Year 10 Flashcards
(102 cards)
1
Q
What sort of reaction would you expect to get from dropping lithium in water?
A
It would fizz and float on the surface of the water.
2
Q
2Na + 2H2O =
A
= 2NaOH + H2
(Sodium hydroxide = NaOH)
(alkaline solution)
3
Q
List the Group 1 metals
A
Lithium, Sodium, Potassium, Rubidium, Caesium, Francium.
4
Q
How do you work out relative atomic mass?
A
Ar = ((mass of one isotope x % abundance) + (mass of other isotope x % abundance))/ 100
5
Q
Define relative atomic mass (Ar)
A
The relative atomic mass of an element is the weighted average of the atomic masses of the isotopes in the element.
6
Q
Define Atomic mass
A
The mass of a single atom of an element measured in units that are equal to 1/12th of a carbon-12 atom.
i.e. one proton or neutron weighs 1 unit.
7
Q
Why are the Group 1 metals called the alkali metals?
A
They form an alkaline solution when mixed with water.
8
Q
Physical properties of the alkali metals. (7)
A
Soft Shiny Tarnish faster than other elements Highly reactive Low melting points Get more dense going down the group Melting + boiling points decrease going down the group
9
Q
Sodium with chlorine equation
A
2Na + Cl2 –> 2NaCl
10
Q
H+
A
Hydrogen cation
11
Q
Li+
A
Lithium cation
12
Q
Na+
A
Sodium cation
13
Q
K+
A
Potassium cation
14
Q
Rb+
A
Rubidium cation
15
Q
Cs+
A
Caesium cation
16
Q
Be2+
A
Beryllium cation
17
Q
Mg2+
A
Magnesium cation
18
Q
Ca2+
A
Calcium cation
19
Q
Sr2+
A
Strontium cation
20
Q
Ba2+
A
Barium cation
21
Q
B3+
A
Boron cation
22
Q
Al3+
A
Aluminium cation
23
Q
Ga3+
A
Gallium cation
24
Q
Ag+
A
Silver cation
25
Cu2+
Copper cation
26
Fe(II)2+
Iron (II) cation
27
Fe(III)3+
Iron (III) cation
28
Pb2+
Lead cation
29
Zn2+
Zinc cation
30
NH4+
Ammonium cation
31
N3-
Nitride anion
32
P3-
Phosphide anion
33
As3-
Arsenide anion
34
O2-
Oxide anion
35
S2-
Sulfide anion
36
Se2-
Selenide anion
37
Te2-
Telluride anion
38
F-
Fluoride anion
39
Cl-
Chloride anion
40
Br-
Bromide anion
41
I-
Iodide anion
42
OH-
Hydroxide anion
43
CO3^2-
Carbonate anion
44
SO4^2-
Sulphate anion
45
NO3^-
Nitrate anion
46
NH4^+
Ammonium cation
47
Ag+
Silver cation
48
Pb^2+
Lead cation
49
Ionic bond
When an atom gives a valence electron to another atom to complete its or the other atom's outer shell.
e.g. a sodium atom gives its outer electron to a chlorine atom to complete both their outer shells.
50
Covalent bond
When two atoms share an electron to complete their outer shells.
e.g. two hydrogen atoms share both their electrons to have a full outer shell.
51
What represents what in a dot and cross diagram?
A dot for the nucleus and normal electrons, and a cross for any donated or shared electrons.
52
Which molecules have covalent bonds?
| 5 examples
```
methane (CH4)
hydrogen (H2)
Chlorine (Cl2)
oxygen (O2)
hydrogen chloride (HCl)
```
53
Electrostatic charge attraction in covalent bond?
The positive nuclei are attracted to the negative shared electrons.
54
What shape is methane?
A tetrahedron.
| This is the furthest apart the positive hydrogen nuclei can be.
55
Which is stronger in water - the covalent bonds between the atoms, or the intermolecular forces?
The covalent bonds.
56
Why are ionic structures typically crystalline?
They form a lattice shape with their ions.
57
What is oxidation?
When an atom or molecule loses electrons in a reaction.
58
What is reduction?
