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GCSE Chem > Atomic Structure And Periodic Table > Flashcards

Atomic Structure And Periodic Table Flashcards

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1
Q

What are atoms

A

They are subatomic particles (protons,neutron and electron)

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2
Q

What is an atoms diameter

A

(1x10^_10 metres)

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3
Q

What is the size of a nucleus in relative to the atom

A

1/10000

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4
Q

Relative charge and relative mass of each subatomic particle

A

Proton: charge+1 - mass 1

Neutron: charge 0 - mass 1

Electron: chareg -1 - 0

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5
Q

Why do atoms have no electrical charge

A

Number of protons equal to number of electrons

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6
Q

How to find mass number of an element

A

Number of protons + neutrons

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7
Q

How to find atomic number of an element

A

Number of protons or electrons

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8
Q

How to electrons orbit the nucleus and give the formation

A

Orbit shells in fixed distances from the nucleus

First shell is 2 with every subsequent electron shell having a max number of 8

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9
Q

What are atoms with incomplete outer shells and what happens during a reaction

A

They become unstabled and when they react they gain a complete outer electron shell

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10
Q

Explain the early concepts of atomic theory

What they are?
When?
Founder?

A

Small,indivisible,spherical atoms

19th century

John Dalton

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11
Q

Explain the plum pudding model

What is it?
When?
Founder?

A

Solid proton sphere with electrons embedded inside it

1904

JJ Thomson

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12
Q

Explain the nuclear model

What is it?

Date?

Founder?

A

Tiny, dense indivisible positive nucleus, surrounded by negative electrons

1911

Ernest Rutherford

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13
Q

What is the orbital model?

Date?

Founder?

A

Tiny,dense, indivisible positive nucleus, orbited by electrons in fixed shells

1913

Niel Bohr

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14
Q

What is the modern atomic structure

What is it?

Date?

Founder?

A

Tiny central nucleus (made of protons and neutrons) orbited by very tiny negative electrons

1926

John Dalton

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15
Q

Explain the alpha particle scattering experiment

Theory

A

Alpha partciles (positively charged- large mass) should pass straight through the gold foil and be detected other side.

This is due to weak, positive,solid atoms in the Plum pudding model have neither a sufficient density to resist the radiation or a strong positive charge to deflect it

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16
Q

Explain the alpha particle scattering experiment

What happened during the experiment

A

Positive alpha particles shot at the gold foil

Radiation did not pass through the gold foil but was significantly deflected and some were reflected to the radiaoactive material

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17
Q

What did Rutherford conduct from the experiment

A

1) Alpha particle passes striaght through the foil without colliding into anything (reflected/deflected). This indicates there is lots of empty space in the atom (mostly)

2) Alpha radiation is deflected through the foil. This shows that the positively charged alpha particles are being repelled by another positive charge. This shows that the atom must have a tiny central nucleus that has a strong posiitve charge.

3) Alpha particles is reflected back to the source. The relatively heavy alpha radiation bounces back of the nucleus. This shows that the nucleus must be very dense.

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18
Q

What is an isotope

A

Atoms of the same element with the same amount of protons but different number of neutrons

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19
Q

How to calculate relative atomic mass

A

Relative atomic mass= (% isotope 1 x Mass isotope 1) + (%isotope 2 x Mass isotope 2)
________________________________________________________________
Sum of all isotope abundance

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20
Q

What are the starting chemicals called

A

Reactants

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21
Q

What is the name of chemical that are made in a reaction

A

Products

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22
Q

What happens to the atoms during a chemical reaction

A

Reactants bond are broken and new chemical bonds made to form the products. Atoms are unchanged , only bonding changes.

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23
Q

What is the conservation of mass

A

Mass of reactants is equal to mass of the products due to mass of the atoms remaining ucnhanged in a chemical reaction

24
Q

What is an elemental compound

A

A molecule of the same element chemically bonded together

25
Q

What is a compound

A

Two or more elements chemically bonded together.

