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Bonding & Structure > Bonding & Structure > Flashcards

Bonding & Structure Flashcards

1
Q

Name the 4 types of solids

A

Ionic, Metallic, covalent, Molecular

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2
Q

Ionic bonding is between…

A

metal cations & non-metal anions

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3
Q

Covalent bonding is between…

A

Non-metal atoms

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4
Q

Molecular bonding is between…

A

non-metal atoms & molecules

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5
Q

Metallic bonding is between…

A

Metal atoms

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6
Q

What solids cannot conduct electricity?

A

Ionic (but can conduct electricity when dissolved in water), molecular, covalent 1D chains and 3D networks

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7
Q

Why can these solids conduct electricity?

A

Some solids can conduct electricity due to delocalized (freely moving) electrons

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8
Q

Why can solids not conduct electricity?

A

No charged particles or freely moving electrons

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9
Q

Describe Ionic bonding

A

There is a strong electrostatic attraction between metal cations & non-metal anions to form a giant 3D lattice

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10
Q

Describe covalent bonding

A

There is a large network of atoms covalently bonded in linear 1D chains, 2D layers & 3D networks

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11
Q

Describe metallic bonding

A

The metal atoms are bonded to all other metal atoms in a 3D lattice

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12
Q

Describe intermolecular forces (molecular)

A

There are weak forces & attractions between molecules

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13
Q

Describe intreamolecular forces (molecular)

A

There are strong covalent bonds between atoms in each molecule

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14
Q

What types of solids are soluble?

A

Ionic, Molecular (only polar molecules)

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15
Q

What types of solids are insoluble?

A

Metallic, Molecular (only non-polar molecules), Covalent

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16
Q

Describe & explain 3D network (covalent)

Include conductivity, MP/BP, hardness

A

The non-metal atoms in a 3D network are held in strong & rigid structures
There are no charged particles, so it cannot conduct electricity
They have a high MP/BP due to the strong covalent bonds

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17
Q

Describe & explain 2D layers (covalent)

Include conductivity, MP/BP, hardness

A

They have a high MP/BP due to the strong covalent bonds
It can conduct electricity, as there are freely moving electrons
These layers slide over each other without disrupting the bonds; making them slippery

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18
Q

Describe & explain 1D chain (covalent)

Include conductivity, MP/BP, hardness

A

It cannot conduct electricity as there are no charged particles or freely moving electrons
Long 1D chains have more sites available for intermolecular forces; so they have a high MP/BP
These chains can slide over each other making them soft & flexible

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19
Q

Describe & explain molecular solid

Include conductivity, MP/BP, hardness

A

There are weak intermolecular forces holding the molecules together; which means this has a low MP/BP. Due to this weak force and attraction, the molecules can easily separate which makes them soft.
They cannot conduct electricity as there are no charged particles.
Molecules can be polar or non-polar. Polar molecules are soluble in water and non-polar molecules are insoluble in water

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20
Q

Describe & explain ionic

Include conductivity, MP/BP, hardness

A

Ionic solids are held together by strong electrostatic attractions in a 3D lattice; which requires lots of energy to break so there is a high MP/BP
Ionic bonds are brittle, when pressure is applied, ions move and like charges repel causing the lattice to break.
They cannot conduct electricity as the ions cannot move from their fixed position, however, when melted, ions are free to move allowing them to conduct electricity
Ionic solids are soluble, as the ions are separated due to attraction towards the polar water molecules

21
Q

Describe & explain metallic

Include conductivity, MP/BP, hardness

A

Metal atoms are held together in a 3D lattice by metallic bonding. There is a strong attraction between + metal atoms & electrons. The electrons are freely moving, hence they are able to conduct electricity.
Metals are not soluble in water, as the metallic bonds are to strong to be broken.
Many metals are hard & strong & therefore have a high MP/BP.
Metals are malleable and ductile as the layers of atoms are able to slide over each other without disputing the bonds

22
Q

What is the bond angle of a tetrahedral arrangement

A

109.5

23
Q

What is the bond angle of bent/V-shaped

A

109.5 (if tetrahedral arrangement)

120

24
Q

What is the bond angle of trigonal planar

A

120

25
Q

What is the bond angle of linear shape

A

180

26
Q

What is the bond angle of trigonal pyramid

A

109.5

27
Q

What is the most Electronegative atom

A

F

28
Q

What does EN stand for

A

Electronegativity

29
Q

How do you show the Electronegativity of an atom

A

Dipole arrows

30
Q

How do you identify if a molecule is polar

A

It contains polar bonds

It is asymmetrical, so dipole arrows are unable to cancel out

31
Q

How do you identify if a molecule is non-polar

A

It contains polar bonds

It is symmetrical, so dipole arrows cancel out

32
Q

Describe endothermic

A

Endothermic is the energy absorbed from the surroundings.

Bond breaking is endothermic

33
Q

Describe exothermic

A

Exothermic is the energy released to the surroundings.

Bond making is exothermic

34
Q

What is Ea

A

Activation energy- minimum energy required for a reaction to take place

35
Q

Solid –> powder –> gas

is this endo or exo?

A

Endothermic reaction as it is bond breaking

36
Q

Gas –> powder –> solid

is this endo or exo?

A

Exothermic reaction as it is bond making

37
Q

What calculation is required to calculate moles

A

n = m / M

38
Q

When drawing Lewis structures, what atom is always in the middle

A

C

39
Q

If the sign of the enthalpy change is negative, what reaction is it

A

Exothermic reaction

40
Q

If the sign of the enthalpy change is positive, what reaction is it

A

Endothermic reaction

41
Q

What calculation is used when calculating bond enthalpy change

A

bonds broken - bonds formed

42
Q

In an exothermic reaction are there more products than reactants, or more reactants than products

A

More reactants than products

43
Q

In an endothermic reaction are there more products than reactants, or more reactants than products

A

More products than reactants

44
Q

What are the exceptions to the octet rule

A 
H, He, Li = 2 e- max
Be = 4 e- max
B = 6 e- max
P = 10 e- max
S = 12 e- max
45
Q

If a molecule is polar & the dipoles are unable to cancel out, what does this mean

A

There are lone pairs; the molecule is asymmetrical

46
Q

Describe & explain if BF3 is polar or non-polar

A

BF3 molecule has 3 B-F covalent bonds. The B-F covalent bonds are polar due to the difference in electronegativity between B & F, with F being more electronegative than B. Thus B-F bonds form dipoles: B (delta positive) & F (delta negative). These dipoles are arranged in a trigonal planar shape and so are arranged symmetrically around the central atom. These dipoles are able to cancel out, so the molecule is a non-polar molecule overall

47
Q

Describe & explain if NH3 is polar or non-polar

A

NH3 molecule has 3 covalent bonds. The N-H covalent bonds are polar due to the difference in electronegativity between N & H, with N being more EN than H. Thus N-H bonds form dipoles; N (delta negative) & H (delta positive). Due to the lone pair of electrons, these dipoles are arranged in a trigonal pyramid shape and so are arranged asymmetrically. These dipoles are unable to cancel out, so the molecule is a polar molecule overall

48
Q

Describe & explain the shape of SO2

A

SO2 molecule, there are 3 electron clouds around the central atom S. These regions repel as far apart as possible due to the valence electron pair repulsion into a trigonal planar arrangement, resulting in a bond angle of 120. There are 2 regions of electrons that are bonding and 1 region of an electron that are lone pairs, which are not observed, so the shape of the molecule is bent/V-shaped

Bonding & Structure (1 decks)

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