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Josh Lee Chemistry > Topic 1 - Atomic Structure And The Periodic Table > Flashcards

Topic 1 - Atomic Structure And The Periodic Table Flashcards

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1
Q

What does an atom contain?

A

Protons, neutrons and electrons

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2
Q

How big is the radius of an atom?

A

About 0.1 nanometers

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3
Q

What are features of the nucleus of an atom?

A 
Its in the middle of the atom.
Contains protons and neutrons.
Radius of about 1 x 10^-14
Positively charges
Where most of the mass of an atom is concentrated.
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4
Q

What are the features of an electron?

A

Moves around the nucleus in electron shells.
Negatively charged
Volume of their orbit determines the size of the atom.
Have virtually no mass.

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5
Q

Whats the difference between an ion and an atom?

A

An ion has more/less electrons than protons which then gives itself a charge.
An atom is neutral since the amount of protons and electrons cancel each other out.

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6
Q

Which number on the periodic table is the mass number and atomic number?

A

Mass number is the bigger number (top)

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7
Q

What does the atomic number tell you?

A

Amount of protons

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8
Q

What does the mass number tell you?

A

Total number of protons and neutrons

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9
Q

What is an element?

A

A substance that only contains atoms with the same atomic number

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10
Q

What is an isotope?

A

They are different forms of the same element with same number of protons but different number of neutrons. So same atomic number but different mass numbers.

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11
Q

How do you find relative atomic mass? (Ar)

A

Ar = sum of (isotope abundance x isotope mass number) / sum of all abundances

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12
Q

What is a compound?

A

Substances formed from 2 or more elements. The atoms of each are in fixed proportions and are held together by chemical bonds.

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13
Q

What are the features of a compound formed from a metal and non metal?

A

Consists of ions.
Metal loses electrons to form positive ions and non metal gains electrons to form negative ions.
Opposite charges of ions means they strongly attract to each other.

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14
Q

What are the features of a compound formed from 2 non metals?

A

Consists of molecules.

The atoms share electrons which other atoms (covalent bonding).

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15
Q

Fill in the blanks. Just as elements are represented with _____ , compounds are represented with _____.

A

1) Symbols

2) Formulas

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16
Q

What is a mixture?

A

2 or more elements mixed together but the atoms are not chemically bonded.
Eg air is a mixture of gases like oxygen, nitrogen, carbon dioxide and argon.

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17
Q

How can you use filtration to separate a mixture?

A

Can be used to separate insoluble solids from a liquid.

Can also be used for purification

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18
Q

How can you use evaporation to separate a mixture?

A

Separate soluble solid from a liquid

1) Pour solution into evaporating dish.
2) Slowly heat the solution. The solvent will evaporate and solution will get more concentrated. Eventually, crystals will start to form.
3) Keep heating evaporating dish until all you have left are dry crystals

19
Q

How can you use crystallisation to separate a mixture?

A

Separate soluble solid from liquid if the salt decomposes when heated.

1) Pour solution into evaporating dish and gently heat the solution.
2) Once some solvent has evaporated, or when you see crystals start to form, remove dish from heat and leave solution to cool.
3) The salt should start to form crystals it becomes insoluble in the cold, highly concentrated solution.
4) Filter crystals out of solution and dry them

20
Q

How can you separate rock salt? (Sand and salt mixed)

A

1) Grind mixture to make sure the salt crystals are small.
2) Put mixture in water and stir. The salt will dissolve but sand won’t.
3) Filter mixture. The sand wont fit through but the salt water will.
4) Evaporate the water from the salt

21
Q

At the start of the 19th century who described atoms as solid spheres?

A

John Dalton

22
Q

Who, in 1897 concluded that atoms had electrons and what theory was this?

A

J J Thomson.
The theory was called ‘The plum pudding model’.
The plum pudding model showed an atom as a ball of positive charge with electrons stuck on it.

