1
Q
What type of bonding involves electrostatic attraction between oppositely charged ions?
A
Ionic bonding
Occurs when electrons are transferred from one atom to another.
2
Q
What structure is formed by oppositely charged ions arranged in a regular repeating pattern?
A
Ionic lattice
The lattice extends in all directions in a giant structure.
3
Q
What type of ion is formed when an atom loses one or more electrons?
A
Cation
Cations are positively charged ions.
4
Q
What type of ion is formed when an atom gains one or more electrons?
A
Anion
Anions are negatively charged ions.
5
Q
True or False:
Ionic bonding involves the sharing of electrons between atoms.
A
False
Sharing occurs in covalent bonding.
6
Q
Which ion has the formula SO₄²⁻?
A
Sulfate
A common polyatomic ion in many salts.
7
Q
Which ion has the formula OH⁻?
A
Hydroxide
Found in alkalis such as sodium hydroxide.
8
Q
Which ion has the formula NO₃⁻?
A
Nitrate
Common in fertilisers and nitric acid salts.
9
Q
Which ion has the formula CO₃²⁻?
A
Carbonate
Found in compounds such as calcium carbonate.
10
Q
Which ion has the formula NH₄⁺?
A
Ammonium
The only common positively charged compound ion.
11
Q
Fill in the blank:
Group 1 elements typically form ions with a charge of _______.
A
+1
They lose one electron to form stable ions.
12
Q
Fill in the blank:
Group 7 elements typically form ions with a charge of _______.
A
−1
They gain one electron to achieve a full outer shell.
13
Q
What rule must be satisfied when writing the formula of an ionic compound?
A
Total charge must equal zero.
Positive and negative charges must balance.
14
Q
True or False:
The formula of magnesium oxide is MgO because Mg²⁺ and O²⁻ charges balance in a 1:1 ratio.
A
True
The simplest whole number ratio is used.
15
Q
What determines the ratio of ions in an ionic compound formula?
A
Ionic charges
The ratio ensures overall electrical neutrality.
16
Q
What type of bond forms when two atoms share a pair of electrons?
A
Covalent bond
Typically occurs between non-metal atoms.
17
Q
How is a single covalent bond usually represented in structural formulas?
A
line
Each line represents one shared pair of electrons.
18
Q
Fill in the blank:
A single covalent bond contains one _______ pair of electrons.
A
shared
Each atom contributes one electron to the pair.
19
Q
What is present between atoms in a double covalent bond?
A
Two shared pairs of electrons
Represented by two lines between atoms.
20
Q
What is present between atoms in a triple covalent bond?
A
Three shared pairs of electrons
Represented by three lines between atoms.
21
Q
True or False:
Covalent bonding involves the transfer of electrons between atoms.
A
False
Transfer occurs in ionic bonding.
22
Q
What type of bond forms when both electrons in the shared pair are donated by one atom?
A
Dative covalent bond
Also known as a coordinate bond.
23
Q
Fill in the blank:
A dative covalent bond forms when one atom donates a _______ pair of electrons.
A
lone
The electron pair forms the shared bond.
24
Q
How is a co-ordinate bond represented in a diagram?
A
Arrow
The arrow points from the donor atom to the acceptor atom.
25
# True or False:
Once formed, a **dative covalent bond** is indistinguishable from other covalent bonds.
True
## Footnote
The bond behaves the same as a normal covalent bond.
26
Which **atom** in a **co-ordinate bond** must have a **lone pair** available for donation?
Donor atom
## Footnote
The acceptor atom must have an empty orbital.
27
What must the **acceptor atom** provide in order for a **co-ordinate bond to form**?
Empty orbital
## Footnote
The donated electron pair occupies this orbital.
28
What type of **bonding** involves attraction between **positive metal ions and delocalised electrons**?
Metallic bonding
## Footnote
Found in metals and alloys.
29
What **structure** are positive metal ions **arranged in within a metal**?
Lattice
## Footnote
A regular repeating arrangement of metal ions.
30
# True or False:
In metallic bonding, electrons are **fixed between two atoms**.
False
## Footnote
The electrons are delocalised and move freely.
31
What **term** describes electrons that are **not associated with a single atom** in a metal?
Delocalised electrons
## Footnote
They move throughout the metallic lattice.
32
What **attraction** holds the **metallic lattice** together?
Electrostatic attraction
## Footnote
Between positive metal ions and delocalised electrons.
33
# Fill in the blanks:
**Metals conduct electricity** because they contain mobile _\_\_\_\_\_\_ _\_\_\_\_\_\_.
delocalised electrons
## Footnote
These electrons can carry charge through the structure.
34
What type of **ions** are present in a **metallic lattice**?
Positive metal ions
## Footnote
Formed when metal atoms lose outer electrons.
35
# True or False:
Metallic bonding occurs between **metal atoms and non-metal atoms**.
False
## Footnote
It occurs only between metal atoms.
36
What are the **four main types of crystal structure** found in solids?
1. Ionic
2. Metallic
3. Macromolecular/ Giant Covalent
4. Molecular
## Footnote
These structures differ in bonding and intermolecular forces.
37
What type of **structure** consists of **oppositely charged ions** arranged in a **giant lattice**?
Ionic lattice
## Footnote
Strong electrostatic attractions exist between ions.
38
What type of **structure** consists of **positive ions** in a **lattice** surrounded by **delocalised electrons**?
Metallic lattice
## Footnote
This structure is responsible for metallic conductivity.
39
What type of **structure** forms a **giant network of atoms** joined by **covalent bonds**?
Macromolecular/ Giant Covalent
## Footnote
Also known as giant covalent structures.
40
What type of **structure** consists of **discrete molecules** held together by **intermolecular forces**?
Molecular
## Footnote
Intermolecular forces are weaker than covalent bonds.
41
Which **giant covalent structure** is formed by **carbon atoms** each bonded to four others in a **tetrahedral arrangement**?
Diamond
## Footnote
Very strong covalent bonds give diamond a very high melting point.
42
Which **form of carbon** has layers of atoms arranged in **hexagons** with **delocalised electrons between atoms**?
Graphite
## Footnote
Delocalised electrons allow graphite to conduct electricity.
43
# True or False:
Diamond can conduct electricity because it has **delocalised electrons**.
False
## Footnote
All electrons are involved in covalent bonds.
44
Which **solid** consists of molecules **held together by hydrogen bonding** in a lattice?
Ice
## Footnote
Hydrogen bonds exist between water molecules.
45
Which **molecular solid** forms a lattice of I₂ molecules **held together by intermolecular forces**?
Iodine
## Footnote
Weak intermolecular forces give iodine a relatively low melting point.
46
What type of **structure** does **magnesium** have in the solid state?
Metallic
## Footnote
Positive Mg²⁺ ions in a sea of delocalised electrons.
47
What type of **crystal lattice** does **sodium chloride** form?
Ionic
## Footnote
Na⁺ and Cl⁻ ions arranged in a giant ionic lattice.
48
# Fill in the blanks:
**Giant ionic lattices** have **high melting points** because of strong _\_\_\_\_\_\_ _\_\_\_\_\_\_ between ions.
electrostatic attractions
## Footnote
Large amounts of energy are needed to overcome these forces.
49
Why can **graphite** conduct electricity while **diamond** cannot?
Graphite has delocalised electrons.
## Footnote
Diamond lacks free electrons to carry charge.
50
# Fill in the blanks:
During a **change of state**, energy is used to overcome _\_\_\_\_\_\_ _\_\_\_\_\_\_.
Intermolecular forces
## Footnote
Covalent bonds usually remain intact.
51
# True or False:
Molecular substances generally have **lower melting points** than giant covalent structures.
True
## Footnote
Intermolecular forces are weaker than covalent bonds.
52
What term describes a **pair of electrons involved in forming a covalent bond**?
Bonding pair
## Footnote
Shared between two atoms.
53
What term describes a **pair of outer-shell electrons not involved in bonding**?
Lone pair
## Footnote
Also called a non-bonding pair.
54
# Fill in the blanks:
Electron pairs arrange themselves as _\_\_\_\_\_\_ _\_\_\_\_\_\_ as possible around the **central atom**.
far apart
## Footnote
This minimises repulsion between electron pairs.
55
Which type of **electron pair repulsion** is the **strongest**?
Lone pair–lone pair repulsion
## Footnote
Lone pairs occupy more space around the atom.
56
Which type of **electron pair repulsion** is the **weakest**?
Bond pair–bond pair repulsion
## Footnote
Bonding pairs are held between nuclei.
57
# True or False:
**Lone pairs** repel **more strongly** than bonding pairs.
True
## Footnote
This reduces bond angles in molecules.
58
What **shape** is formed when **two bonding pairs** surround a central atom with **no lone pairs**?
Linear
## Footnote
Bond angle is 180°.
59
What **shape** results from **three bonding pairs and no lone pairs** around the central atom?
Trigonal planar
## Footnote
Bond angle is 120°.
60
What **shape** results from **four bonding pairs and no lone pairs** around the central atom?
Tetrahedral
## Footnote
Bond angle is 109.5°.
61
What **shape** results when **three bonding pairs and one lone pair** surround a central atom?
Trigonal pyramidal
## Footnote
Bond angle is about 107°.
62
What **shape** results when **two bonding pairs and two lone pairs** surround a central atom?
Non-linear
## Footnote
Also called bent or V-shaped.
63
# Fill in the blank:
**Lone pairs** reduce **bond angles** because they cause greater _\_\_\_\_\_\_ between electron pairs.
repulsion
## Footnote
Lone pairs occupy more space than bonding pairs.
64
How many **electron pairs** can surround the **central atom** in molecules typically studied at this level?
Up to six
## Footnote
Includes both bonding and lone pairs.
65
# True or False:
**Molecular shape** is determined only by **bonding pairs of electrons**.
False
## Footnote
Lone pairs also affect the final shape.
66
What is the ability of an atom to **attract the bonding pair of electrons in a covalent bond** called?
Electronegativity
## Footnote
Values differ between elements and influence bond polarity.
67
What type of **bond** forms when two atoms with **different electronegativities** share electrons **unequally**?
Polar covalent bond
## Footnote
Electron density is pulled towards the more electronegative atom.
68
What **symbol** is used to show a **slight positive charge in a polar bond**?
δ⁺
## Footnote
Indicates lower electron density.
69
What **symbol** is used to show a **slight negative charge in a polar bond**?
δ⁻
## Footnote
Indicates higher electron density.
70
# True or False:
A polar bond occurs when **electrons are shared equally between atoms**.
False
## Footnote
Equal sharing produces a non-polar bond.
71
What term describes the **separation of charge** that occurs in a **polar molecule**?
Permanent dipole
## Footnote
One end of the molecule is slightly positive and the other slightly negative.
72
# Fill in the blank:
A **molecule** has a **permanent dipole** when the centres of positive and negative _\_\_\_\_\_\_ do not coincide.
charge
## Footnote
Caused by polar bonds and molecular shape.
73
Why might a molecule containing polar bonds have **no permanent dipole**?
Dipoles cancel.
## Footnote
Symmetrical shapes cause bond dipoles to balance.
74
# True or False:
**Carbon dioxide** has polar bonds but no permanent dipole.
True
## Footnote
The linear shape causes bond dipoles to cancel.
75
What must be present in a **molecule** for a **permanent dipole** to form?
Polar bonds and asymmetrical shape.
## Footnote
Both bond polarity and molecular geometry matter.
76
# Fill in the blank:
Differences in _\_\_\_\_\_\_ between atoms cause **polar covalent bonds**.
electronegativity
## Footnote
The greater the difference, the more polar the bond.
