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Chemistry > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

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1
Q

What do physical/chemical properties of compounds depend on

A

Depend on the way compounds are held together by chemical bonds and intermolecular forces

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2
Q

Define ionic bonding

A

The electrostatic attraction between oppositely charged ions in a giant ionic lattice

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3
Q

Describe ionic lattices

A

Giant, regular repeating arrangement of ions

Crystal structures

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4
Q

Properties of ionic compounds

A

Strong electrostatic forces require lots of energy to overcome, so they have high melting/boiling points

Once molten, ions are free to move and can conduct an electric current

Often ionic compounds are soluble in water

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5
Q

Define a covalent bond

A

Electrostatic attraction between the nuclei and the shared pair of electrons

Non metals bonded together

Electron pair(s) shared

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6
Q

Describe singular molecular structures

A

Although covalent bonds are strong, molecules are not strongly attracted to eachother

Covalently bonded compounds have a small difference in electronegativity

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7
Q

Co-ordinate bonding:

A

A covalent bond where one of the atoms provides both of the electrons which form the bond

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8
Q

What is coordinate bonding also known as

A

Dative bonding

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9
Q

Where do arrows point towards in a dative bond

A

Towards the recipient ion

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10
Q

Describe metallic bonding

A

Involves the attraction between a ‘sea of delocalised electrons’ and positive ions arranged in a lattice

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11
Q

Properties of metals

A

Good conductors - delocalised electrons

High melting points - giant structures, electrostatic attraction between positive metal cations and delocalised electrons

Malleable/ductile - ions can slide over each other

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12
Q

What does the strength of a metal depend on

A

-size of the charge on the ion

-size of the ion

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13
Q

What are crystals

A

Solids in which the particles have a regular arrangement and are held together by forces of attraction

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14
Q

Four basic crystal types

A

Ionic
Metallic
Molecular
Macromolecular (giant covalent)

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15
Q

How much stronger are covalent bonds than hydrogen bonds

A

10 times

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16
Q

What are the two types of bonding in graphite

A

Strong covalent bonds

Weak van der waals

17
Q

What is within a hydrogen bond

A

H bonds with F,O, or N

18
Q

Another way to say van der walls

A

Instantaneous dipole

19
Q

What size molecules have the strongest van der waals

A

Bigger molecules, since they have a bigger swing of electrons

20
Q

Elements involved in dipole dipole interactions

A

C or H and halogen, O or N

21
Q

Define electronegativity

A

The tendency of an atom to attract a pair of electrons in a covalent bond

22
Q

What causes a permanent dipole

A

When two atoms in a covalent bond have different electronegativies, then electron distribution will be unsymmetrical

23
Q

What affects the polarity of a covalent bond

A

The difference in electronegativity

24
Q

What causes dipoles to cancel out

A

Linear molecule
Tetrahedral

25
Q

Why is hydrogen bonding in ice so important

A

Hydrogen bonding in water causes ice to be less dense
Floats on top of rivers
Insulates ponds

26
Q

Which area of the periodic table is most electronegative

A

Top right

27
Q

What happens to metallic domes after being moulded

A

Bonds reform to a similar strength

28
Q

2 bonding pairs

A

Linear

Bond angle 180

29
Q

3 bonding pairs

A

Triangular planar

120 degrees

30
Q

2 bonding pairs
1 lone pair

A

Bent

31
Q

4 bonding pairs

A

Tetrahedral

109.5

32
Q

3 bonding pairs
1 lone pair

A

Trigononal pyramidal

33
Q

2 bonding pairs
2 lone pairs

A

Angular, bent

34
Q

5 bonding pairs

A

Triangular bipyramidal

90 degrees and 120 degrees

35
Q

4 bonding pairs
1 lone pair

A

Seesaw

Notice: lone pair in equatorial plane

36
Q

3 bonding pairs
1 lone pair

A

T-shape

Lone pairs in equatorial plane

37
Q

6 bonding pairs

A

Octahedral

90 degrees

38
Q

5 bonding pairs
1 lone pair

A

Square pyramidal

39
Q

4 bonding pairs
2 lone pairs

A

Square planar

Chemistry (5 decks)

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