26
Q

What is a symbol equation

A

Number of atoms of each element involved. Symbol equations must be balanced so that the number of atoms of each element is the same before and after the chemical reaction.

27
Q

What is a mixture

A

A mixture contains two or more substances not chemically joined and relatively easy to seperate

28
Q

What is a solution

A

A mixture of a liquid (solvent) and one or more dissolved solids (solutes)

29
Q

What is a solvent

A

A liquid that dissolves a certain solute to make a solution

30
Q

What is a solute

A

A solid that can be dissolved in solvent to make a solution

31
Q

What is soluble and insoluble

A

Soluble-can be dissolved in a given solvent

Insoluble-can not be dissolved in a given solution

32
Q

What seperation technique is bested used for:

seperating liquid and insoluble solids

Liquid and soluble

Liquid-liquid mixtures

A

Filtration

Evaporation,crystallization

Fractional distillation

33
Q

Equipment used in filtration and how the experiment is conducted

A

Insoluble solid, filter paper,filter funnel,conical flask and liquid solvent

Filter paper is folded into a cone and is inserted in the neck of the fliter funnel. Placed inside a conical flask and the mixture is poured into the filter funnel.

The filter paper allows liquid to pass through however it prevent solids from passing through.

Insoluble solids called residue is seperated from the filtered liquid (filtrate)

34
Q

Equipment used in distillation and how the experiment is conducted

A

Solution,heat (bunsen burner) ,rounded bottom flask, cork,condenser,flask

It is sued to seperate solvent from a solution.

Solution is poured into a rounded-bottomed flask connected to a condenser. The solution is heated causing the liquid solvent to boil and evaporate.

The gas passes through the condenser, is cooled and condense back into liquid (distillate) collected by the flask.

The solid solute remains as residue on the inside of the round-bottomed flask

35
Q

Equipment used in evaporation and how the experiment is conducted

A

Water,salt crystals,bunsen burner,evaporating basin,tripod

Seperates solute from a solution

Solution is poured into the evaporating basin and heated. The solvent evaporates solution becomes more concentrated. Do this until all that is left are dry crystals

36
Q

Equipment used in crystallisation and how its conducted

A

Water,heat,tripod,salt crystals,flask,funnel,filter paper

Used to seperate out solute from a solution

Solution poured into an evaporating basin and gently heated , causing liquid solvent to evaporate, until crystals start to form.

The evaporating dish is cooled, encouraging crystals to form in the residual solution.

Once cooled any remaining solution can be removed by filtration and crystals are patted dry.

37
Q

Equipment in fractional distillation and how it is conducted

A

Solution,bunsen burner,thermometer,cork,condenser,flask, rounded bottom flask,beakers

Fractional distillation used to seperate mixture of two or more liquids

Mixture of liquid poured into rounded bottom and connected to condenser. The mixture is heated using a busnen burner and the temperature must reach a point to equal the lowest boiling point of the mixture using the thermometer

The liquid turns into a gas in the condenser and turns back into a liquid. The liquid boils until it can’t anymore and is collected by the flask.

Once all the fraction is collected the temperature is raised until it reaches the lowest boiling point for the second fraction and a different beaker is used to collect the liquid.

This is repeated until all liquids in the mixture is seperated using boiling point

38
Q

What is chromatography

A

Used to seperate mixtures according to solubility of the components.

It makes use of the attraction of a substance to a stationary phase and to a solvent to seperate mixtures along a chromatography medium.

39
Q

How was the periodic table organised in the 1800

A

Organised on atomic weight.

40
Q

Why was the early periodic table bad

A

The chemical properties of the elements were imperfect when ordered by atomic weight.
It lead togroupings to be dissimilar.

Didn’t take into account properties

41
Q

How did Dmitri Mendeleev categorise the periodic table

A

Ordered elements primarily by increasing atomic wieght. However, also ordered elements so that chemically similar properties of elements were in the same group.

