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Chemistry > Ionic And Covalant Bonding Ch. 6 > Flashcards

Ionic And Covalant Bonding Ch. 6 Flashcards

1
Q

What is water crystallisation

A

Water that is chemically combined in definite proportions in a crystalline compound

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2
Q

What is the octet rule

A

All atoms are looking to have a full outer shell of 8 electrons

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3
Q

Hydroxide

A

OH-

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4
Q

Carbonate

A

CO3 2-

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5
Q

Nitrate

A

NO3 -

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6
Q

Hydrogencarbonate

A

HCO3-

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7
Q

Sulfite

A

SO3 2-

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8
Q

Sulfate

A

SO4 2-

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9
Q

Phosphate

A

PO4 3-

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10
Q

Dichromate

A

Cr2O7 2-

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11
Q

Ethanoate

A

CH3COO -

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12
Q

Ammonium

A

NH4 +

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13
Q

Manganate(VII)

A

MnO4 -

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14
Q

Chromate

A

CrO4 -

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15
Q

Exceptions to the octet rule

A

Beryllium and boron do not have enough electrons in their outer shell to get 8 electrons, d-block elements don’t obey the rule Hydrogen and lithium tend to reach the electronic structure of helium.

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16
Q

What is an ionic bond

A

The electrostatic force of attraction between oppositely charged ions

17
Q

What do iconic bonds form

A

Three dimensional lattice structures

18
Q

What is a covalent bond

A

Formed when two atoms share a pair of electrons

19
Q

What is sigma bonding

A

Involves the end on overlap of p-orbitals and s-orbitals, stronger than pi bonding and occurs first

20
Q

What are pi bonds

A

Involves the side on overlap of p-orbitals, forms the 2nd and 3rd bond and is weaker than sigma bonds

21
Q

What kind of bond occurs when two oxygen atoms bond

A

Pure covalent bond, forms a molecule of oxygen (O2)

22
Q

Define electronegativity

A

The relative attraction of an atom for shared pairs of electrons in a covalent bond

23
Q

What three factors affect the electronegativity of an element

A

Nuclear charge, atomic radius, screening effect

24
Q

General trend for electronegativity across a period

A

Electronegativity increases due to a larger nuclear charge and a smaller atomic radius

25
Q

General trend for electronegativity down a group

A

Electronegativity decreases due to an increase in the screening effect and an increase in atomic radius

26
Q

Electronegativity difference < 1.7

A

Polar covalant

27
Q

Electronegativity difference < 0.4

A

Covalant (slight polarity)

28
Q

Electronegativity difference > 1.7

A

Ionic

29
Q

Properties of Ionic compounds

A

High melting point, conduct electricity when molten or in an aqueous solution, hard solids

30
Q

Properties of covalent compounds

A

Low melting points, do not conduct electricity in the liquid state, are gases, liquids or soft solids

31
Q

How do you purify covalent compounds

A

Via recrystallization

Chemistry (8 decks)

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