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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What do ionic bonds form between

A

A metal and a non-metal

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2
Q

What is the attraction between ions called

A

Electrostatic attraction between the opposite charges of ions in a lattice

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3
Q

What is the formula and charge of a sulphate ion

A

SO4 2-

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4
Q

What is the formula and charge of a hydroxide ion

A

OH 1-

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5
Q

What is the formula and charge of a nitrate ion

A

NO3 1-

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6
Q

What is the formula and charge of a carbonate ion

A

CO3 2-

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7
Q

What is the formula and charge of a ammonium ion

A

NH4 1+

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8
Q

Properties of ionic compounds

A

Solid at room temperature
Giant structures
High melting points
Conduct electricity when molten / dissolved

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9
Q

What does a covalent bond contain

A

A shared pair of electrons

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10
Q

What is another name for a dative bond

A

A coordinate bond

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11
Q

What is a dative bond

A

Contains a shared pair of electrons with both electrons supplied by 1 atom

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12
Q

How are dative bonds represented

A

An arrow

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13
Q

Why do metals conduct electricity

A

They have delocalised electrons

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14
Q

What does the strength of a metallic bond depend on

A

Number of delocalised electrons
Size of the ions

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15
Q

What are the 4 types of crystal structure

A

Molecular
Macromolecular
Ionic
Metallic

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16
Q

What is the structure of diamond

A

Consists of pure carbon
4 covalent bonds
Bond angles of 109.5

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17
Q

What is the structure of graphite

A

Consist of pure carbon
Has 3 strong covalent bonds and VDW’s
120 bond angles
Has delocalised electrons so can conduct electricity

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18
Q

Why do metals have high boiling points

A

They have giant structures. Large amounts of energy are needed to overcome the metallic bonds

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19
Q

What are bonding pairs of electrons

A

2 electrons shared between atoms

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20
Q

What are lone pairs of electrons

A

A pair of valence electrons (electrons on the outer shell) that are not shared with another atom

21
Q

Why do pairs of electrons position themselves as far from each other

A

To minimise repulsion

22
Q

What is the order of repulsion strength from highest to lowest

A

Lone pair-lone pair
Lone pair-bond pair
Bond pair-bond pair

23
Q

How does a lone pair of electrons effect bond angles

A

A lone pair will push bonding pairs together

24
Q

What is a molecules shape with 2 bonding electron pairs and what are the bond angles

A

Linear
180

25
Q

What is a molecules shape with 3 bonding electron pairs and what are the bond angles

A

Trigonal planar
120

26
Q

What is a molecules shape with 4 bonding electron pairs and what are the bond angles

A

Tetrahedral
109.5

27
Q

What is a molecules shape with 5 bonding electron pairs and what are the bond angles

A

Trigonal bipyramidal
120
90

28
Q

What is a molecules shape with 6 bonding electron pairs and what are the bond angles

A

Octahedral
90

29
Q

What is a molecules shape with 3 bonding electron pairs and 1 lone pair. What are the bond angles

A

Pyramidal
107

30
Q

What is a molecules shape with 2 bonding electron pairs and 1 lone pair. What are the bond angles

A

V-shaped
117.5

31
Q

What is a molecules shape with 4 bonding electron pairs and 2 lone pair. What are the bond angles

A

Square planar
90

32
Q

How do you work out number of unbonded electron pairs

A

Group number - (Number of atoms bonded + charge)
/2

33
Q

What is electronegativity

A

The power of an atom to attract a bonding pair of electrons towards itself in a covalent bond

34
Q

What does electronegativity depend on

A

Nuclear charge (number of protons in the nucleus)
Distance between nucleus and outer shell
The shielding of the nuclear charge

35
Q

How does the symmetry of a covalent bond between 2 atoms with different electronegativities change

A

The bond would be drawn towards the more electronegative atom

36
Q

What does an unsymmetrical covalent bond cause

A

A polar bond which can lead to a permanent dipole being formed

37
Q

What are the 3 types of intermolecular force

A

VDW forces
Dipole-dipole forces
Hydrogen bonding

38
Q

What do VDW forces act between

A

All atoms and molecules

39
Q

What do dipole-dipole forces act between

A

Act between molecules with polar bonds

40
Q

What do Hydrogen bonds form between

A

Only between h and fluorine, oxygen or nitrogen (FON)

41
Q

How do VDW forces form

A

At any one time in a covalent bond, some electrons may happen to be closer to one atom. This will induce a temporary dipole. This then affects neighbouring atoms so they are attracted to each other for a short space of time

42
Q

What is the order of strength of intermolecular forces

A

Hydrogen bonding
Dipole dipole bonding
VDW’s

43
Q

Why are hydrogen bonds important in ice

A

When water freezes, all H bonds fix the molecules in a stable position. These molecules are further away from each other than liquid water do ice is less dense. This allows fish to survive etc

44
Q

Give an example of a bond with multiple shared pair of electrons

A

N≡N

45
Q

How are metals bonded

A

Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice

46
Q

What type of structure is ice

A

Ice is a molecular crystal that is connected by hydrogen bonds

47
Q

What type of crystal is iodine

A

Molecular covalent crystal

48
Q

What type of crystal is sodium chloride?

A

An ionic salt

Crystal lattice

49
Q

What type of crystal is magnesium?

A

Giant metallic lattice

Chemistry (36 decks)

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