He also left gaps to accomodate new elements and predicted future properties of elements based on gaps.

42
Q

How is the modern periodic table categorised

A

Organises elements by increasing atomic/proton number. Every 8 elements have similar chemical properties.

8 columns called groups . Each group has similar chemical properties due to same number of electron in outermosts shell

Rows in the periodic table are called rows. Each period collects elements with the same number of electron shells

43
Q

Properties of metals

A

Shiny,hard,malleable,dense,good electrical and thermal conductors.

Gains a full outer shell by losing electrons

44
Q

Properties of non metals

A

Dull,non-conductive,brittle,less dense, gas/liquid at room temp.

Gain a full outer shell by gaining or sharing electrons

45
Q

Properties of transition metals

A

Has general properties of metals, but have useful additional properties such as can form coloured compounds in chemical reactions.

Act as a catalyst

Lose different number of electrons in different chemical reactions

46
Q

Group 1 reaction trends

A

Increases in reactivity as you go down

Low melting and boiling point

High relative atomic mass

React with water to produce metal hydroxide solutions (Alkali Metal+Water→Metal Hydroxide+Hydrogen)

React with acids to produce salts and hydrogen gas.( Alkali Metal+Acid→Salt+Hydrogen)

React with oxygen to produce metal oxides
(Alkali Metal+Oxygen→Metal Oxide)

React with halogens to produce salts
(Alkali Metal+Halogen→Salt)

47
Q

Direction of reactivity down group 1

A

Increases in reactivity as it goes down

48
Q

Lithium , sodium and pottasium reaction with water

A

Lithium: mild fizzing whilst reacting and dissolves to form lithium hydroxide solution

Sodium: reacts more vigorously. It will move around more and melt into a ball. Greater fizzing

Pottasium: More vigorous. It will melt into a ball rapidly. Pottasium will burn with a lilac flame with a great effeverscence

49
Q

Group 7 reaction trends

A

As you go down the elements are less recative

Higher melting/boiling points

Higher relative atomic mass

React with alkali to form salts
(Halogen+Alkali Metal→salt)

Halogen can displace another in a compound
(Halogen+Compound→Compound+(Displaced) Halogen)

50
Q

What direction does reactivity go when it goes down group 7 and why

A

Reactivity decreases down group 7. Chlorine reacts less vigorously with sodium then fluorine.

Group 7 elements have 7 outer shell electrons . In a chemical reaction they gain an additional electron to gain a full shell. The more shells there are the harder it is for it to gain an electron. This is due to the shell acting as a shield to negate the pull from the positive nucleus.

51
Q

Similar physical trends in halogens

A

Low density, melting point and boiling point

52
Q

Trend in physical properties of halogens

A

Down the group relative atomic mass increases and melting/boiling point.:

At room temperature, Fluorine is a toxic yellow gas.

At room temperature, Chlorine is a toxic, dense green gas.

At room temperature, Bromine is a dense red-brown liquid.

At room temperature, Iodine is a dark grey solid

53
Q

Similar properties of noble gases

A

Low densities, low melting/ boiling points

54
Q

Trend going down the noble gases

A

Increasing relative atomic mass and increasing melting/boiling point

55
Q

Why are noble gases unreactive

A

They exists as single atoms and don’t bond with other atoms due to their full outer electron shell, therefore they do not lose or gain an electron in a reaction

56
Q

Equipment in chromatograohy and how it is conducted:

A

Equipment: Filter paper, pencil,capillary tube, ink,beaker, lid

1) Draw a line near the bottom of the filter paper

2) Add a spot of ink onto the line (place filter paper inside beaker of water)

3) Make sure ink isn’t touching solvent but water comes into contact with paper

4) Place lid to stop evaporation

5) Wait until water seperates the ink

6) Wait until ink has nearly reached the top or has stopped

7) pattern of the spots is the result (chromatogram)

57
Q

Order of subatomic particles found

A

Electron, proton and neutron

GCSE Chem (11 decks)

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