occurs, atoms tend to reach an electron arrangement with 8 electrons in the outer shell.

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7
Q

What are the limitations of the octet rule?

A
  • Hydrogen
  • Lithium
  • Transition Elements
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8
Q

What is a valency?

A

It is the number of bonds an atom makes when it reacts.

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9
Q

What is a transition metal?

A

It is a metal that forms at least one ion with a particularly filled ‘d’ sublevel.

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10
Q

List three facts about transition metals which could be good to know.

A
  • They have a variable valency.
  • They form coloured compounds
  • They are used mainly as catalysts.
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11
Q

What are the two exceptions of transition metals?

A
  • Zinc (Zn)

- Scandium (Sc)

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12
Q

What is ionic bonding?

A

It is the transfer of electrons.

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13
Q

What is an ion?

A

A charged atom/group of atoms.

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14
Q

What is the charge of a cation?

A

Positive

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15
Q

What is the charge of an anion?

A

Negative

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16
Q

List the chemical equation of how cations formed.

A

Na —> (Na+) + (e-)

Ca —> (Ca2+) + (2e-)

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17
Q

List the chemical equation of how anions formed.

A

Cl- —> (Cl) + (e-)

O2- —> (O) + (2e-)

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18
Q

Define ionic compounds.

A

It is the force of attraction between oppositely charged ions in a compound.

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19
Q

What are the characteristics of ionic substances?

A
  • Strong forces between the ions mean it is very hard to break up due to the lattice structure.
  • Cannot conduct electricity when solid but can when dissolved in water.
  • Most dissolvable in water.
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20
Q

With ionic substances, comment on the:

  • boiling and melting points.
  • the state that it’s in at room temperature.
A

Both boiling and melting points are high and it is solid at room temperature.

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21
Q

Name two everyday examples of ionic substances.

A
  • Table salt (Sodium Chloride) (NaCl)

- Floridation (Sodium Floride) (NaF)

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22
Q

When is a covalent bond formed?

A

When atoms share electrons.

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23
Q

What is an example of a single covalent bond?

A

H2

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24
Q

What is an example of a double covalent bond?

