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Atomic structure and the periodic table Flashcards

1
Q

What are all substances made from?

A

Atoms

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2
Q

What do atoms contain?

A

Protons, Neutrons, Electrons

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3
Q

What is the raidus of an atom?

A

0.1 nanometers / 1x10^-10

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4
Q

What is in the middle of the atom?

A

Nucleus

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5
Q

What does the Nucleus contain?

A

Protons and Neutrons

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6
Q

What is the raidus of the nucleus?

A

1x10^-14

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7
Q

What charge does the nucleus have?

A

Positive because of the protons

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8
Q

What does the electron do?

A

Move around the nucleus in electron shells

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9
Q

What charge do electrons have?

A

Negative

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10
Q

What charge do protons have?

A

Positive

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11
Q

What charge do neutrons have?

A

Neutral

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12
Q

What is the relative mass of electrons ?

A

1/2000 (sometimes taken as 0)

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13
Q

What is the relative mass of Protons and Neutrons ?

A

Both 1

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14
Q

What charge do atoms have?

A

Atoms are neutral because they have the same number of protons as electrons.The charge of Electrons and protons are the same but opposite so they cancel out.

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15
Q

What charge does an ion have?

A

The number of protons doesn’t equal the number of electrons which means it has an overall charge.

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16
Q

What does a nuclear symbol of an atom tell you?

A

It tells you its atomic (proton)number and mass number

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17
Q

What does the atomic number tell you?

A

(Small number)Atomic number tells you how many protons there are

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18
Q

What does the mass number tell you?

A

(Big number)the total number of protons and neutrons in the atom

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19
Q

How do you find the amount of neutrons?

A

Subtract the atomic number from the mass number

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20
Q

What is an element?

A

An element is a substance made up of atoms that all have the same number of protons in their nucleus.

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21
Q

What are isotopes?

A

They are different forms of the same element,which have the same number of protons but a different number of neutrons.

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22
Q

What is the formula to work out the relative formula of an element?

A

Relative atomic mass =sum of (isotope abundance x isotope mass number) / sum of abundance of all the isotopes

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23
Q

How are compounds formed?

A

They are formed from two or more elements, which are each in fixed proportions throughout the compound and they’re held together by chemical bonds

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24
Q

What does making bonds involve?

A

It involves atoms giving away, taking or sharing electrons.(Only electrons are affected)

