Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > The Periodic Table and energy > Flashcards

The Periodic Table and energy Flashcards

(i) The periodic table: periodic and group properties (ii) Enthalpy changes and their determination (iii) Rates of reaction (iv) Reversible reactions and chemical equilibrium (v) Consideration of energy and yield in improving sustainability. (86 cards)

Start Studying
1
Q

What are groups in the periodic table?

A

They are vertical columns that have elements with the same number of electrons in their outer shell and so they have similar chemical properties.

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

What are periods in the periodic table?

A

They are horizontal rows that have elements with the same number of highest energy electron shell

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

How are the elements arranged in the periodic table?

A

The elements are arranged in order of increasing PROTON number

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

What is Periodicity?

A

It is a pattern of repeating trends across periods

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

What is the periodic trends for electron configuration across periods?

A

Across periods, each successive elements gains one electron

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

What is the periodic trends for electron configuration down a group?

A

Down a group, the number of electrons in each outermost shell and type of sub shell stays the same

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

What is Ionisation energy?

A

it is the energy needed to remove electrons

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

What is the first ionisation energy?

A

It is the energy needed to remove 1 mole of electrons from 1 mole of gaseous atom to form one mole of gaseous 1+ ions

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

Factors affecting IE

A

Atomic radius
Nuclear charge
Electron shielding

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

How does Atomic radius affect IE

A

The greater the atomic radius between the nucleus and outer electron shells, the weaker the nuclear attraction and so the smaller than IE

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

How does Nuclear charge affect IE?

A

The more positively charged the nucleus is, the stronger the attraction between the nucleus and the outer electron shells and so the greater the IE

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

How does Electron Shielding affect IE?

A

The greater the number of inner shells, the greater the shielding from the nucleus to the outer electron shell therefore the weaker the nuclear attraction which reduces the IE

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

Trends in IE down a group.

A

Down a group, the IE decreases. This is because the atomic radius increases because there are more inner shells so shielding increases. This increased shielding decreases the nuclear attraction between the nucleus and the outer electron so less energy is needed to remove them, so IE decreases.

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

Trends in IE across a period

A

Across a period, the IE increases. This is because nuclear charge increases, which increases the nuclear attraction between the nucleus and outer electron shell, decreasing the atomic radius. This requires more energy to remove the outer electron so IE increases

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

Exceptions to increasing IE across period 2 and 3- Be to B

A

In Boron, the outer electron is in a p-sub-shell which is of a higher energy than a s-sub-shell and also further away from the nucleus. Because of this, the 2p electron in Boron is easier to remove than the 2s electron so it has a lower IE than beryllium

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

Exceptions to increasing IE across period 2 and 3- N to O

A

Oxygen has a lower IE than Nitrogen because one of oxygen 2p orbitals has a pair of electrons which repel each other making it easier to remove an electron.

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

What does this provide evidence for?

A

It provides evidence for the existence of sub-shells, their energies and how orbitals fill with electrons

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

What predictions can be made from successive IE values?

A
  1. The number of electrons in their outer electron shell which equals the group number
  2. the identity of the element
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are allotropes?

A

They are different forms of the same element in the same state.

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

What are the 3 allotropes of carbon?

A

Diamond, Graphite and Graphene

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

What are giant covalent structures?

A

They are structures that contain many billions of atoms held together by a network of strong covalent bonds.

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

What elements form giant covalent lattices?

A

Boron, carbon and silicon

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

Properties of Giant covalent structures

A
  1. High MP and BP
  2. They are insoluble in water
  3. They cannot conduct electricity with exceptions of graphite and graphene
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why do giant covalent structures have high MP and BP?

