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Chemisty As > Physical Chemisty Bonding 3 > Flashcards

Physical Chemisty Bonding 3 Flashcards

1
Q

What is ionic bonding

A

Ionic bonding occurs between metals and non-metals
Electrons are transferred from metal atoms to non-metal atoms
Positive and negative ions are formed

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2
Q

Why do ions attract each other?

A

Two ions are attracted to each other by electrostatic attraction between their opposite charges. The attraction spreads throughout the compound. Every positive ion attracts every negative ion and vice versa.

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3
Q

What is the structure called that ionic compounds exist in?

A

Lattice

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4
Q

What are ionic compounds at room temp

A

Solids

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5
Q

Do ionic compounds have low or high melting points and why?

A

High melting points as they have a giant structure. This is because in order to melt an ionic compound, energy must be supplied to break up the lattice of ions.

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6
Q

Do ionic compounds conduct electricity if yes when

A

Yes, but only when molten or dissolved in water but not when solid. This is because the ions that carry the current are to free to move in liquid state not solid.

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7
Q

What does aqueous mean

A

Dissolved in water

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8
Q

Why do ionic compounds shatter easily

A

This is because they form a lattice of alternating positive and negative ions. A blow can cause the ions to move and produce contact between like charges.

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9
Q

What is the ionic formula of ammonium

A

NH4+

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10
Q

What is the ionic formula for Carbonate

A

CO3 ^2-

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11
Q

What is the ionic formula for hydroxide

A

OH^-

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12
Q

What is the ionic formula for Nitrate

A

NO3^-

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13
Q

What is the ionic formula for Sulfate

A

SO4 ^2-

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14
Q

What is an ionic compound

A

when oppositely charged ions come together and form ionic bonds you get an ionic compound

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15
Q

What is a covalent bond

A

Covalent bond forms between a pair of non metal atoms

they do this to get a full shell of electrons.

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16
Q

What does a single covalent bond contain

A

a shared pair of electrons

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17
Q

How does sharing electrons hold atoms together?

A

Atoms with covalent bonds are held together by the electrostatic force of attraction between the nuclei and the shared electrons

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18
Q

What happens in a double bond

A

In a double bond four electrons are shared. For example Oxygen. you represent double bonds with two lines.

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19
Q

How do you represent a triple bond

A

three lines

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20
Q

What is co-ordinate/covalent bonding?

A

Where one of the atoms provides both of the shared electrons. For example: NH4+ is formed by co-ordinate bonding. It forms when a nitrogen atom in an ammonia molecule donates a pair of electrons to a proton H+.

21
Q

What is metallic bonding

A

Metals exist as a giant lattice of positive ions surrounded by delocalised electrons. This means the electrons are able to move about the metal. Furthermore, the positive ions are attracted to the negative electrons meaning they are closely packed

22
Q

What does the number of delocalised electrons depend on?

A

It depends on the amount of electrons lost by each metal atom.

23
Q

Why are metals good conductors of electricity

A

The delocalised electrons can move and carry a current.

24
Q

Why are metals good conductors of heat

A

The delocalised electrons can pass kinetic energy to each other, making metals good thermal conductors.

25
Q

why do metals have high melting points

A

Because of their giant structures. There is a strong attraction between the sea of electrons and positive ions making the atoms difficult to seperate.

26
Q

What does it mean when something is malleable?

A

can be beaten into shape

27
Q

what does it mean when something is ductile?

A

can be pulled into thin wires

28
Q

Why are metals malleable and ductile?

A

the metal ions are able to slide over each other.

29
Q

In general what does the strength of any metallic bond depend on?

A

The greater the charge on the ion, the greater the number of electrons and the stronger the force of attraction between the ions and electrons.
The smaller the ion the closer the electrons are to the positive ions making the bond stronger.

30
Q

What is electronegativity?

A

The ability to attract the bonding electrons in a covalent bond is electronegativity. It is measured on the pauling scale.

31
Q

What does a higher number on the pauling scale mean?

A

An element is better able to attract the bonding electrons

32
Q

What is the most electronegative element?

A

Fluorine, closely followed by oxygen, nitrogen and chlorine.

33
Q

What do bonding pairs/ lone pairs exist as?

A

They exist as charge clouds

34
Q

What is a charge cloud

A

A charge cloud is an area where you have a big chance of finding an electron. The electrons dont stay still they whizz around the inside of the cloud

35
Q

What is electron pair repulsion

A

Electrons are all negatively charged so charge clouds repel each other until they are as far apart as possible.

36
Q

What affects how much a charge cloud repels another charge cloud?

A

The shape of a charge cloud.

37
Q

What repels more lone pair charge clouds or bonding pair clouds and what does this do?

A

Lone pair charge clouds, so bond angles are often reduced because bonding pairs are pushed together by lone pair repulsion.

38
Q

Central atom with two electron pairs

A

Linear 180

39
Q

Central atom with three electron pairs

A

trigonal planar 120

40
Q

central atom with four electron pairs

A

tetrahedral 109.5

41
Q

Central atom with three bonding pairs and one lone pair

A

trigonal pyramidal 107

42
Q

central atom with two bonding pairs and 2 lone pairs

A

bent 104.5

43
Q

central atom with 5 electron pairs

A

trigonal bipyramidal 120 and 90

44
Q

central atom with four bonding pairs and 1 lone pair

A

seesaw 102 and 86.5

45
Q

central atom with three bonding pairs and 2 lone pairs

A

t shape 87.5

46
Q

central atom with six electron pairs

A

octahedral 90

47
Q

central atom with 5 bonding pairs and 1 lone pair

A

square pyramidal 90

48
Q

central atom with 4 bonding pairs and 2 lone pairs

A

square planar 90

Chemisty As (5 decks)

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