Topic 1 - Atomic Structure And The Periodic Table Flashcards
(106 cards)
1
Q
What are all substances made of?
A
Atoms
2
Q
What is the radius of an atom?
A
0.1 manometers
3
Q
What type or particles are in the nucleus?
A
Protons and neutrons
4
Q
What type of particles are found in shells outside of the nucleus?
A
Electrons
5
Q
What is the charge of an electron?
A
Negative
6
Q
What is the charge of a proton?
A
Positive
7
Q
What is the charge of a neutron?
A
None
8
Q
What is the relative mass of an electron?
A
0
9
Q
What is the relative mass of a proton?
A
1
10
Q
What is the relative mass of a neutron?
A
1
11
Q
The number of protons in an atom is equivalent to what?
A
The number of electrons
12
Q
What is the overall charge of an atom?
A
Neutral
13
Q
What does the atomic number of a nuclear symbol tell you?
A
How many protons (and therefore electrons) an atom has
14
Q
What does the mass number of a nuclear symbol tell you?
A
The relative atomic mass of the atom
15
Q
How do you figure out the number of electrons from a nuclear symbol?
A
Mass number - atomic number
16
Q
What is an element?
A
A substance made up of atoms that are all the same
17
Q
What determines what type of atom and atom is?
A
The number of protons
18
Q
What are isotopes?
A
Different forms of the same element with just a different number of neutrons
19
Q
Atoms and their corresponding isotopes have the same _____ number.
A
Atomic
20
Q
Atoms and there corresponding isotopes have different _____ numbers.
A
Mass
21
Q
What is the relative atomic mass of an element?
A
How much that element weighs depending on the types of isotopes it contains
22
Q
Relative atomic mass of an element =
A
Sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes
23
Q
What is a compound?
A
A mix of elements
24
Q
How are compounds formed?
A
When elements react
25
When stones combine to form compounds, how are they held together?
Chemical bonds
26
What happens to electrons when bonds are made?
They are given, taken or shared
27
A compound of a metal and a non-metal will form what type of bonds?
Ionic bonding
28
What happens to metals in ionic bonding?
They lose electrons and become positive ions
29
What happens to non-metals in ionic bonding?
They gain electrons to become negative ions
30
A compound of non-metals will form what kind of bonds?
Atoms share electrons
31
Are properties of compounds usually similar or different to the elements from which they came from?
No
32
How can we represent compounds?
With formulas
33
If a symbol has a small number after and slightly below it, what does that mean?
There are that many of that specific element in the compound proportionally.
34
If a formula has a large number before it, what does that mean?
You would work out the smaller numbers first. Then double all the elements that are listed in the formula
35
What does it mean if there is a small number after brackets?
Multiply all the elements within the brackets by that number
36
What is the formula of ammonia?
NH3
37
What is the formula of sulphuric acid?
H2SO4
38
What are the two types of chemical equations?
Word and symbol
39
What are the molecules on the left hand side of an equation called?
Reactants
40
What are the molecules on the right hand side of an equation called?
Products
41
What do you have to do to symbol equations?
Balance them
42
What are you allowed to add to an equation to balance it?
Big numbers in front of formulas
43
What is the difference between a compound and a mixture?
Mixtures have no chemical bonds
44
What is the most common mixture?
Air
45
Do mixtures have the same properties of the elements they contain?
Yes
46
Who created a theory of atomic structure in the early 19th century?
John Dalton
47
What was John Dalton’s theory?
That atoms were solid spheres, and different spheres made different elements
48
Who created a theory of atomic structure in 1897?
JJ Tomson
49
What was JJ Thomson’s theory?
The plum pudding model: atoms were balls of positive charge containing negative electrons
50
What did Rutherford prove?
That the plum pudding model was wrong
51
What was Rutherford’s experiment?
Firing positively charged alpha particles at a thin sheet of gold foil
52
What results was Rutherford expecting based on the plum pudding model?
Particles to pass straight through with some rare slight deflection
53
What results did Rutherford get?
Most particles passed through, but a lot were deflected more than expected and a few even deflected backwards
54
What was Rutherford’s theory of atomic structure?