A

This is because of the strong covalent bond between the molecules which require high temperatures to provide the large quantity of energy needed to break them.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Why are giant covalent structures insoluble in water?
They are insoluble because the covalent bonds holding the atoms in the lattice are far too strong to be broken by interactions with solvents
26
Why can't most giant covalent structures (diamond and silicon) conduct electricity?
They cannot conduct electricity because all 4 outer electrons are involved in covalent bonding so they cannot move and carry electricity
27
Why can graphite (and so graphene) conduct electricity?
In graphite, three outer-shell electrons are involved in covalent bonding within each layer, so it has one delocalised electron that is free to move and carry charge.
28
What is the bond shape in diamond?
It forms a tetrahedral shape as each carbon atom is covalently bonded to 4 other carbon atoms
29
What is the bond shape in graphite?
It forms a hexagonal layer with bond angles of 120° by electron pair repulsion
30
What is metallic bonding?
It is the strong electrostatic force of attraction between metal cations and delocalised electrons.
31
What type of structure do metals form?
Metals form a giant metallic lattice
32
Properties of metals
1. High MP and BP 2. Good conductors of electricity 3. Good thermal conductors 4. Malleable and ductile 5. Insoluble
33
Why do metals have high MP and BP?
This is because of the strong electrostatic force of attraction between the cations and delocalised electrons which require large amount of energy to overcome
34
What does the MP of metals depend on?
It depends on the size of the charge and the number of delocalised electrons per atom.
35
Why are metals good thermal conductors?
This is because the delocalised electrons can pass kinetic energy to each other.
36
Why are metals good electricity conductors?
This is because the delocalised electrons are free to move and carry charge through the lattice
37
Why do simple molecular structures have low MP and BP?
This is because of the weak induced dipole dipole forces between their molecules so little energy is needed to overcome them.
38
Why do noble gases have low MP and BP?
This is because they exist as individual atoms resulting in very weak induced dipole-dipole forces.
39
Why are Group 2 elements described as reducing agents?
They are described as reducing agents because they cause other species to gain electrons (reduction) while they become oxidised
40
Trend in reactivity down Group 2
Reactivity increases down Group 2. This is because the atomic radius increases due to the increasing number of inner shells increasing shielding. This increased shielding decreases the nuclear attraction between the nucleus and the outer electron making it easier for the element to lose its outer electron
41
Reaction of Metals with Oxygen
Metal + Oxygen ➡ Metal Oxide
42
Reaction of Metals with water
Metal + Water ➡ Metal hydroxide + Hydrogen
43
Reaction of Metals with Dilute acid
Metal + Dilute acid ➡ Salt + Hydrogen
44
Reaction of Metal Oxide with water
Metal Oxide + water ➡ Metal Hydroxide which dissociates releasing OH- into the solution making it more alkaline
45
Trend in solubility of Metal Hydroxides
Down the group, the metal hydroxides solubility increases so the solution becomes more alkaline increasing pH
46
What is Calcium hydroxide used for?
It is used by farmers to neutralise the soil's acidity forming neutral water.
47
What is Magnesium hydroxide and Calcium carbonate used for?
They are used to treat indigestion by neutralising stomach acid (HCl)
48
Equation of Magnesium Hydroxide with stomach acid (HCl)
Mg(OH)2 (s) + 2HCl (aq) ➡ MgCl2 (aq) + 2H2O (l)
49
Equation of Calcium Carbonate with stomach acid
CaC03 (s) + 2HCl (aq) ➡ CaCl2 (aq) + CO2 (g) + H20 (l)
50
Ionic equation for neutralisation reaction
H+ (aq) + OH- (aq) ➡ H20 (l)
51
How do halogens exist as at RTP?
They exists as diatomic molecules- two atoms joined together by a single covalent bond
52
Trend in MP and BP down the halogen group
Down the halogen group, MP and Bp increases. This is because the number of electrons increases, which increases the strength of the induced dipole dipole forces between the molecules which need more energy to break
53
Trend in physical state down Group 7
