Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem Mr D > Bonding > Flashcards

Bonding Flashcards

(78 cards)

Start Studying
1
Q

How to make something malleable?

A

Add alloy

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

Group 2 bonding compared to group 1 bonding

A
  • stronger electrostatic force of attraction

- higher melting point

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

Metalling bonding drawing

A
  • bigger circles = bigger mass

- number in circles depends on how many electrons lost

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

What does it mean if an atom had a more positive nucleus?

A

-shells closer together so they are smaller

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

What are the 3 types of bonding?

A

Ionic
Covalent
Metallic

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

What is the nature of ionic bonding?

A

Electrostatic attraction between positive + ions

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

What is the nature of covalent bonding?

A

Shared pair of electrons between atoms

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

What is the nature of metallic bonding?

A

Attraction between lattice of positive metal ions + delocalised outer shell electrons

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

Which types of structure have ionic bonding?

A

Ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Types of structure with covalent bonding

A

Simple molecular

Giant covalent

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

Types of structure with metallic bonding

A

Metallic

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

Strength of ionic bonding

A

smaller the ions + the greater the charge on ions, the stronger attraction between positive + negative ions

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

Strength of covalent bonding

A
  • Shorter the bond, the stronger the bond
  • double bonds are stronger than single bonds
  • triple bonds stronger than double bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Strength of metallic bonds

A
  • smaller the metal ions, the greater the charge on ions

- the more delocalised outer shell electrons, the stronger the attraction between ions + electrons

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

What are the 3 types of forces between molecules?

A

Van der Waals forces
Dipole-dipole attractions
Hydrogen bonds

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

How are ions formed?

A
  • When a metal + non-metal react
  • metal atoms lose electrons to form positive ions
  • non metals gain electron to form negative ions
  • both obtain full outer shells
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How are covalent bonds formed?

A

When non-metal + non-metal react

-the atoms share electrons so they both have full outer shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What do 2 shared electrons make?

A

Single bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What do 4 shared electrons make?

A

Double bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What do 6 shared electrons make?

A

Triple bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is a co-ordinate (dative covalent) bond?

A

where both electrons come from the same species

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Why are co-ordinate bonds often drawn with -> rather than - ?

A

To show the direction in which the electrons are donated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What happens when coordinate bonds are formed?

A

They are identical to covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Sodium chloride structure bonding

