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CHEMSITRY > CHAPTER 1 > Flashcards

CHAPTER 1 Flashcards

1
Q

What is an element?

A

Made of one type of atom

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2
Q

What is a compound?

A

Substance made of different types of atoms bonded together

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3
Q

Differences between compounds and mixtures

A

Mixtures aren’t chemically combined

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4
Q

What is filtration

A

Separate insoluble substances from a solution

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5
Q

What is crystallisation

A

Evaporate water from solution to leave crystals

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6
Q

What is fractional distillation

A

When liquid are separated because of their boiling points

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7
Q

What did JJ Thompson discover

A

Electron

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8
Q

What is an ion

A

Atoms with different numbers of electrons

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9
Q

What is an isotope

A

Different number of electrons

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10
Q

What is an atom

A

The smallest part of an element

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11
Q

What do the symbols in the periodic table represent

A

Atoms

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12
Q

What is a compound

A

Different types of atoms bonded together

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13
Q

What is the law of conservation of mass

A

The total mass of products formed = mass of reactants

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14
Q

What holds a compound together

A

Chemical bonds

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15
Q

Is hydrogen a metal or non metal

A

Hydrogen is a metal. A metal must conduct heat and electricity which solid hydrogen does. The properties of metals like malleability are just coincidence

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16
Q

With open containers, why does it sometimes look like the law of conservation is broke

A

With gases, the carbon dioxide formed will escape or oxygen will enter. When gas escapes, the law is kept because oxygen will react with the metal to keep the same weight the same

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17
Q

What is an element determined by

A

Number of protons

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18
Q

When you change the number of neutrons, you get an

A

isotope

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19
Q

When you change the number of electrons you get an

A

Ion

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20
Q

How to separate elements in a compound

A

Chemical reaction

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21
Q

What does filtration separate

A

One solute that is soluble in a solvent and one isn’t

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22
Q

How does crystallisation work

A

Filter the substances, then evaporate the liquid to leave the material

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23
Q

When should heating be stopped during crystallisation

A

When the solution is just forming crystals

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24
Q

What are elements ordered by in a stable

A

Smaller number - atomic number

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25
Q

How to calculate the relative atomic mass using isotopes

A

Multiple percentage by mass, add and then divide by 100

26
Q

What are the columns in the periodic table called

A

Groups

27
Q

What does the symbol of an element show

A

One atom of the element

28
Q

What do chemical equations show

A

The reactants and the products

29
Q

What happens in a chemical reaction

A

The atoms in the reactants get rearranged into the products

30
Q

What is an aqueous solution

A

A substance that has been dissolved in water

31
Q

Process of filtration

A

Pour the mixture through a filter funnel

32
Q

Process of evaporation

A

Heat the solution with a Bunsen burner

Keep heating until all the liquid has gone and you are left with dry crystals

33
Q

Process of crystallisation

A

Gently heat the solution
once some of the liquid has evaporated, stop heating
Leave the solution to cool
Now more crystals will form
Filter out the crystals out and then you’re done

34
Q

Process of chromatography

A

Draw a pencil line of the paper
Place blobs of your in
Place the paper in water so the ink isn’t touching the solution
The solvent will move up the paper and carry the ink

35
Q

When to use simple distillation

A

When you want to separate a liquid from a solution

36
Q

Process of simple distillation

A

The solution is heated to evaporate the part of it with the lowest boiling point first
This vapour is cooled, condensed and collected

37
Q

When to use fractional distillation

A

When you have a mixture of liquids with similar boiling points

38
Q

Process of fractional distillation

A

You heat the mixture until it reaches the boiling point of the first liquid
This liquid evaporates first
It reaches the top of the column, runs down the tubs and is collected
You repeat this with higher temperatures

39
Q

What did John Dalton suggest

A

Atoms were tiny hard spheres

40
Q

Who discovered the electron

A

JJ Thompson

41
Q

Who discovered and the nucleus and how

A

Geiger and Marsden fired atoms at gold foil and some rebounded

42
Q

who discovered that electrons were in shells

A

Niels Bohr

43
Q

Who found there were neutrons in the nucleus?

A

James Chadwick

44
Q

Charge of a proton

A

+1

45
Q

Mass of proton

A

+1

46
Q

Charge of neutron

A

0

47
Q

Mass of neutron

A

1

48
Q

Charge of electron

A

-1

49
Q

Mass of electron

A

very small

50
Q

What is the mass number

A

The mass of nucleus

51
Q

What is the atomic number

A

The number of electrons or protons

52
Q

When an atom gains electrons what is the charge on the ion

A

-

53
Q

When an atom loses electrons what is the charge on the ion

A

+

54
Q

Why will isotopes of the same element have the same chemical properties

A

Their chemical properties depend on their electronic structure

55
Q

How to write the electronic structure

A

Number of electrons in first shell, followed by second and third

56
Q

What determines how an element reacts

A

Electrons in outer shell

57
Q

What experiment did JJ Thompson do and how did this lead to him finding the electron

A

He found that the mysterious particle was attracted to a positive charge, showing they must be negatively charged

58
Q

What was Bohrs experiment

A

he noticed light was given out when electron were heated - they were moving between energy levels

59
Q

Why is it impossible to predict the mass of crystals that can be obtained during crystallisation

A

Mixtures have no fixed composition

60
Q

What was Geiger and Marsden’s experiment

A

They fired alpha particles at gold foil
Due to the current model of the atoms which was the plum pudding one, they expected most of the particles to pass straight through. The positive alpha particles pass straight through. The positive alpha particles were detected by the negative electrons

CHEMSITRY (13 decks)

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