Fluorine is a pale yellow gas Chlorine is a green gas Bromine is a red-brown liquid Iodine is a shiny grey black solid
54
How do halogens react?
They react by gaining one electron to form a 1- ion
55
Why are Halogens referred to as oxidising agents?
They are referred to as oxidising agents because they cause another species to lose their electron for the halogen to gain
56
Trend in reactivity down Halogen group
Down Group 7, reactivity decreases. This is because the atomic radius increases as there are more inner shells, increasing shielding. This means that there's less attraction to capture an electron from another species so reactivity decreases.
57
Displacement reaction of halogens
A halogen will displace a less reactive halide from its solution.
58
What is the colour of Chlorine in water?
Pale green/colourless
59
What is the colour of Bromine in water?
Orange
60
What is the colour of Iodine in water?
Brown
61
What is the colour of Chlorine in an organic solvent?
Pale green/colourless
62
What is the colour of Bromine in an organic solvent?
Orange
63
What is the colour of Iodine in an organic solvent?
Violet
64
Test for Halides
1. Add dilute nitric acid to remove ions that might interfere with the test 2. Add silver nitrate- AgNO3. A precipitate of silver halide will be formed
65
What is the colour of Silver chloride precipitate?
White precipitate
66
What is the colour of Silver bromide precipitate?
Cream precipitate
67
What is the colour of Silver iodide precipitate?
Yellow precipitate
68
What other test can be used to confirm the halide present?
Adding ammonia solution
69
Solubility of the different halides in ammonia solution
Silver chloride- soluble in both dilute and concentrated ammonia Silver bromide- soluble in only concentrated ammonia Silver iodide- soluble in neither dilute nor concentrated ammonia.
70
What is a disproportionation reaction?
This is a redox reaction in which the same element is both oxidised and reduced
71
Examples of disproportionation reactions
Chlorine with water and; Chlorine with cold, dilute sodium hydroxide
72
Equation reaction of chlorine with water
Chlorine + water ➡ Chloric (I) acid + Hydrochloric acid Cl2 (g) + H2O (l) ➡ HClO (aq) + HCl (aq)
73
Equation reaction of Chloric (I) acid with water
Chloric (I) acid + water ➡ Chlorate (I) ion + Hydronium ion HClO (aq) + H2O (l) ➡ ClO- (aq)+ H30+ (aq)
74
Equation reaction of chlorine with cold, dilute sodium hydroxide
Chlorine + Sodium hydroxide ➡ Sodium chlorate (I) + Sodium chloride + water Cl2 + 2NaOH ➡ NaClO + NaCl + H2O
75
What is sodium chlorate (I) used as?
It is used as household bleach
76
What is chlorine used for?
It is used in water purification by killing water borne microorganisms
77
Risks of using chlorine in water
1. It can form chlorinated hydrocarbons which are carcinogenic- cancer causing 2. It is a toxic gas which is harmful.
78
What are the three anions we can test for?
1. Sulphate- SO4 2. Carbonate- CO3 3. Halide ions, Cl-, Br- and I-
79
Test for sulphate ions
1. Add dilute HCl and Barium chloride If the unknown solution contains sulphate ions, then a **white** precipitate will be formed. Ba2+ (aq) + SO4 (aq) ➡ BaSO4 (s)
80
Test for carbonate ions
1. Add dilute acid (eg nitric acid or hydrochloric acid) to the unknown sample. If carbonate is present, CO2 will be released 2. Bubble the CO2 through lime water (calcium hydroxide) and the lime water turns cloudy.
81
Test for Ammonium ion, NH4+
Add sodium hydroxide to the unknown solution and warm the mixture. NH4+ + OH- ➡ NH3+ H2O Ammonia is a gas and can be tested using a damp red litmus paper which will turn blue in the presence of ammonia.
82
What are the standard conditions?
100kPa, 298K (25°C), 1 mol/dm^3
83
What is the standard enthalpy change of combustion?
It is the enthalpy change when 1 mole of a substance is completely burned in oxygen under standard conditions with all the elements in their standard state.
84
What is the standard enthalpy change of formation?
It is the enthalpy change when 1 mole of a compound is formed from its elements under standard states, in standard conditions.
85
What is standard enthalpy change of neutralisation?
It is the enthalpy change when 1 mole of water is formed when an acid and a base react in a neutralisation reaction under standard conditions with all elements in their standard states.
86

Chemistry (3 decks)

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