Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

CHEMISTRY - JAY > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

1
Q

how big is the radius of an atom

A

0.1 nanometers ( 1 x 10(-10))

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

what charge has the nucleus got?

A

positive

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

where is most of the mass concentrated in the atom?

A

the nucleus

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

what determines the size of an atom?

A

the volume of electron orbits

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

do electrons have mass?

A

they have virtually no mass

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

whats the overall charge of an atom?

A

neutral (protons and electrons are equal and balanced)

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

what does the atomic number tell you?

A

number of protons (bottom number)

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

what does the mass umber tell you?

A

total number of protons and neutrons (top number)

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

how do you find total number of neutrons?

A

subtract atomic number from the mass number

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

W hat are isotopes?

A

different forms of the same element, they have the same number of protons but a different number of neutrons, they have the same atomic number but different mass numbers. e.g carbon -12 and carbon-13

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

what is relative atomic mass?

A

(Ar) an average mass of an element taking into account all its isotopes

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

what is the formula for Ar

A

sum of (isotope abundance x isotope mass number) / sum of abundance of all isotopes

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

In a compound formed by metals and non metals, do metal atoms lose or gain electrons?

A

lose electrons, they become positively charged.

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

In a compound formed by metals and non metals, do non metal atoms lose or gain electrons?

A

gain electrons, the become negatively charged.

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

Bonding formed by opposite charges reacting is called what?

A

ionic bonding

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

bonding by sharing electrons is called?

A

covalent bonding

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

examples of ionic bonding?

A

sodium chloride, magnesium oxide and calcium oxide.

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

examples of covalent bonding?

A

hydrogen chloride gas, carbon monoxide and water.

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

what is chromatography?

A

a way of separating different dyes in ink.

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

how do you carry out chromatography?

A

1- draw a pencil line near the bottom of a sheet of filter paper.
2-add a spot of ink you want to test to the line and place in a beaker of shallow solvent (e.g water)
3- ensure ink isn’t touching solvent as it will dissolve into the liquid.
4- place a lid on container to avoid solvent evaporating.
5- the solvent will carry ink up the filter paper
6- each dye will move up the paper at different rates so the dye will separate out, each dye will form 1 spot,
7-if dyes are insoluble they will stay on the baseline.
8-when the solvent has nearly reached top of the paper, take the paper out to dry

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

In a chromatography why do you use a pencil

A

because pencil is in soluble.

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

is water always used as a solvent?

A

no, some compound won’t dissolve in water so other solvents such as ethanol are used.

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

What does filtration do?

A

sperate insoluble solids from a liquid reaction mixture.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what is purification?

A

solid impurities in the reaction mixture being filtered out of the reaction mixture.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Name two ways to separate soluble solids from solutions.
evaporation and crystallisation.
26
what is evaporation? (separation)
heating a solution in a evaporating dish to evaporate the solvent making the solution more concentrated. crystals then form.
27
what is crystallisation? (separation)
heating solution in a evaporating dish to evaporate the solvent to leave a more concentrated solution, when the point of crystallisation is noticeable the dish is removed from heat, the salt then forms crystals and is insoluble. crystals are the filtered out.
28
examples of when filtration and crystallisation are used?
to separate rock salt.
29
What is rock salt?
a mixture of salt and sand (grit)
30
is rock salt a compound?
yes
31
is rock salt soluble?
salt dissolves but sand doesn't.
32
How do you separate rock salt?
1- Grind rock salt so salt crystals are small (will dissolve easier) 2- put mixture in water, salt will dissolve but sand will not. 3- filter mixture 4- evaporate water to form salt crystals
33
How can you help salt dissolve?
heat the mixture.
34
What is distillation?
separating liquids from mixtures.
35
what are the types of distillation called?
simple and fractional
36
how do you carry out fractional distillation?
1- heat the solution, the liquid with the lowest boiling point will evaporate first. 2-the vapour will then cool and condense in a condenser, you can then collect it. 3- the res of the solution is then left behind in the flask.
37
what is a condencer?
a tube designed to condense gas. the walls are filled with water to cool the gas.
38
examples of simple distillation
to get pure salt from saltwater. the water evaporates first leaving pure salt in the flask.
39
disadvantages of distillation
you can only use it to separate liquids with very different boiling points.
40
How do you separate liquids with similar boiling points?
Fractional distillation.
41
Give an example of a liquid you could separate by fractional distillation
Crude oil
42
How does fractional distillation work?
Liquids have different boiling points so they evaporate at different temperatures. The liquid with the lowest boiling point will evaporate first.
43
Who described atoms as solid spheres?
John Dalton
44
Who concluded from their experiments that atoms were not solid spheres?
J J Thompson
45
What did J J Thompson’s measurements of charge and mass show about the atom?
The presence of electrons
46
Who invented the plum pudding model?
J J Thompson
47
What does the plum pudding model show?
It shows a ball of positive charge with electrons stuck in it
48
Who showed that the plum pudding model was wrong?
Rutherford
49
Describe rutherfords alpha particles scattering experiments.
Rutherford fired positively charged alpha particles at an extremely thin sheet of gold.
50
From the Plum Pudding model what did Rutherford expect to see in his scattering experiments?
Rutherford expected to see the particles pass straight through the sheet or be slightly deflected bat most.
51
What showed that the Plum Pudding Model couldn't be right?
Some alpha particles were deflected more than expected and some were deflected backwards.
52
What model/idea did rutherford create?
The Nuclear Model of the atom
53
Explain the nuclear model of the atom.
The nuclear model shows the positively charged nucleus at the centre where most of the pass is concentrated. a 'cloud' of negative electrons surrounding the nucleus
54
Who created a more advanced nuclear model?
Bohr.
55
Why did scientists not agree with the theory of a 'cloud'' pf negative electrons?
The electrons would be attracted to the nucleus causing the atom to collapse.
56
What did Bohr's model propose?
Electrons orbit the nucleus in fixed shells. each shell being a fixed distance from the nucleus.
57
Was Bohr's theory well supported?
yes, It was supported by experiments and helped explain lots of scientific observations at the time.
58
What did further experiments show? (after Bohr's theory)
The existence of Protons.
59
What did Rutherford show about protons?
He showed they were smaller particles of the nucleus with the same charge of a hydrogen nucleus.
60
Who provided evidence for neutral particles in the nucleus?
James Chadwick
61
What are shells sometimes referred to as?
Energy levels.
62
What type of energy level is filled first?
Lowest
63
How many electrons are allowed in the first shell?
2
64
How many electrons are allowed in the second shell
8
65
How many electrons are allowed in the third shell?
8
66
In the Early 1800 hundreds what were elements arranged by?
Atomic Mass
67
How did Dmitri Mendeleev arrange his periodic table?
He put elements in order of atomic mass but he switched the order if the properties meant it should be changed
68
Why did Mendeleev leave gaps in his periodic table?
To ensure elements with similar properties stayed in the same groups
69
What did gaps in Mendeleevs periodic table show?
The existence of undiscovered elements.
70
What did isotopes show?
That mendeleevs periodic table was incorrect and needed to be ordered in atomic mass instead.
71
What are similar properties of Metals?
- They are strong and malleable - There great at conducting heat or electricity - They have high boiling and melting points
72
What are properties of non-metals?
- dull looking - brittle - not always solids at room temperature - don't generally conduct electricity - lower density
73
Where are transition metals found between?
Group 2 and Group 3
74
What are transition metals?
They are typical metals
75
What are properties of transition metals?
- They can have more than one ion - They are often coloured - Transition metal compounds make good catalysts
76
What are group 1 elements known as?
Alkali Metals
77
What are the Alkali metals?
Lithium, Sodium, Potassium, Rubidium, Caesium and Francium
78
How many electrons are in the outer shell of alkali metals
One electron
79
What are alkali metals like?
They are all soft and have a low density
80
What are the trends for alkali metals as you go down the group?
- Increasing reactivity (the electron is further away from the nucleus as you go down the group) - lower melting and boiling points - higher relative atomic mass
81
What ions do group 1 elements form?
1+ ions
82
How do alkali metals react with water?
They react vigorously to form hydrogen gas and metal hydroxides ( more violent as you go down the group )
83
How do alkali metals react with chlorine?
They react vigorously to form white chloride salts, as you go down the group the reaction becomes more vigorous.
84
How do group 1 metals react with oxygen?
they react with oxygen to form a metal oxide
85
What oxide does lithium become when reacted with oxygen?
lithium oxide.
86
What oxide does sodium become when reacted with oxygen?
a mixture of sodium oxide and sodium peroxide.
87
What oxide does potassium become when reacted with oxygen?
a mixture of potassium peroxide and potassium superoxide.
88
Whats the difference between alkali metals and transition metals?
- Alkali metals are more reactive then transition metals | - alkali metals are much less dense, strong and hard then the transition metals.
89
What are the group 7 elements also known as?
The halogens
90
What are the halogens?
Non-metals with coloured vapours.
91
What elements are the halogens?
Fluorine, Chlorine, Bromine, iodine and Astatine.
92
What is fluorine?
A very reactive poisonous yellow gas.
93
What is chlorine?
a fairly reactive, poisonous dense green gas.
94
What is Bromine like
A dense, poisonous, red-brown volatile liquid
95
what is iodine?
a dark grey crystalline solid or a purple solid.
96
What are the trends of halogens as you go down the group?
- They become less reactive ( its harder to gain an extra electron because its further from the nucleus) - increasing boiling and melting points - higher relative atomic masses
97
How many electrons do halogens have in their outer shell?
7
98
What can halogens form?
Molecular compounds
99
How do Halogens share their electrons
via covalent bonding with other non-metals
100
What do halogens form with metals?
Ionic Bonds
101
Give and example of a ionic bond formed with a halogen .
Na(+)Cl(-)
102
What do more reactive halogens displace?
less reactive ones
103
What do displacement reactions occur between?
A halogen and a salt of a less reactive one.
104
Give an example of halogen displacement.
Chlorine can displace bromine and iodine to form an aqueous solution of its salt (iodine and bromine)
105
What are group 0 elements also known as?
The noble gases.
106
What are the noble gases?
Helium, Neon, Argon, Krypton, xenon and Radon
107
How many electrons are in the outer shell of a noble gas?
8 except helium which has two.
108
Noble gases are monatomic gases, What does this mean?
they are single atoms not bonds to each other.
109
At room temperature what are noble gases like?
colourless gases
110
What are the trends of noble gases as you go down the group?
- Boiling points increase as you go down the group, this is due to greater intermolecular force as more electrons are in the atoms

CHEMISTRY - JAY (3 decks)

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