Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

iAlevel Chemistry Y1 > Bonding And Structure Ch3 > Flashcards

Bonding And Structure Ch3 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Definition

Ionic Bonding

A

The elctrostatic force of attraction between oppositily charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Factors

Strength of ionic bonding

A
  1. Ionic charge
  2. size of ions

greater charge = stronger bond
smaller size = bond-closer together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Trends

Ionic radii

Between cations and anions

A

Number of protons:elections
State of attraction or repulsion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Trend

Ionic Raddi

Group 1 & 7

A

Down group ions have more elections - ion gets larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Trend

Ionic Radii

Period 2 & 3

A

radius decrease as proton number increase
no shielding
positive charge increase- elctrons attracted strongly- pulled closer to nuclues

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Definition

Isoelectronic

A

two or more elements and/or ions have the same electronic configuration.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Definition

Polarisation

A

The distortion of the electron density of a negative ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Definiftion

Polarising power

A

The ability of a cation to distort the electron density of a neighouring anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Trends

Polarisation

List

A
  1. high charge and small size of the cation.
  2. large size of the anion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Properties

Ionic Compounds

Physical

A

Very high melting point
Very brittle
Don’t electricity unless molten
Is soluble in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Definition

Colvalent Bonding

A

The electrostatic force of attration between a shared paired of electrons and the nuclei of the atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Definition

Dative Covalent Bonding

A

A covalent bond which both electrons comes from the same atom/ spieces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Description

Sigma Bond

A

End-on-end overlap of s or p orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Description

Pi bond

A

sideways overlap of two p-orbitals, Creates a cloud of electrons.

Weaker bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Definition

Octet Rule

A

Outer shell of each atom must have the same number of electrons a the outer shell of a noble gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Definition

Electronegativity

A

The ability of an atom to attract a bonding pair of electrons in a colvalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Trend

electronegativity

A
  1. decrease down a group
  2. increase acrosss a period
18
Q

Electron density

distribution of same electronegativity

A

bonded together by overlap of atomic orbital - symetical shape

19
Q

Electron Density

distribution of different electronegativity

A

bonded together by overlap of atomic orbital - shape not symmetrical

20
Q

Shape of molecules and ions

Why that shape

A

caused by repulsion between the apir of electrons - arrange themselves to minimise repulsion

21
Q

Shape

Linear

Bond Angle + lone Pair

A

180 + no lone pair

22
Q

Shape

Trigonal Planar

Bond angle + lone pair

A

120 + no lone pair

23
Q

Shape

Tetrahedral

Bond angle + lone pair

A

109.5 + no lone pair

24
Q

Shape

Trigonal Pyramidal

Bond angle + lone pair

A

106.7 + one lone pair

25
Q

Shape

V-shaped

Bond angle + lone pair

A

104.5 + two lone pair

26
Q

Shape

Trigonal bipyramidal

Bond angle + lone pair

A

120, 90 + no lone pair

27
Q

Shape

Octahedral

Bond angle + lone pair

A

180,90 + no lone pair

28
Q

Definition

Polarity

Dipole

A

Difference in electronegativity between 2 will result in electrons being pulled further to one end

separation of charge

29
Q

Polar and non-polar

Linear Molecules

example CO2

A

CO2 molecule are polar, but dipoles cancel each other out

NON - POLAR

30
Q

Polar and non-polar

Trigonal Planar Molecule

example BCl3

A

Bonds are polar, but molecules are symmetrical so cancels each other out

NON - POLAR

31
Q

Polar and non-polar

Tetrahedral Molecule

example CCl4

A

CCl4 molecule are polar, it is symmetricalso the dipoles cancel each other out

NON _ POLAR

32
Q

Polar and non-polar

Trigonal Pyramidal Molecule

example NH3

A

NH3 molecule are polar, and dipoles reinforce each other out

POLAR

33
Q

Polar and non-polar

V - shaped

examples H2O

A

Bonds are polar, and dipoles reinforn each other.

POLAR

34
Q

Definition

Metallic Bonding

A

the electrostatic force of attraction between the metal cations and delocalised electrons

delocalised electons;electon that not associated with any single atom

35
Q

Metallic bonding

Sodium (Na)

A

relatively weak metallic bond
each atom donates one electron

to the sea of delocalised electrons

36
Q

Metallic bonding

Potassium (K)

A

weaker than Na metallic bond
ions are larger - weak electrostatic force

between cations and sea of delocalised electrons

37
Q

Metallic Bonding

Magnesium (Mg)

A

Stronger metallic bonding then Na
donates 2 e-
Mg2+ ions smaller

strong force of attraction between ions and delocalised electrons

38
Q

Properties

Metallic Bonding

Physical

A

Malleable
Ductile
Melting point:
number of delocalised electrons per cation
charge:cation

incease across group
decrease down group

39
Q

Giant Covalent Bonding

Diamond

5 points

A

each carbon bonded to 4 other carbons
tetrahedral + 109.5
high melting and boiling point (due to strong c-c covalent bond)
very hard
doesn’t conduct electricity

40
Q

Giant Covalent Bonding

Graphite

5 point

A

each carbon bonded to 3 other carbons
Hexagonal + 120
covalent bond - between carbons
Intermolecular bond (weak) - between layers
high melting / boiling point (strong C-C covalent bond)
conduct electricity

41
Q

Giant Colvalent Bonding

Graphene

3 points

A

Hexagonagal - 120
One atom thick
conducts elelctricity

42
Q

Giant Colvalent Bonding

Silicon Dioxide (Silica)

A

High melting / boiling point
Tetrahedral - 109.5

iAlevel Chemistry Y1 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions