Brainscape's Knowledge GenomeTM

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


See full index

Higher Chemistry > Chemical Changes And Structure > Flashcards

Chemical Changes And Structure Flashcards

1
Q

How are elements arranged on the periodic table

A

By increasing atomic number

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

What do elements in the same group have in common

A

They have the same number of outer electrons

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

How do elements in the same group differ

A

Going down a group elements have an extra electron shell

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

What is the trend in elements across a period on the periodic table

A

Elements add an outer electron across the periodic table, they also change from metal to non metal elements

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

4 types of bonding found in the first 20 elements

A

Metallic
Covalent molecular
Covalent network
Monatomic

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

Which of the First 20 elements are metallic

A

Lithium
beryllium
Sodium
Magnesium
Aluminium
Potassium
Calcium

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

Which of the first 20 elements are covalent molecular

A

H2
N2
O2
F2
CO2
P4
S8
Carbon in the form of fullerene C60

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

Which of the first 20 elements are covalent networks X3

A

Boron
Silicon
Carbon (diamond, graphite)

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

Which of the first 20 elements are monatomic

A

Helium
Neon
Argon

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

What is meant by covalent radius

A

The measure of the size of an atom from the nucleus to outermost electron

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

Describe the trend in a covalent radius going down a group

A

Covalent radius increases as the number of occupied shells increase

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

Describe trend in covalent radius going along a period

A

Covalent radius decreases across the period as the nuclear charge increases

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

What is meant by the first ionisation energy

A

The energy required to remove one mole of electrons from one mole of gaseous atoms

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

What is meant by the second ionisation energy

A

The energy required to remove the second mole of electrons from one mole of gaseous atoms

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

What is meant by the second ionisation energy

A

The energy required to remove the second mole of electrons from one mole of gaseous atoms

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

Equation for the first ionisation energy of magnesium

A

Mg ——> Mg+ + e-

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

Equation for the second ionisation energy for calcium

A

Ca+ ——> Ca2+ + e-

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

Equation for third ionisation energy of aluminium

A

Al2+ ——> Al3+ + e-

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

Equation for third ionisation energy of aluminium

A

Al2+ ——> Al3+ + e-

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

What is meant by electro negativity

A

A measure of the attraction which an atom has for shared electrons in the bond

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

Describe the trend of electro negativity going down a group

A

Electro negativity decreases due to increase in shielding effect

22
Q

Describe the trend of electro negativity across a period

A

Increases due to the increase in nuclear charge

23
Q

How are covalent bonds formed

A

The result of two positive nuclei being held together by their common attraction for the shared pair of electrons

24
Q

What is meant by polar covalent bonds

A

Form when atoms in a bind have different electro negativity values

25
Q

What happens to the electrons in a polar covalent bond

A

The atom with a larger electro negativity value attracts the bonding electrons closer to it, this means that it has a delta negative charge and the other atom has a delta positive charge

26
Q

What is meant by the term pure covalent

A

Pure covalent bonds are formed when the atoms in the bond have the same electro negativity value

27
Q

Describe the bonding continuum

A

The bonding continuum shows the bonds by increasing ionic character

It goes from pure covalent bonds < polar covalent bind < ionic bond

28
Q

Describe how the states of compounds at room temperature can help identify the type of bonding

A
  • covalent networks are solid
  • covalent molecular are gas or liquid
  • ionic substances are solids
29
Q

Describe how the melting points of compounds can help identify the type of bonding

A

Covalent molecular have low melting points, covalent networks and ionic substances have high melting points

30
Q

Describe the solubility of different compounds

A

Solubility decreases as molecules increase in size. Polar covalent compounds and ionic compounds tend to be soluble in water and other polar solvents, nonpolar compounds are soluble and nonpolar solvents.

31
Q

Describe the electrical conductivity of different compounds

A

Covalent molecular and covalent networks do not conduct electricity except graphite. Ionic bonds can conduct when molten or in a solution

32
Q

What is meant by an intermolecular force

A

Act between molecules these are knows as van der waals forces

33
Q

3 types on inter molecular force

A

London dispersion force
Permanent dipole permanent dipole
Hydrogen bonding

34
Q

How do London dispersion forces arise

A

Formed by the electrostatic attraction between temporary dipoles and induced dipoles which are caused by the movement of electrons

35
Q

Where are London dispersion forces found

A

Can operate between all atoms and molecules

36
Q

Strength of LDFs

A

LDF is the weakest intermolecular force LDF gets stronger when there are more electrons as the strength of LDF increase the melting/boiling point increases

37
Q

Explain when a molecule can be described as being polar

A

When they have permanent dipole - once end of the molecule is positive the other is negative caused by the atoms in the molecule having different electro negativities

38
Q

Explain when a molecule can be described as being non polar

A

When the shape of the molecule is symmetrical

39
Q

Describe a hydrogen bond

A

Formed between one molecule which contains hydrogen and another molecule which contained either nitrogen oxygen or fluorine

40
Q

Strength of a hydrogen bond

A

Strongest intermolecular force

41
Q

Explain how inter molecular forces of attraction affect a molecules physical properties

A

The higher the inter molecular force the higher the melting and boiling points the string the inter molecular force also increases viscosity

42
Q

Why does ammonia and water have high melting points

A

They have hydrogen bonds between their molecules which increases the melting point

43
Q

Explain how to fully predict the solubility of a compound

A

Like dissolves like, so polar compounds will dissolve in polar solvents and non polar compounds will dissolve in non polar solvents

44
Q

What is meant by the term oxidation

A

The loss of electrons it can also mean the gain of oxygen or loss of hydrogen

45
Q

What is meant by the term reduction

A

The gain of electrons it can also mean the loss of oxygen or gain of hydrogen

46
Q

What is meant by a redox reaction

A

When oxidation and a reduction reaction take place at the same time

47
Q

What is meant by the term reducing agent

A

A substance that donates electrons it is oxidised itself

48
Q

What is meant by an oxidising agent

A

A substance that accept electrons it is reduced itself

49
Q

Where are oxidising and reducing agents found in the periodic table

A

Strongest reducing agents are group 1
Strongest oxidising agents group 7

50
Q

How to identify oxidising and reducing agents by their electronegativities

A

Elements with low electronegativities can form ions by losing electrons so act as reducing agents

51
Q

Name some compounds that act as oxidising agents

A

Permanganate, dichromate and hydrogen peroxide

52
Q

Uses of oxidising agents

A

Used to kill fungi bacteria and as a bleach

Higher Chemistry (3 decks)

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