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Physical Chemistry > Unit 1: Section 3- Bonding > Flashcards

Unit 1: Section 3- Bonding Flashcards

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1
Q

Define ionic bonding

A

Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer

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2
Q

What type of ion does a metal form?

A

positive

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3
Q

What type of ion does a non metal form?

A

negative

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4
Q

What structure do ionic crystals have?

A

giant lattice of ions

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5
Q

How does the size of the ions affect the properties of the bond?

A

ionic bonding is stronger and the melting points higher when the ions are smaller

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6
Q

How can the charges affect the strength of the ionic bond?

A

if the charges are higher, the ionic bonds are stronger

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7
Q

Explain why negative ions formed in group 5 to 7 are larger

A

the negative ion has more electrons than the corresponding atom but the same number of protons, so the pull of the nucleus is shared over more electrons, and the attraction per electron and the attraction per electron is less, making the ion bigger

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8
Q

What happens to ionic radii size going down a group?

A

it increases, because there are more shells of electrons

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9
Q

What is a covalent bond?

A

shared pair of electrons

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10
Q

What is a dative covalent bond?

A

when the shared pair of electrons comes from only one of the bonding atoms

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11
Q

What is metallic bonding?

A

metallic bonding is the electrostatic force of attraction between the positive metal atoms and delocalised electrons

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12
Q

Name three things that effect the strength of a metallic bond

A
  • number of protons (strength of nuclear attraction)
  • number of delocalised electrons
  • size of the ions
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13
Q

What is the structure of ionic bonded molecules?

A

giant ionic lattice

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14
Q

What is the structure of molecules that are covalently bonded?

A

simple molecular: (Van der Waals forces, permanent dipoles, hydrogen bonds)

macromolecular: giant molecular structures

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15
Q

What is the structure of molecules that are metallically bonded?

A

giant molecular lattice

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16
Q

What words do you use to describe simple molecular substances?

A

molecules
intermolecular forces

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17
Q

State the solubility in water of ionic, molecular, macromolecular and metallic compounds

A

Generally good
generally poor
insoluble
insoluble

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18
Q

State how conductive when solid ionic, molecular, macromolecular and metallic compounds are

A

poor
poor
poor
good

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19
Q

State how conductive when molten ionic, molecular, macromolecular and metallic compounds are

A

good
poor
poor
good

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20
Q

State the BP and MPs of ionic, molecular, macromolecular and metallic compounds

A

high
low
high
high

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21
Q

Describe a linear molecule

A

2 bonding pairs
0 lone pairs
bond angle- 180

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22
Q

Name three examples of linear molecules

A

CO2 CS2 HCN

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23
Q

Describe a trigonal planar molecule

A

3 bonding pairs
0 lone pairs
bond angle- 120

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24
Q

Name 3 examples of trigonal planar molecules

A

BF3
AlCl3
SO3

25
Q

Describe a tetrahedral molecule

A

4 bonding pairs
0 lone pairs
bond angle- 109.5

26
Q

Name two examples of tetrahedral molecules

A

SiCl4, SO4 2-

27
Q

Describe a trigonal pyramidal molecule

A

3 bonding pairs
1 lone pair
bond angle- 107

28
Q

Describe a bent molecule

A

2 bonding pairs
2 lone pairs
bond angle- 104.5

29
Q

Describe a trigonal bipyramidal molecule

A

5 bonding pairs
0 lone pairs
bond angle- 120 and 90

30
Q

Describe an octahedral molecule

A

6 bonding pairs
0 lone pairs
bond angle- 90

31
Q

Explain which repels more: lone pairs or bonding pairs

A

lone pairs- by about 2.5 degrees more per lone pair

32
Q

Define electronegativity

A

the relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself

33
Q

How is electronegativity measured?

A

Pauling scale (1-4)

34
Q

What are the most electronegative elements?

A

fluorine, oxygen, nitrogen, chlorine

35
Q

Describe the trend in electronegativity along a period

A

increases
as the number of protons increases and the atomic radius decreases because the electrons in the same shell are pulled in more

36
Q

Describe the trend in electronegativity down a group

A

it decreases down a group because the distance between the nucleus and the outer electrons increases and the shielding of inner shell electrons increases

37
Q

What type of bonding will a compound have if it contains elements of a similar electronegativity?

A

purely covalent

38
Q

What type of bonding will a compound have if it contains elements with a large electronegativity difference?

A

ionic

39
Q

When does a polar covalent bond form?

A

when the elements in the bond have different electronegativities (0.3-1.7)

40
Q

What is a polar covalent bond?

A

a bond where it has an unequal distribution of electrons in the bond and produces a charge separation (dipole ends)

41
Q

How do you identify a symmetrical molecule?

A

all bonds identical and no lone pairs of electrons

42
Q

Can a symmetrical molecule be polar?

A

no, even if the individual bonds within the molecule are polar

43
Q

Give an example of a symmetrical molecule

A

CO2

44
Q

What molecules do Van der Waals forces occur in?

A

everything except ionic substances

45
Q

What are Van der Waals also called?

A

transient, induced dipole- dipole interactions

46
Q

How do Van der Waals forces occur in molecules?

A

the electrons are moving constantly and randomly, so the electron density can fluctuate and parts of the molecule become more or less negative

47
Q

What is the main factor affecting the size of Van der Waals forces?

A

the more electrons there are in the molecule the higher the chance that temporary dipoles will form, so stronger Van der Waals forces

48
Q

How can you explain the increasing boiling points down group 7?

A

increasing numbers of electrons, bigger molecules, so increasing Van der Waals forces between molecules.

49
Q

What is the trend in boiling points down group 7?

A

increasing

50
Q

How can you explain why I2 is a solid and Cl2 is a gas?

A

Van der Waals forces

51
Q

How can increasing boiling points of alkanes be explained?

A

long, more electrons, stronger Van der Waals

52
Q

What does the permanent dipole-dipole force occur between?

A

polar molecules

53
Q

Which bonds are stronger, dipole-dipole or Van der Waals forces?

A

permanent dipole- dipole

54
Q

What type of molecules are polar molecules?

A

asymmetrical

55
Q

How do polar molecules form a bond?

A

the significant difference in electronegativity

56
Q

How does hydrogen bonding occur?

A

it occurs in compounds that have hydrogen atom attached to one of the three most electronegative atoms of nitrogen, oxygen and fluorine. which must also have an available lone pair of electrons

57
Q

What is the strongest type of intermolecular bonding?

A

hydrogen bonding

58
Q

Why is the boiling point of H2O so anonamously high?

A

the hydrogen bonding between the molecules

59
Q

What can form hydrogen bonds?

A

alcohols, carboxylic acids, proteins, amides

Physical Chemistry (11 decks)

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