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Chemistry > 1.3 bonding > Flashcards

1.3 bonding Flashcards

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1
Q

Name 5 compound ions

A

Ammonium NH4+
Nitrate NO3-
Carbonate CO3^2-
Sulfate SO4^2-
Hydroxide OH-

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2
Q

What is an ionic bond?

A

Many strong electrostatic forces of attraction between positive and negative ions

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3
Q

Examples of ionic compounds (atoms held in lattice)

A

MgO, MgCl2, NaCl

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4
Q

Why can ionic compounds conduct electricity when molten/ dissolved?

A

Ions are free to move through the structure and carry a charge

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5
Q

Do ionic compounds have a high or low mp? Why?

A

Many string electrostatic forces between opposite charges take lots of energy to break

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6
Q

Why are ionic compounds soluble?

A

Water molecules are polar so pull ions away from lattice causing it to dissolve

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7
Q

Why are ionic compounds brittle?

A

Layers slide causing like charges to line up and repel

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8
Q

What is a molecule and how are they held together
Examples

A

Two or more atoms bonded and held together by string covalent bonds
Cl2, H2O, CO, C2H5OH

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9
Q

What is a covalent bond?

A

A shared pair of valence electrons between the nuclei of 2 atoms

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10
Q

Do simple covalent compounds have a high or low mp? Why?

A

Weak intermolecular forces

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11
Q

What is graphite?

A

Carbon atoms arranged in sheets of flat hexagons covalent it bonded with 3 bonds.

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12
Q

Properties of graphite

A

1) slippery as weak vanderwaals between layers
2) electric conductor as 4th electron is delocalised
3) strong and light as layers far apart so low density
4) High mp as strong covalent bonds
5) insoluble in any solvent as strong covalent bonds

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13
Q

What is diamond?

A

Each carbon atom bonded covalently to 4 others forming tetrahedral shape and crystal lattice structure

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14
Q

Properties of diamond

A

1) high mp as strong covalent bonds
2) extremely hard as strong covalent bonds
3) good thermal conductor as strong bonds so vibrations travel easily through stiff structure
4)can’t conduct electricity as all electrons bonded
5) insoluble in any solvent as strong covalent bonds

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15
Q

What is a coordinate covalent bond?
Examples?

A

An atom donates a lone pair of valence electrons to form a coordinate bond with another atom/ ion

Eg ammonium ion and hydroxonium ion

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16
Q

What is a charge cloud?

A

Where you have a big chance of finding an electron

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17
Q

Shape of charge cloud affects how much it repels other charge clouds. Order the repulsion

A

Lone pair to lone pair Strong
Lone pair to bonded pair. Middle
Bonded pair to bonded pair Weak

18
Q

How do you represent different directions in shapes of molecules?

A

/\ towards
——— away
_________ parallel to paper

19
Q

What is electronegativity?

A

The ability of an atom to attract the bonding electrons in a covalent bond.

20
Q

What does electronegativity depend on?

A

1) atomic radius
2) e- shielding
3) charge

21
Q

What happens to electronegativity down a group?

A

Decreases
Increase radius so more energy levels so more shielding and less nuclear attraction.

22
Q

What happens to electronegativity across a period?

A

Increases
Decrease radius as higher nuclear charge there is no extra e- shielding so nuclear attraction increases

23
Q

What is a non polar bond?

A

Equal electronegativity so electrons are equally attracted to both nuclei eg in diatomic gases

24
Q

What is a polar bond?

A

Atoms with different electronegativity- bonding electrons pulled towards more electronegative atoms. Bigger difference, more polar

25
Q

What is a dipole?

A

A difference in electronegativity causing an uneven charge distribution

26
Q

If the bonds are symmetrical, is it a permanent dipole?

A

No they cancel

27
Q

If bonds are in same rough direction, is it permanent dipole?

A

Yes bonds don’t cancel so charge unevenly distributed

28
Q

What is an intermolecular force?

A

Forces between molecules

29
Q

What are van der waals forces?

A

Electrons move quickly in charge cloud creating temporary dipole. This causes opposite dipole in other direction on neighbouring atom etc so they are attracted

30
Q

Why do larger molecules have higher mp and bp?

A

Bigger radius so more electrons so more van der waals more energy needed to overcome

31
Q

What are permanent dipole dipole forces?

A

Polar molecules attracting other polar molecules. There will be weak electrostatic forces of attraction between d+ and d-

32
Q

What is hydrogen bonding?

A

Bonding between H and and F,O or N atom with a lone pair

33
Q

Why does water have higher bp than other group 6 hydrides?

A

Extra energy needed to break hydrogen bonds in water

34
Q

Why is ice less dense than water?

A

When it cools, molecules make more hydrogen bonds and arrange in regular lattice. H bonds are long so big distance between molecules

35
Q

What is metallic bonding?

A

Many strong electrostatic forces of attraction between delocalised valence electrons and layers of positive metal ions.

36
Q

Why do metals have high melting points?

A

Strong electrostatic forces of attraction. The more delocalised electrons the stringer the bonds and the higher the mp

37
Q

Why are metals ductile and malleable?

A

No bonds holding specific ions together so layers can slide

38
Q

Why can metals conduct electricity?

A

Delocalised electrons are free to move throughout the structure and carry a charge

39
Q

Why can metals conduct heat?

A

Delocalised electrons can pass kinetic energy to each other

40
Q

Why aren’t metals soluble?

A

The metallic bond is too strong

41
Q

What are giant covalent structures?

A

A type of crystal structure with a huge network of atoms bonded covalently

Chemistry (18 decks)

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