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25
What is ionic bonding?
A compound formed from a metal and a non-metal consists of ions.The metal atoms lose electrons to form positive ions and the non-metal atoms gain electrons to form negative ions.The opposite charges of the ions means that they're strongly attracted to each other.
26
What is covalent bonding?
A compound formed from non-metals consists of molecules. Each atom shares an electron with another atom
27
What is a formula?
compounds represented by symbols (like elements)(e.g CO)
28
What is on the left and right of a chemical equation?
Molecules on the left hand side of the equation are called reactants because they react with eachother Molecules on the right hand side of the equation are called products because they've been produced from the reactant
29
What are mixtures?
A subtance made from mixing two or more different substances together but are not chemically bonded
30
How can you seperate mixtures?
Mixtures can be either elements or compounds, they can be seperated out by physical methods such as filtration, crystalistation, simple distillation, fractional distillation and chromotography
31
What are the properties of a mixture?
The propertiese of a mixture are the propertiese of the seperate parts.
32
What is Filtration used for?
filtration is used if your product is an insolube solid that needs to be seperated from a liquid reaction mixture.It can also be used in purfication aswell, solid impurities in the reaction mixture can be seperated out.
33
What are two ways you can seperate a solube salt from a solution?
Evporation and evaporation
34
What does the plum pudding model show?
Shows the atom as a ball of positive charge with electrons stuck in it
35
What did JJ thomsom conclude from his experiments?
That atoms weren't solid spheres. His measurements of charge and mass showed that an atom must contain even smaller, negatively charged particles(electrons)
36
What was Rutherford's experiment?
They fired positively charged alpha particles at an extremely thin sheet of gold.
37
What did Rutherford's experiment show?
some particles were deflected more than expected and a small number were deflected backwards, so the plum pudding couldn't be right.
38
What was Rutherford conclusion from his experiment?
That theres a tiny, positively charged nucleus at the centre where most the mass is concentrated. And a cloud of negative electrons surround this nucleus so the atom is mainly empty space.
39
What did Bohr's Nuclear model suggest?
that all the electrons were contained in shells, he proposed that electrons orbit the nucleus in fixed shells that aren't anywhere in between.
40
What did Further experiments by Rutherford show?
that the nucleus can be divided into smaller particles, which each have the same charge as the hydrogen nucleus .These particles were named protons.
41
How was the perodic table arranged in the early 1800s?
They were arranged by Atomic Mass
42
How did Mendeleev arrange the periodic table and what did he do?
Mendeleev put the elements mainly in order of atomic mass but did switch that order if the peroperties meant it should be changed.He left gaps in the table to make sure that elements with similar properties stayed in the same groups.
43
How is the modern periodic table arranged?
In order of atomic number
44
What are in the colums ?
Elements with similar properties
45
What are groups?
Depending on what group, it tells how many electrons are in the outer shell.
46
What are periods?
each new peroid represents another full shell of electrons.
47
What ions do metals form and where are they in the periodic table?
positive ions and they are towards the bottom and to the left.
48
Where are non-metals located in the periodic table?
They are to the far right and top
49
Why do atoms react?
They react to form a full outer shell, they do this by loosing gaining or sharing electrons.
50
What are some properties of metal?
(All metals have metallic bonding which causes them to have similar basic physical properties ) They're strong, but can be bent or hammered into different shapes Good at conducting heat and electricity High boiling and melting points
51
Properties of non-metals?
``` (dont have metallic bonding) more brittle aren't always solids at room-temp low density not good for conducting electricity ```
52
What are transition metals?
They are in the centre of the peroidic table,they are typical metals
53
Properties of transition metals
More than 1 ion they are often coloured they are good catalysts
54
What are the alkali metals?
Lithium, sodium,potassium, rubidium, caesium and francium
55
What do alkali metals have?
They have 1 electron on the outside so they are very reactive and gives them similar properties
56
What are trends for the alkali metals as you go down group 1
Increasing reactivity Lower melting and boiling points Higher relative atomic mass
57
What ions do group 1 metals form?
1+ ions
58
What do group 1 metals react to form?
ionic compounds, white solids that dissolve in water to form colourless solutions
59
What happens when group 1 metals react with water?
They react vigorously to produce hydrogen gas and metal hydroxides-salts that dissolve in water to produce alkaline solutions More reactive lower down in the group
60
What happens when group 1 metals react with chlorine?
React vigorously when heated in chlorine gas to form white metal chloride salts More reactive lower down in the group
61
What happens when group 1 metals react with oxygen?
They form metal oxide(different types of oxide with form depending on the group 1 metal) Lithium reacts to form lithium oxide Sodium reacts to form a mixture of sodium oxide and soidum peroxide Potassium reacts to form potassium peroxide and potassium superoxide
62
What are group 7 elements?
Halogens , non-metals with coloured vapours
63
What happens as you go down group 7?
Become less reactive- harder to gain electrons because further away from nucleus higher melting and boiling point higher relative atomic mass
64
How do halogens get a full outer shell?
They share electrons via covalent bonding
65
What ions do halogens form?
1- ions called halides
66
Can a more reactive halogen displace a less reactive one?
yes a displacement reaction can occur between a more reactive halogen and the salt of a less reactive one
67
What are group 0 elements?
Noble gasses, they have eight electrons in their outer shell apart from helium which has 2. As is it generally stable they dont need to give up or gain an electron to become more stable.(they dont react much[inert])
68
What do group 0 elements exist as?
monatomic gases - single atoms not bonded to each other
69
Properties of noble gasses
colourless at room temp non-flammable because inert boiling point increase the lower in the group
70
Why does the boiling point of noble gasses increase lower in the group?
There is an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome.

Chemistry (10 decks)

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