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Chemistry 10INT > Topic 4 Test Review > Flashcards

Topic 4 Test Review Flashcards

This deck covers most, if not all, theory needed for the test. For practice refer to the worksheet on GC and make sure you go over the textbook in case I missed anything

You may prefer our related Brainscape-certified flashcards:
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1
Q

Sulphate

A

SO4 2-

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2
Q

Phosphate

A

PO4 3-

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3
Q

Nitrate

A

NO3 -

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4
Q

Carbonate

A

CO3 2-

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5
Q

Hydrogen Carbonate

A

HCO3 -

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6
Q

Hydroxide

A

OH -

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7
Q

Ammonium

A

NH4 +

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8
Q

Ionic Bonding

A

the electrostatic attraction between oppositely charged ions (metals+non-metals)

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9
Q

How are cations formed?

A

metals loosing their outer shell electrons (+)

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10
Q

How are anions formed?

A

non-metals gain enough electrons to complete outer shell (-)

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11
Q

Lattice Structure

A

ionic lattice is a strong alternating pattern of anions and cations.

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12
Q

Properties of Lattice Structure

A

Only conducts electricity when molten or dissolved. Low volatility (high melting point). Soluble in water.

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13
Q

Covalent Bonding

A

the attraction of two atoms to a shared pair of electrons (non-metals)

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14
Q

Single<–>Triple Bonds
(properties)

A

Longer—Shorter
Weaker—Stronger

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15
Q

Expanded Octet

A

Periods ≥ 3 (can have more than 8 electrons)

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16
Q

< 8 electrons exceptions

A

B (Boron) = 6
Be (Beryllium) = 4
H (Hydrogen) = 2

17
Q

Polar Covalent Bonds

A

When one atom has a greater attraction for the shared pair of electrons than the other atom
greater attraction = (ẟ-)
weaker attraction = (ẟ+)

18
Q

Electronegativities and bond type

A

Ionic: Δχp > 1.8
Non-polar covalent: Δχp = 0
Polar covalent: 0 < Δχp < 1.8

19
Q

non-polar / pure covalent bond

A

shared pair of electrons is shared equally

20
Q

Allotropes

A

different forms of the same element
C = diamond, graphite, fullerene (C60)

21
Q

Resonance structures

A

occur when there is more than one possible for a double bond in a molecule (ex. carbonate (CO3 2-), O3)

22
Q

linear angle

A

180*

23
Q

trigonal planar angle

A

120*

24
Q

tetrahedral angle

A

109.5*

25
Q

Trigonal pyramidal angle

A

107*

26
Q

Bent angle

A

<180*

27
Q

Metallic Bonding

A

electrostatic attraction between the positive nuclei and delocalised sea of electrons

28
Q

(why) electron conductivity

A

the sea of electrons are free to move

29
Q

(why) thermal conductivity

A

due to nuclei vibrations

30
Q

(why) high boiling + melting point

A

higher boiling/melting point = stronger attraction
- ionic charge
- size
- strong electrostatic attraction

31
Q

(why) malleability

A

positive nuclei can slide over each other due to the pressure of the sea of electrons

32
Q

alloys properties

A
  • stronger than pure metals
  • more resistant to corrosion
33
Q

SiO2

A

tetrahedral

34
Q

bent tetrahedral angle

A

104.5*

Chemistry 10INT (5 decks)

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