When an atom or molecule gains electrons in a reaction.
59
What happens to iron in a reaction?
It goes to iron (II)/Fe2+ or iron (III)/Fe3+.
60
Suffixes -ate and -ide
-ate means there is oxygen involved, -ide means it is just the elements in the name
61
Define lattice
A regular repeating structure
62
Define giant ionic lattice
An ionically bonded structure with no individual atoms
63
Why are ionic crystals brittle?
Distortion causes the atoms to move, causing positive to be next to positive and negative to be next to negative. This causes the molecule to split apart.
64
Symbol for a double covalent bond
two lines i.e. O==O
65
Symbol for a single covalent bond
one line i.e. O—O
66
Symbol for a triple covalent bond
three lines
67
Give examples of covalent compounds
Diatomic hydrogen, Diatomic oxygen, Diatomic nitrogen, Carbon dioxide, Ammonia, Methane, Ethane, Water, Hydrogen chloride
68
Simple molecular structures have strong ……….. and weak ………….
strong covalent bonds, weak intermolecular forces
69
Melting and boiling points of simple molecular substances?
low because the intermolecular forces are easily broken
70
Why does silica have a high melting point and what is silica?
It has a giant covalent structure, so the covalent bonds are very strong.
71
Why is graphite a good lubricant?
The layers can slide over each other as there is weak attraction between the layers.
72
Why does graphite conduct electricity?
All its electrons are delocalised
73
Is silica similar to diamond?
Yes, they are both giant covalent structures
74
An allotrope of carbon that forms a ball shape?
buckminsterfullerene (C60)
75
T or F: All sodium, potassium, and ammonium salts are dissolvable
True, e.g. sodium chloride, ammonium sulfate
76
Define an acid
A substance the contains or creates H+ ions
77
Define an alkali
A soluble base that releases OH- ions
78
A base is always…
A metal oxide
A metal hydroxide
A metal carbonate
79
metal + acid is a ____ reaction
redox
80
What is OIL RIG?
Oxidation is Loss Reduction Is Gain
81
What is an H+ ion atomically?
A single proton
82
What is a proton transfer?
Transfer of an H+ ion
83
Difference between a weak and strong acid
```
Weak = partially ionises
Strong = fully ionises
```
84
metal + acid ==>
salt + hydrogen
85
metal oxide + acid ==>
salt + water
86
metal hydroxide + acid ==>
salt + water
87
carbonate + acid ==>
salt + carbon dioxide + water
88
which salts are soluble
all ammonium salts, potassium salts, nitrates, and sodium salts
most chlorides and sulfates
some carbonates and hydroxides
89
why doesn’t copper work for making salts
it doesn’t react
90
why don’t potassium, sodium, and calcium work for making salts
they are too reactive
91
where do you read on a level of liquid in a tube
at the bottom of the meniscus (surface)
92
define titration
using a titrate to measure the concentration of a solution.
93
Top to bottom fractions
```
refinery gases
gasoline
kerosene
diesel oil
fuel oil
bitumen
```
94
Top to bottom fraction colour
```
refinery gases light
gasoline ^
kerosene ||
diesel oil ||
fuel oil v
bitumen dark
```
95
Top to bottom fraction boiling point
```
refinery gases low
gasoline ^
kerosene ||
diesel oil ||
fuel oil v
bitumen high
```
96
Top to bottom fraction viscosity
```
refinery gases low
gasoline ^
kerosene ||
diesel oil ||
fuel oil v
bitumen high
```
97
Methane formulae
Empirical Molecular Structural
| CH4 CH4 CH4
98
Ethane formulae
Empirical Molecular Structural
| CH3 C2H6 CH3 CH3
99
Propane formulae
Empirical Molecular Structural
| C3H8 C3H8 CH3CH2CH3
100
Butane formulae
Empirical Molecular Structural
| C2H5 C4H10 CH3CH2CH2CH3
101
MEPBPH-alkanes
```
Methane
Ethane
Propane
Butane
Pentane
Hexane
```
102
EPB1B2-alkenes
Ethene
Propene
But-1-ene
But-2-ene
