C1 Atomic Structure Flashcards
(126 cards)
1
Q
What are group 1 metals known as?
A
Alkali Metals
2
Q
Looking down group 1, do the metals get more or less reactive?
A
More reactive
3
Q
What happens when alkali metals react with water?
A
Rapid reaction, producing an alkaline solution and hydrogen gas
4
Q
What are group 7 elements known as?
A
Halogens
5
Q
Name the 2 halogens which are gases:
A
Fluorine and Chlorine
6
Q
What is the Halogen, Bromine?
A
One of only 2 liquid elements in Group 7
7
Q
What is the Halogen, Iodine?
A
A solid
8
Q
Do halogens exist as monatomic or diatomic molecules?
A
Diatomic
9
Q
What are the elements in group 0 known as?
A
Noble Gases
10
Q
What are diatomic molecules?
A
2 atoms in each molecule
11
Q
Looking down group 7, do the elements get more or less reactive?
A
Less reactive
12
Q
Are Noble Gases monatomic or diatomic?
A
Monatomic
13
Q
What are monatomic elements?
A
Elements which exist as individual atoms
14
Q
How reactive are Noble Gases and why?
A
They are unreactive as they have a full outer shell of electrons
15
Q
Where are transition metals found on the periodic table?
A
Groups 2 and 3
16
Q
Give 3 examples of transition metals:
A
Iron, copper and gold
17
Q
What are the properties of transition metals? Are they dense? What types of compounds do they form?
A
Generally quite dense (heavy) and may form brightly coloured compounds
18
Q
How is the periodic table ordered?
A
In order of increasing atomic number
19
Q
What are the horizontal rows on the periodic table called?
A
Periods
20
Q
What are the vertical columns on the periodic table called?
A
Groups
21
Q
Why do elements in the same group have similar chemical properties?
A
They have the same number of outer electrons and the same valency
22
Q
How many elements are represented by the periodic table?
A
Over 100
23
Q
What does the structure of the atom impact?
A
Everything in the world is made of atoms. The structure of the atom is what gives the element its chemical and physical properties.
24
Q
What are electrons?
A
Negatively charged particles that spin around the positive centre of the atom in circles called energy levels
25
What is the mass of an electron?
0 - so small it is nearly 0
26
What are protons?
Positively charged particles that are contained in the nucleus of the atom (the centre)
27
What is the mass of a proton?
1 amu (atomic mass unit)
28
What are neutrons?
Particles with no charge that are also contained in the nucleus of the atom.
29
What is the mass of a neutron?
1 amu (atomic mass unit)
30
What is the charge of an electron?
-1
31
What is the charge of a proton?
+1
32
What is the charge of a neutron?
0
33
What is the overall charge of every atom?
0. Every atom has no overall charge. While atoms do contain charged particles, they have the same number of positive protons and negative electrons which cancel out causing a neutral charge
34
What is the atomic number?
Number describing how many protons that element has (and also number of electrons)
35
What is the mass number?
Number referring to the number of protons + neutrons in an atom
36
What is an isotope?
An atom with the same atomic number but different mass number
37
What is an atom?
The smallest amount of an element that can still be recognised as that element
38
What is an element?
A substance made up of only one type of atom. An element cannot be broken down into any simpler substance
39
What is a compound?
A substance made up of 2 or more elements chemically bonded together
40
What is an ion?
A charged particle produced by the loss or gain of electrons
41
What is an isotope?
Atoms that have the same number of protons but a different number of neutrons. SAME ATOMIC NUMBER, DIFFERENT MASS NUMBERS
42
What is the nucleus (of an atom)?
The very small and dense centre part of an atom - contains protons and neutrons
43
What is a shell?
An area in an atom around its nucleus where electrons are found
44
What are fullerenes?
Hollow shaped molecules made up of carbon atoms
45
Give the name of the most common fullerene:
C60 Buckminsterfullerene - contains 60 carbon atoms (hence the name)
46
What is the charge of a proton?
+1
47
What is the mass of a proton?
1
48
What is the charge of an electron?
-1
49
What is the mass of an electron?
0 (1/2000th)
50
What is the charge of a neutron?
0
51
What is the mass of a neutron?
1
52
What is a giant lattice structure?
A huge 3D network of atoms or ions, such as a GIANT COVALENT STRUCTURE
53
What is a giant covalent structure?
A huge 3D network of covalently bonded atoms
54
What are simple molecules?
Made when a few non-metal atoms join with strong covalent bonds
55
What is electrostatic attraction?
The pulling force between positive and negative particles. Similar to magnet forces (North -> South)
56
What are intermolecular forces?
The attraction between simple molecules
57
What is a delocalised electron?
An electron that is no longer associated with one particular atom. It can move around and carry a charge
58
What is a neutron?
A dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge
59
What is a proton?
A tiny positive particle found inside the nucleus of an atom
60
What is an electron?
A tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells
61
What type of bonding is METAL + NON-METAL?
Ionic
62
What type of bonding is METAL + METAL
Metallic
63
What type of bonding is NON-METAL + NON-METAL?
Covalent
64
Can ionic substances conduct electricity?
When molten or in solution
65
Do ionic substances have high/low melting and boiling points?
High melting/boiling points
66
What did John Dalton say in 1808?
Atoms were tiny solid spheres which can't be divided
67
What did J.J. Thompson say in 1897?
Discovered electrons - theorised it was a ball of positive charge with electrons randomly embedded in it
68
Who came up with the plum pudding model?