A

Giant ionic lattice

Ionic bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Magnesium structure + bonding
Giant metallic lattice | Metallic
26
Diamond structure + bonding
Simple covalent molecule / tetrahedral | Covalent
27
Iodine structure + bonding
Simple covalent molecule | Simple covalent
28
Graphite structure bonding
Giant covalent lattice | Covalent
29
Ice structure + bonding
Regular crystal iron structure | Hydrogen
30
How many electrons can some outer shell have?
B 6 P 10 S 12
31
Do both the electrons have to come from different elements?
No Element with 5 can share with element with 3 as 2 can come from element with 5 This is a coordinate bond
32
Shape of molecules list
``` Linear 180 Triangular planar 120 Square planar 90 Tetrahedral 109.5 Triangular based bi pyramid 90 Octahedral 90 ```
33
Which shapes of molecules are 3d ?
Tetrahedral Triangular based bi pyramid Octahedral
34
How to use shape of molecule theory?
``` 1- central atom 2- group (outer shell electron number) 3- charge (+ means lose electron) 4- bonds (no.of bonds) 5- total (add up 2,3,4) 6- divide by 2 (= no. of electron pairs) 7- structure (not shape) 8- look at 6+4 to see if any lone pairs 9- shape 10- bond angle ```
35
What do we use electronegativity for?
Measure the ionic or covalent -ness of a bond
36
Where to electronegativity bonds go from?
1 to 4
37
Electronegativity definition
Measure of tendency of an atom to attract a Hindu f pair of elections in a covalent bond
38
What is the most electronegative element?
Fluorine
39
What 3 things determine the size of electronegativity?
- size of nuclear charge (no. of protons) - distance between the nucleus + outer electron shell - shielding
40
Electronegativity scale from most to least
Ionic Ionic with covalent character Covalent with ionic character Covalent
41
What happens to electronegativity if size of nuclear charge increases?
Increases - lots of protons in nucleus - nuclear charge size increases - increased attraction between nucleus + pair of electrons In covalent bond
42
What happens to electronegativity when size of atom + shielding increase?
Decreases - atom size increases - park of electrons in covalent bond further away from nucleus - more shielding - decreases attraction from nucleus
43
What is a polar bond?
- if the atoms have big differences in electronegativity - meaning one atom holds electrons closer to itself in the bond - one end of bond will be slightly negative due to electrons being there - other end will be slightly positive due to electrons not being there
44
What symbol do we used to show polarity?
delta negative + delta positive
45
When does a non-polar covalent bond happen?
When 2 atoms in a covalent bond have the same electronegativity
46
When does a polar covalent bond happen?
when two atoms in a covalent bond have a different electronegativity
47
What does a non-polar covalent bond mean?
two electrons are shared in covalent bond
48
What does polar covalent bond mean?
two electrons aren’t shared equally
49
What happens with more electronegative atom?
Greater share of 2 electrons | Delta negative
50
What happens with less electronegative atom?
Lower share of electrons | Delta positive
51
Explain CO2 in terms of polar bond
Contains polar bonds but all dipole moments cancel out
52
Explain H2O in terms of plat bonds
contains polar but all duplex moments don’t cancel out
53
Explain CH4 In terms of polar bonds
no polar bonds
54
What are intermolecular forces?
forces between molecules
55
Sodium, + aluminium structure
giant metallic lattice
56
Sodium chloride, silicon dioxide, graphite + graphene structure
Giant ionic lattice
57
Methane, water, iodine + carbon dioxide structures
Simple covalent molecules
58
Which structure are intermolecular forces in?
Simple covalent molecules
59
Are intermolecular forces weaker or stronger that covalent bonds?
Weaker
60
What are the 3 types of bonding in order of weakest to strongest?
Van der Waals Dipole-dipole forces Hydrogen bonding
61
What does van der Waals bonding result in?
Formation of a very slight negative charge at end of the atom
62
What does van der Waals bond state?
at any one moment there could be more electrons at one end of an atom just through chance
63
What does more electrons mean in regards to van der Waals bonding?
More van der Waals bonding
64
What can is instantaneous dipole?
There the other side of the atom has a very slight positive charge where there are less electrons
65
What can instantaneous dipole cause?
- formation of induced dipole in neighbouring atoms | - weak attractive forces between delta positive + delta negative atoms
66
What must you have for dipole-dipole forces?
2 molecules
67
What does dipole-dipole forces cause?
- Attractive forces between molecules | - permanent in a molecule
68
Explain HCL in terms of more dipole dipole bonding?
Chlorine is more electronegative than hydrogen so pulls electrons toward it
69
What does some covalent bond being polar mean?
Means they have an electronegative elements attached to them
70
Why are dipole-dipole forces not for symmetrical shape molecules?
Dipoles cancel eachother out
71
What is a substances boiling point a measure for?
The intermolecular forces present between particles
72
What are hydrides?
Elements joint to hydrogen
74
What is hydrogen bonding related to?
Hydride boiling points
75
What is hydrogen bonding?
The lone pair of electrons on oxygen atoms from other water molecules can interact with hydrogen This forms a very strong intermolecular attraction called hydrogen bonding
76
When does hydrogen bonding form?
When hydrogen is joined to nitrogen oxygen + fluorine
77
What is the hydrogen bond always between?
The lone pair or N, F or O + H delta +
78
What are some importance’s of hydrogen bonding?
Protein folding DNA base pairing Enzyme reactions
79
What do noble gases + hydrides show?
Gradual increase in boiling points

Chem Mr D (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions