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chemistry > c1 atomic structure and the periodic table > Flashcards

c1 atomic structure and the periodic table Flashcards

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1
Q

define atom

A

the smallest part of an element that can exist

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2
Q

what are the groups on the periodic table

A

vertical, 1-7 then 0

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3
Q

what are periods on the periodic table

A

horizontal

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4
Q

why is a chemical formula used

A

to represent and element or compound in balanced chemical equations

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5
Q

which elements exist as molecules made up of two of the same atoms joined together

A

iodine, bromine, chlorine, fluorine, oxygen, nitrogen, hydrogen

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6
Q

how do you remember the elements that are written as (element)2

A

I Bring Clay For Our New House

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7
Q

define compound

A

a substance that contains two or more elements that are chemically combined in fixed proportions

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8
Q

what does it mean if the second word of a compounds name starts with mon, di or tri

A

its made up of non metals only, and shows how many there are of that element for every one atom of the first element. e. g carbon dioxide, one carbon to two oxygen (C02)

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9
Q

what is an ion

A

and charged particle formed when an atom or a group of atoms loses or gains an electron

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10
Q

How do you predict the formula of an ionic compound?

A

using the formula of its ions. The number of ions in a formula must give an equal number of positive and negative charges.

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11
Q

what is a word equation?

A

A chemical reaction that uses the names of the substances instead of the specific substance itself

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12
Q

what is a reactant?

A

The substances that react together in a chemical reaction

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13
Q

What is a balanced chemical equation

A

A chemical reaction that uses the formula of the reactants and products, and shows the number of units of the substance

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14
Q

what is an aqueous solution

A

forms when a substance dissolves in water

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15
Q

What is the law of conservation of mass?

A

No atoms are lost or major chemical reaction, so the total mass of the product is equal to the total mass of the reactants

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16
Q

What is a plum pudding model?

A

A ball of positive charge with negative electrons studded into it

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17
Q

why did Mendeleev put some elements in groups?

A

Because they had similar chemical properties for example, they react violently with water

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18
Q

Why did Mendeleev leave gaps in his periodic table?

A

four elements that had not been discovered yet

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19
Q

what is the relative atomic masses of the subatomic particles

A

protons and neutrons: 1
electrons: 0

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20
Q

what are the charges of the subatomic particles

A

protons: positive
neutrons: neutral
electrons: negative

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21
Q

what is an isotope

A

different forms of the same element the have the same number of protons but a different number of neutrons

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22
Q

what does abundance mean

A

how common or rare that isotope is

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23
Q

what is the equation for relative atomic mass

A

sum of (isotope abundance x isotope mass)
————————
sum of abundances of all the isotopes

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24
Q

define molecule

A

2 or more atoms held together by chemical bonds

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25
Q

how do you find percentage mass of an element

A

mass of element
————————- x 100
total mass of compound

26
Q

Define pure

A

A substance that consists of only one element or one compound or a mixture that consists of two or more substances, not chemically joined together

27
Q

How do you separate a mixture?

A

A physical process.

I don’t need to involve chemical reactions and no new substances are made

28
Q

when is filtration used?

A

Two. Separate an insoluble solid from a liquid, for example, sand and water.

29
Q

what is crystallisation?

A

a process To produce solid crystals from a solution.

When is solution is room to some of this open evaporates leaving crystals behind

30
Q

When would you use simple distillation?

A

To separate a solvent from a solution, for example, pure water from seawater

31
Q

what is fractional distillation?

A

 A process used to separate different liquids for a mixture of liquids, for example, ethanol from a mixture of ethanol and water

32
Q

What is paper chromatography?

A

A process used to separate mixtures of soluble substances

33
Q

how does chromatography work

A

The different dissolved substances in the mixture are attracted to the two phases in different proportions. This causes them to move at different routes through the paper. 

34
Q

what are the two phases in chromatography?

A

The stationary phase and the mobile phase

35
Q

how can you tell if two substances are the same on a paper chromatogram

A

they produce the same number of spots which match on colour. And the spots travel the same distance up the paper.

36
Q

whose ideas about atoms were published in 1803 and what were they?

A

John Dalton thought that all matter was made a tiny particles called atoms, which he imagined as tiny spheres that couldnt be divided

37
Q

Who suggested the plum pudding model and what is it?

A

JJ Thompson. He suggested that an atom is a ball of positive charge with negative electrons studded into it.

38
Q

Who designed an experiment to test the plum pudding model and what was it?

A

Ernest Rutherford .

In the experiment positively charged alpha particles were fired at Sid gold foil. Most of the particles went through the foil, but a few were scattered in different directions. this showed that the gold atoms were mostly empty Space 

39
Q

What did Ernest create?

A

A new model called the nuclear model.
the mass of an atom is concentrated at its centre, the nucleus.
And the nuclues positively charged

40
Q

Who adapted Ernest Rutherfords nuclear model?

A

niels bohr

41
Q

what did Niels discover?

A

That electrons orbit the nucleus in shells which were at certain distances from the nucleus. He also discovered that the nucleus contain small particles called protons, which each had a small amount of positive charge.

42
Q

Who discovered neutrons?

A

James Chadwick

43
Q

how do you calculate the relative atomic mass?

A

Total mass of atoms/total number of atoms

44
Q

What are periods arranged in?

A

In order of increasing atomic number

45
Q

what are groups arranged in?

A

Elements with similar properties

46
Q

how are the chemical properties of compound of metal and nonmetals elements different?

A

most metal oxides are basic, and most non-metal oxides are acidic

47
Q

what are the differences in metal and nonmetal physical properties?

A

Most metals have high, melting and boiling points, whereas most nonmetals have a low, melting and boiling points

48
Q

properties of metal

A

Good conductor of electricity and heat, shiny, high-density, malleable, ductile

49
Q

properties of nonmetals when solid

A

Poor conductor of electricity and heat, doll, low-density, brittle

50
Q

What are elements in group 0 called

A

Noble gases

51
Q

Which element has the lowest boiling point

A

Hydrogen

52
Q

How did the elements change as you go down group 0

A

Atoms become larger, intermolecular forces between atoms become stronger, more energy is needed to overcome the forces

53
Q

what are group 1 elements called?

A

Alkali metals

54
Q

Properties of alkali metals

A

soft, relatively low melting, points, and low density

55
Q

What is the equation for when alkali metals react with water?

A

Metal plus water –> metal hydroxide plus hydrogen

56
Q

what happens to elements as they go down group one?

A

Atoms become larger, how to electron becomes further from the nucleus, the force of attraction between the nucleus, and the outer electron decreases, and the outer electron is lost more easily

57
Q

What is group 7 called

A

Halogens

58
Q

What happened to elements as you go down group 7

A

molecules become larger, intermolecular forces become stronger, what energy is needed to overcome these forces

59
Q

What are halogens?

A

Simple molecules, pair of non metals, joined by a single covalent bond

60
Q

What happens when halogens react with metals?

A

They produce salts

61
Q

What happens to the reactivity of elements down group 7

A

It decreases

62
Q

What happened to elements as you go down group 7

A

outer shell gets further away
less reactive as it is harder to gain an electron when outer shell is far
higher m&b points
higher ar

chemistry (3 decks)

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