J.J. Thompson
69
What did Rutherford say in 1909?
Observed that after firing alpha particles at gold foil, some were deflected - must be a nucleus in the centre where mass is concentrated
70
Who came up with the nuclear model?
Earnest Rutherford
71
What did Niles Bohr say in 1913?
Electrons were organised in shells/energy levels - orbit at fixed distances
72
Who came up with the Bohr model?
Niles Bohr
73
What did James Chadwick do in 1932?
Discovered the neutron and added it to the nucleus of an atom
74
What is the charge of a proton?
+1
75
What is the mass of a proton?
1
76
What is the charge of an electron?
-1
77
What is the mass of an electron?
0 (1/2000th of an atom)
78
What is the charge of a neutron?
0
79
What is the mass of a neutron?
1
80
Which number is the atomic number?
Bottom number
81
Which number is the atomic mass?
Top number
82
What is the relative atomic mass?
Mean average mass of all isotopes in that element
83
What is the equation for calculating relative atomic mass?
(mass isotope 1 x % isotope 1) + (mass isotope 2 x % isotope 2) / 100
84
What are the 3 things John Dalton did to develop the periodic table?
1. Gave each element a drawing/symbol
2. Ordered list by atomic mass
3. Periodic table arranged in a perfect square
85
What are the 3 things John Newland did to develop the periodic table?
1. Used letter symbols over drawings
2. Ordered by octave's law (a failed theory). Where it didn't apply, he added a seemingly random element
3. Periodic table arranged a perfect square
86
What are the 3 things Dmitri Mendeleev did to develop the periodic table?
1. Elements ordered by atomic number
2. Left gaps for undiscovered elements - predictions of properties came true
3. Not arranged in a perfect square arrangement
87
What is an isotope?
An atom of the same element with the same number of protons and a different number of neutrons - different relative atomic mass
88
What is a metallic bond?
Electrostatic attraction between positive metal ions and delocalised electrons
89
What is a covalent bond?
A shared pair of electrons
90
What is an ionic bond?
Strong electrostatic attraction between oppositely charged ions
91
What is an ion/how is it formed?
Atoms with a positive or negative charge formed when atoms gain or lose electrons to form a full outer shell
92
Which group on the periodic table is Halogens?
7
93
What is the charge of a Halogen - Group 7?
-1
94
What is the trend of reactivity for Group 7 (Halogens)?
The lower down the group, the darker the colour and the higher the melting/boiling point
95
How reactive are Halogens (Group 7)?
Very reactive - only 1 outer electron
96
What is the most reactive element in Group 7?
Iodine
97
What are Noble Gases?
Chemical elements which are not at all reactive - they have a full outer shell of electrons.
98
How reactive are Noble Gases?
They have a full outer shell - do not need to react to form ions
99
What is the name of Group 0 on the periodic table?
Noble Gases
100
What is the charge of Alkali Metals?
+1
101
What is the name of group 1 elements?
Alkali Metals
102
How reactive are Alkali Metals?
Very reactive - only 1 electron in the outer shell
103
What is the trend of reactivity of Alkali Metals?
Every electron going down group 1 has only 1 electron in its outer shell
104
Give 2 properties of transition metals:
Any 2 from:
Lustrous (shiny), malleable, high melting/boiling point, good heat conductors, mostly non-magnetic, coloured compounds, hard and strong, ductile, high density, high conductors of electricity, very unreactive
105
How reactive are transition metals?
Very unreactive
106
What are the properties of ionic compounds?
1. Form crystals
2. Hard and brittle
3. High melting and boiling points
4. Conduct electricity when molten or in solution
5. Good insulators - solid at room temperature
6. Often soluble in water
7. Strong ionic bonds
107
What are polymers also known as?
Macromolecules
108
What is a polymer?
A large molecule made up of many repeating small units
109
What type of bonding is in a polymer?
Covalent bonding
110
What are the properties of polymers?
Strong and do not melt
111
What are polymers used for?
Shopping bags, manufacturing
112
What is graphite?
A giant covalent structure
113
What is graphene?
One layer of graphite
114
What are the properties of graphite?
Strong, high melting/boiling points (covalent bonds), atoms arranged in hexagon layers which can slide over each other (soft surface), bonded to 3 carbon atoms - can conduct electricity
115
What are the properties of graphene?
High melting/boiling points - covalent bonds, can conduct electricity (unbonded electron), strong, inexpensive, lightweight, used in solar cells/batteries
116
Why do metals conduct electricity?
They contain delocalised electrons
117
What are allotropes?
Different structural forms of the same element in the same physical state
118
What is required for a substance to conduct electricity?
They must have some delocalised electrons
119
What are the properties of metals?
All atoms are same size and shape, layers slide easily - more malleable
120
What are the properties of alloys?
Atoms are different sizes - harder for the layers to slide (less malleable/stronger)
121
What are the properties of diamond?
Strong, high melting/boiling points (giant covalent structure), bonded to 4 carbon atoms so can't conduct electricity
122
When are giant lattice structures formed?
When a huge number of non-metal atoms are held together by strong covalent bonds
123
What are the properties of giant lattice structures?
Very high melting/boiling point, do not conduct electricity (except graphite), very strong
124
What are the properties of small molecules/simple molecular substances?
Do not conduct electricity
125
Why do simple molecular substances have a low melting/boiling point?
Weak intermolecular forces
126
What are simple molecular substances?
Small molecules in which the atoms in the molecules are joined by strong covalent bonds but between the molecules are weak intermolecular forces