23
Q

Who in 1909 conducted the alpha particle scattering experiments and what did he conclude from this?

A

Rutherford.
He shot positively charged alpha particles and a thin sheet on gold expecting particles to pass straight through or be slightly deflected at most.
Most did go through but more than expected were deflected which led to the discovery if the nucleus which deflected alpha particles

24
Q

Who discovered that electrons orbit the nucleus in fixed shells?

A

Bohr

25
Q

Who discovered protons?

A

Rutherford

26
Q

Who discovered neutrons?

A

James chadwick

27
Q

In the early 1800s how were elements arranged in the periodic table?

A

By atomic mass

28
Q

How are elements in the periodic table arranged now?

A

Their physical and chemical properties.

Relative atomic mass

29
Q

What did Dmitri Mendeleev do?

A

In 1869 he left gaps and predicted new elements in the periodic table.
He mainly put elements in order of atomic mass but switched the order if the properties meant it should be changed.
He left gaps to make sure elements with similar properties stayed in the same groups. Also for undiscovered elements in which Mendeleev predicted their properties.

30
Q

What are features of columns in the periodic table?

A

Also known as groups.
They contain elements with similar properties.
Group number tells you how many electrons they have in their outer shell.

31
Q

What are features of metals in the periodic table?

A

Metals form positive ions when they react.
Towards bottom and left of periodic table.

The ones to the left dont have many electrons to remove and ones towards the bottom have electrons in their outer shell really far away from the nucleus. This makes it easy to react to form positive ions with a full outer shell.

32
Q

What are features of non-metals on the periodic table?

A

On far right and top of periodic table.
Dont generally form positive ions when they react.

Forming positive ions is difficult.
They are to the right of the periodic table so have a lot of electrons to remove to get a full outer shell or towards the top where outer electrons are close to the nucleus so feel a strong attraction. Its easier for them to gain electrons.

33
Q

What are physical properties of metals?

A

Theyre strong but malleable.
Good conducting heat and electricity
High boiling and melting points

34
Q

What are physical properties of non-metals?

A

Brittle
Not always solid at room temperature
Dont generally conducts electricity and have lower density.

35
Q

What are transition metals and its properties?

A

In the centre of periodic table.
Typical metals.

They can have more than one ion.
Often coloured so compounds that contain them are colourful.
Transition metal compounds often make good catalysts. Eg an iron catalyst is used in the Haber process.

36
Q

What are features and trends of group 1 elements?(Alkali metals)

A

All have 1 electron in outer shell so very reactive.
Soft and low density.

Trends as you go down:

Increasing reactivity
Lower melting and boiling points
Higher relative atomic mass

37
Q

What happens when group 1 metals react with water/chlorine/oxygen?

A

Water:

React vigorously when out in water to produce hydrogen gas and metal hydroxides

Chlorine:

React vigorously when heated in chlorine gas to form white metal hydroxide salts

Oxygen:

Forms metal oxides

38
Q

Whats the difference between group 1 metals and transition metals?

A

Group 1 metals are more reactive.

Group 1 metals are less dense, strong and hard than transition metals and have lower melting and boiling points. The exception to this is mercury which is liquid at room temperature.

39
Q

What are features and trends of group 2 elements?(The halogens)

A

Non-metals with coloured vapours.

Trends as you go down:

Less reactive
Higher melting and boiling points
Higher relative atomic mass

40
Q

What type of compounds to group 1 elements form

A

Ionic compounds

41
Q

What type of compounds do group 7 elements form?

A

Molecular compounds or ionic compounds with metals

42
Q

What happens when a halogen (group 7)reacts with another halogen salt?

A

The more reactive one displaces the other

43
Q

What are features and trends of group 0 elements?(Noble gases)

A 
Full outer shell
Very unreactive
Exist as monatomic gases (single atoms not bonded to each other)
Colourless gases at room temperature
Non flammable

Trends as you go down:

Boinling and

Josh Lee Chemistry (5 decks)

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