In the centre of an atom was a tiny positive nucleus. Around this was a cloud of electrons and a lot of empty space.
55
What alteration did Bohr make to Rutherford’s atomic structure?
He realised electrons had to be fixed else they’d be attracted to the nucleus, so he proposed they were in fixed shells a certain distance from the nucleus
56
What did Rutherford later prove about atomic structure?
The nucleus could be divided into smaller, positive particles: protons
57
What did James Chadwick prove about the atomic structure?
The nucleus also contained neutral particles: neutrons
58
Which shells are filled first in atoms?
Those closest to the nucleus
59
How many electron fit into the first shell?
2
60
How many electron fit into the 2nd shell onwards?
8
61
How many electrons do atoms want in their outermost shells?
The most possible, 2 or normally 8
62
Which elements have full outer shells?
The noble gases
63
How were elements originally arranged?
By atomic mass
64
What did Dmitri Mendeleev do?
Left gaps, predicted elements and swapped elements around depending on their properties
65
How are elements organised in the modern periodic table?
Atomic number
66
Columns of elements have similar properties, what are they called?
Groups
67
What does the group number tell you about an atom’s electronic structure?
How many electrons are in the outer shell
68
Each new row means another full shell in the atom, what are these rows called?
Periods
69
Which side of the periodic table do metals lie on?
Left
70
Which side of the periodic table do non-metals lie?
Right
71
What type of ions do metals form?
Positive
72
What type of ions do non-metals typically form?
Negative
73
Why do atoms react?
To form full outer shells
74
Why do metals form positive ions?
The number of electrons in their outer shell makes it easier to lose than gain. They are lower in the table so their outer shells are further from the nucleus and have weaker forces of attraction.
75
Why do non-metals form negative ions?
The number of electrons in their outer shells make it easier to gain than lose. They are higher in the table so their outer shells are closer to the nucleus and have stronger forces of attraction
76
A compound of metals will form what type of bonds?
Metallic
77
What are four main properties of metals?
Strong, malleable, conductive, high melting and boiling points
78
What are five main properties of non-metals?
Brittle, not always solids at room temp, full, not conductive, lower densities
79
What are transition metals?
Typical metals, found between groups 2 and 3
80
What are the three specific properties found in transition metals?
More than one ion, coloured, good catalysts
81
What are Group 1 metals known as?
Alkali metals
82
What are the first three alkali metals?
Lithium, sodium, potassium
83
How many electrons do alkali metals have in their outer shells?
1
84
Do alkali metals increase reactivity going up or down the column and why?
Down, because there are more shells therefore weaker forces of attraction therefore the 1 outer electron is more easily lost
85
Going down the column, do alkali metals’ MP and BP increase or decrease?
Decrease
86
How do alkali metals react with water?
Vigorously, producing hydrogen gas and sometimes enough energy to ignite the hydrogen gas
87
How do alkali metals react with chlorine?
Vigorously, producing metal chloride salts
88
How do alkali metals react with oxygen?
Producing metal oxide
89
What are Group 7 elements also known as?
Halogens
90
What are the first four halogens?
Fluorine, chlorine, bromine, iodine
91
What does fluorine look like?
Yellow gas
92
What does chlorine look like?
Green gas
93
What does bromine look like?
Red-brown liquid
94
What does iodine look like?
Grey solid or purple gas
95
What do all the halogen molecules do?
Pair up
96
What happens to reactivity as you go down the halogen column and why?
Decreases, because the outer shell gets further from the nucleus therefore the forces of attraction are weaker therefore it’s harder to gain an electron.
97
How many electrons do the halogens have in their outer shells?
7
98
What types of bonding can halogens do?
Covalent and ionic
99
What happens when a halogen salt reacts with a more reactive halogen?
The more reactive halogen will displace the other
100
What are Group 0 elements also known as?
Noble gases
101
What are the first three noble gases?
Helium, neon, argon
102
How many electrons do noble gases have on their outer shells?
8, or 2 in helium’s case
103
What are they called because of their reactivity?
Inert - barely react with anything
104
What do all noble gases look like?
Colourless gases
105
Are noble gases flammable?
No
106
Do the BPs and MPs increase or decrease going down the column?
Increase