A

O2

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25
What is an example of a triple covalent bond?
N2
26
What are bonding pairs?
They have shared electron pairs that form covalent bonds.
27
What are lone pairs?
They are electron pairs that aren't involved in covalent bonds.
28
What happens to the orbitals in a covalent bond?
The orbitals overlap each other
29
How are sigma bonds formed?
They are formed by the head-on overlap of two orbitals (can be s or p orbitals).
30
How are pi bonds formed?
They are formed by the sideways overlap of p-orbitals.
31
Why are sigma bonds stronger than pi bonds?
There is more of an overlap between orbitals with sigma bonds than pi bonds.
32
What bonds do a single covalent bond possess?
1 sigma
33
What bonds do a double covalent bond possess?
1 sigma + 1 pi
34
What bonds do a triple covalent bond possess?
1 sigma + 2 pi
35
Briefly outline 3 differences between ionic and covalent bonds.
Ionic - Transfer of electrons - Ions formed - Usually solid at room temperature Covalent - Sharing electrons - Covalent bond formed - Usually liquid or gas at room temperature.
36
How are molecules formed?
They are formed when atoms are joined together by covalent bonds.
37
What do you use to figure out the arrangement of atoms in a molecule?
You use the Valence Shell Electron Pair Repulsion theory (VSEPR).
38
Talk about the lone pairs around the central atom and how that has an effect on the shape of the molecule.
Lone pairs are closer to the nucleus of the atom which means they are closer together (forming a stronger negative). Their collective nuclear charge pushes the bonding pairs further apart, decreasing the bond angle and distorts the shape of the molecule (i.e. H20).
39
Talk about the bonding pairs around the central atom.
The electrons in the bonding pairs repel each other and want to be as far apart as possible.
40
For a substance that has 2 bonding pairs: - What is the shape? - What's an example? - What is the bond angle?
Shape - Linear Example - BeH2 Bond angle - 180*
41
For a substance that has 3 bonding pairs: - What is the shape? - What's an example? - What is the bond angle?
Shape - Trigonal planar Example - BCl3 Bond angle - 120*
42
For a substance that has 4 bonding pairs: - What is the shape? - What's an example? - What is the bond angle?
Shape - Tetrahedral Example - Ch4 Bond angle - 109.5*
43
In order of most powerful to least powerful of repulsion, name the 3 types between lone pairs and bonding pairs.
Most - lone and lone Moderate - lone and bonding Weakest - bonding and bonding
44
In the NH3 molecule: - How many bond pairs are present? - How many lone pairs are present? - What is the bond angle? - What is the shape of the molecule?
B.P - 3 L.P - 1 B.A - 107* Shape - Pyramidal
45
In the H20 molecule: - How many bond pairs are present? - How many lone pairs are present? - What is the bond angle? - What is the shape of the molecule?
B.P - 2 L.P - 2 B.A - 104.5* Shape - V-shaped
46
What is meant when it is said that an atom is non-polar?
It is when atoms in a covalent bond share electrons equally (eg H2, N2, O2).
47
What is meant when it is said that an atom is polar?
It is when atoms in a covalent bond don't share electrons equally (eg HCl, NH2).
48
What is electronegativity?
It is the relative attraction an atom has for a shared pair of electrons in a single covalent bond.
49
What happens when the electronegativity increases?
The pull also increases.
50
Why is there an increase of electronegativity across the periodic table?
- An increased nuclear charge. | - A decreased atomic radius.
51
Why is there a decrease of electronegativity down the periodic table?
- Screening is in effect. | - Increase in atomic radius.
52
How do you know the difference between the negative and positive dipoles?
The atom that has a slightly greater pull on the electrons is the negative dipole and the other atom(s) are the positive dipole(s).
53
Give an example of a molecule with positive and negative dipoles.
H20 H - (𝛿) H - (𝛿) O- (𝛿2-)
54
What bond types are formed with these values of electronegativity: - (0.00 - 0.40) - (0.41 - 1.70) - (1.71 - +)
- Non-polar covalent - Polar covalent - Ionic
55
Give two examples of everyday polar substances
- Water | - Ethanol
56
Give two examples of everyday non-polar substances
- Tetrachloroethene | - Acetone
57
Can a molecule that has polar bonds be non-polar overall?
Yes, if it one of the following shapes; - Linear - Planar - Tetrahedral
58
If a molecule is a-symmetrical, what shape is it?
- Pyramidal | - V-shaped
59
What is intramolecular bonding?
It is bonding within the molecule (eg between hydrogen and oxygen atoms in H20).
60
What is intermolecular bonding?
It is bonding between molecules (between H20 molecules).
61
What are the three types of intermolecular bonding?
- Van der Waal - Dipole-Dipole - Hydrogen
62
What are Van der Waal forces?
They are weak forces of attraction between temporary dipoles.
63
Where are temporary dipoles set up?
In non-polar molecules.
64
How long do Van der Wall's last?
Not very long and they have low boiling points.
65
Do Van der Wall's have a high or low boiling point?
They have a low boiling point.
66
What are dipole-dipole forces?
They are forces of attraction between the negative pole of one molecule and the positive pole of another.
67
What is the dipole-dipole strength in relation to ionic bonds?
They are much weaker than ionic bonds.
68
What is hydrogen bonding?
Hydrogen bonding occurs in molecules where an atom of hydrogen is bonded to nitrogen, oxygen or fluorine. The hydrogen then carries a positive charge and is attracted to the electronegative atom in another molecule.
69
What boiling points do hydrogen atoms have?
They have high boiling points.
70
What three elements are the most electronegative?
- Nitrogen - Oxygen - Fluorine

Chemistry (11 decks)

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