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Chemistry > Atomic Structure and Periodic Table > Flashcards

Atomic Structure and Periodic Table Flashcards

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1
Q

What does the atom consist of

A

Protons
Neutrons
Electrons

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2
Q

What is atomic number

A

Number of protons

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3
Q

Mass Number

A

Number of protons AND Neutrons

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4
Q

What is an element

A

A group of atoms with the same atomic number

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5
Q

What is an istotope

A

An element with the same amount of protons and electrons, but a different amount of neutrons

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6
Q

What is Relative atomic mass

A

Average mass taking into account the different masses and abundances of all the isotopes that make up the element

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7
Q

How do you calculate the relative atomic mass

A

(Abundance X Atomic number) +(Abundance X Atomic number)
/Sum of abundances of all isotopes

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8
Q

Elements react to form

A

Compounds

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9
Q

Compound

A

Substances of two or more elements, the atoms of each are in fixed proportions and held together by chemical bonds

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10
Q

Mixtures

A

A collection of elements or compounds that are not chemically bonded together

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11
Q

Methods to seperate mixtures (3)

A
  • Chromatography
  • Filtration and Crustallisation
    -Distillation
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12
Q

How do you perform chromatography

A
  • Draw a line in pencil and a pen dot on filter paper above the water level
  • Place a lid so it doesnt evaporate
  • Each different dye in the ink will move up the paper at different rates
  • When it’s done take it out and leave it to dry
    -End result is a chromatogram
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13
Q

What is filtration

A

Seperating insoluble solids from liquids

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14
Q

How to perform filtration

A
  • Roll up filter paper
  • Place in a funnel over a beaker
  • Pour solution with insoluble solid in and wait
    -Solution should pass through filter paper and be pure
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15
Q

Two ways of seperating soluble solids from solutions

A

Evaporation, Crystallisation

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16
Q

Describe process of evaporation

A

-Pour solution into evaporating dish
- Slowly heat the solution. The solvent will evaporate and the solution will get more concentrated. Eventually crystals will start to form.
- Keep heating until you only have dry crystals

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17
Q

Describe the process of crystallisation

A
  • Pour the solution into an evaporating dish
  • Heat for a bit
  • When you see crystals, remove from heat and leave to cool
  • Filter the crystals out of the colution and leave in a warm place to dry.
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18
Q

How can you use filtration and crystallistaion to seperate rock salt

A

1- Grind the rock salt to ensure the salt crystals are as small as possibkle and can dissolve easily
2- Place the salt in water and stir until the salt dissolved
3- Filter the solution
4- Evaporate the water from the salt so that it forms dry crystals

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19
Q

What is simple distillation

A

The process of seperating out two solutions

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20
Q

Explain the process of simple distillation and two liquids it can seperate

A

Seperating pure water and sea water
-Solution is heated to the lowest boiling point of the two solutions
- The vapour condenses and is collected in a beaker whilst the rest of the solution is left behind

21
Q

When do you use fractional distillation

A

To seperate a mixture of three or more liquids

22
Q

How do you carry out fractional distillation

A
  • Put your mixture in a flask and put a fractionating column ontop
  • Heat the flask and the liquid with the lowest boiling point will evaporate first. It will evaporate, rise up, go through a condenser and then is collected in a test tube
23
Q

What was Thompson’s theory of the atom

A

Plum pudding model- Atom’s weren’t solid spheres but positive balls with negative electrons

24
Q

What was Rutherford’s theory of the atom

A

After the gold foil experiment he knew there was a dense positively charged nucleus in the middle with electrons in a ‘cloud ‘outside it.

25
Q

What was Bohr’s theory of the atom

A

The elctrons orbited the nucleus in fixed energy shells

26
Q

What was Chadwick’s theory of the atom

A

He discovered neutrons were in the nucleus which then became the nucleur model

27
Q

What was Dalton’s theory of the atom

A

They were just solid spheres

28
Q

What are the electron shell rules

A
  • Lowest energy shells are alwaays filled first
  • Only 2 electrons allowed in first shell
  • Only 8 electrons allowed in second and third shell
    -Atoms want full energy shells to be ✨happy✨
29
Q

How were periodic tables arranged before mendeleev

A

-Physical appearnace
-Atomic weight

30
Q

Disadvantages of periodic table before mendeleev

A

Some elements were in the wrong group because elements were put in order of atomic weight

31
Q

What did Mendeleev’s periodic table have

A
  • Put the Elements in order of atomic weight but switched some around to account for properties
  • Left gaps for new elements that hadn’t been discovered so that elements with similar properties could be in the same group
32
Q

Why and how do atoms react

A

To form full outer shells, by gaining or losing electrons

33
Q

How do non metals react

A

They often gain electrons, forming negative ions, as they have to gain less electrons than lose

34
Q

How do metals react

A

They often lose electrons to form positive ions as they have to lose less electrons than gain

35
Q

Where can transition metals be found in the periopdic table

A

Between group 2 and 3

36
Q

Properties of transition metals (6- 3 long 3 short)

A
  • Strong
  • Dense
  • Shiny
  • Different coloured compounds
  • Can have different charges (more than 1 ion)
  • Can be used as catalysts
37
Q

Properties of group 1 metals (3)

A
  • One electron in the outer shell
  • Soft
  • Low density
38
Q

Trends of alkali metals as you go down the group (3)

A
  • Increasing reactivity
  • Lower melting points
  • Higher RAM
39
Q

Group 1 metals often form an outer shell by… making them have a charge of…

A

Losing one electron
1+

40
Q

Group 1 metal reaction with water

A

Metal + Water –> Metal hydroxide + Hydrogen

41
Q

Group 1 metal reaction with chlorine

A

Metal + Chlorine –> Metal chloride

42
Q

Why do group 1 metals tarnish in the air

A

The metal reacts with oxygen to form a dull oxide layer

43
Q

Group 1 metal reaction with oxygen

A

Metal + Oxygen –> Metal Oxide

44
Q

Group 1 Vs Transition metal (4)

A
  • Group 1 metals are more reactive
  • Group 1 reacts more vigorously with water and oxygen
  • Transition metals are more dense hard and strong
  • Transition metals have higher melting points
45
Q

Colours and states of halogens:
- Fluorine
- Chlorine
- Bromine
- Iodine

A

Fluorine- yellow gas
Chlorine- dense green gas
Bromine- Red volatile liquid
Iodine- Purple vapour

46
Q

Trends of halogens going down the group (3)

A

-Less reactive
- Higher melting and boiling point
- Higher RAMs

47
Q

Properties of group 0 (3)

A
  • Inert, colourless gases
  • Exist as monoatomic gases
  • Non flamable
48
Q

Trends of group 0 going down the group (2)

A
  • Boiling point increases because increased number of electrons so theres greater intermolecular forces between them

Chemistry (10 decks)

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