77
What are the **weak forces of attraction** that occur **between molecules** called?
Intermolecular forces
## Footnote
These forces influence physical properties such as boiling point.
78
What type of **intermolecular force** occurs between **molecules with permanent dipoles**?
Permanent dipole–dipole forces
## Footnote
Occurs when molecules contain polar bonds and an overall dipole.
79
What type of **intermolecular force** arises from **temporary fluctuations in electron distribution**?
Induced dipole–dipole forces
## Footnote
Also called London or dispersion forces.
80
# Fill in the blanks:
**Induced dipole–dipole forces** are also known as _\_\_\_\_\_\_ _\_\_\_\_\_\_ forces.
London dispersion
## Footnote
Often collectively called van der Waals forces.
81
What type of **intermolecular force** occurs when **hydrogen is bonded to nitrogen, oxygen or fluorine**?
Hydrogen bonding
## Footnote
This is the strongest common intermolecular force.
82
# True or False:
**Hydrogen bonding** is a type of **covalent bond**.
False
## Footnote
It is an intermolecular force, not a covalent bond.
83
Why are **hydrogen bonds** particularly **strong** compared with other intermolecular forces?
Large electronegativity difference
## Footnote
This creates a highly polar H–X bond.
84
How do stronger intermolecular forces affect **boiling points**?
Increase boiling point.
## Footnote
More energy is required to separate molecules.
85
# True or False:
Substances with only **London forces** usually have **lower boiling points** than those with hydrogen bonding.
True
## Footnote
London forces are the weakest intermolecular forces.
86
Why does **ice** have a **lower density than liquid water**?
Hydrogen bonding forms an open lattice.
## Footnote
The structure holds molecules further apart.
87
Why does **water** have an **unusually high boiling point** compared with similar molecules?
Hydrogen bonding
## Footnote
Extra energy is required to break these interactions.
88
# Fill in the blank:
**Intermolecular forces** are _\_\_\_\_\_\_ than covalent bonds.
weaker
## Footnote
Therefore molecular substances usually have lower melting points.
89
What **property of molecules** mainly determines the **strength of induced dipole–dipole forces**?
Number of electrons
## Footnote
Larger electron clouds are more easily distorted.
90
# True or False:
All molecules experience **induced dipole–dipole forces**.
True
## Footnote
These forces occur even in non-polar molecules.
A-Level Chemistry (AQA)
flashcards
Decks in class (34)
# Cards
-
3.1.1 Atomic structure50
-
3.1.2 Amount of substance47
-
3.1.3 Bonding90
-
3.1.4 Energetics62
-
3.1.5 Kinetics55
-
3.1.6 Equilibria & Kc24
-
3.1.7 Redox equations17
-
3.1.8 Thermodynamics27
-
3.1.9 Rate equations24
-
3.1.10 Kp12
-
3.1.11 Electrode potentials46
-
3.1.12 Acids and bases69
-
3.2.1 Periodicity22
-
3.2.2 Group 2 metals24
-
3.2.3 Group 7 (halogens)31
-
3.2.4 Period 3 oxides35
-
3.2.5 Transition metals95
-
3.2.6 Ions in aqueous solution39
-
3.3.1 Intro to organic chemistry42
-
3.3.2 Alkanes49
-
3.3.3 Halogenoalkanes36
-
3.3.4 Alkenes36
-
3.3.5 Alcohols43
-
3.3.6 Organic analysis36
-
3.3.7 Optical isomerism12
-
3.3.8 Aldehydes & ketones20
-
3.3.9 Carboxylic acids & derivatives25
-
3.3.10 Aromatic chemistry29
-
3.3.11 Amines41
-
3.3.12 Polymers24
-
3.3.13 Amino acids, proteins, DNA61
-
3.3.14 Organic synthesis12
-
3.3.15 NMR spectroscopy14
-
3.3.16 Chromatography12
