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Chemistry > Atomic structure and the periodic table > Flashcards

Atomic structure and the periodic table Flashcards

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1
Q

What are all substances made from?

A

Atoms

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2
Q

What do atoms contain?

A

Protons, Neutrons, Electrons

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3
Q

What is the raidus of an atom?

A

0.1 nanometers / 1x10^-10

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4
Q

What is in the middle of the atom?

A

Nucleus

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5
Q

What does the Nucleus contain?

A

Protons and Neutrons

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6
Q

What is the raidus of the nucleus?

A

1x10^-14

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7
Q

What charge does the nucleus have?

A

Positive because of the protons

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8
Q

What does the electron do?

A

Move around the nucleus in electron shells

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9
Q

What charge do electrons have?

A

Negative

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10
Q

What charge do protons have?

A

Positive

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11
Q

What charge do neutrons have?

A

Neutral

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12
Q

What is the relative mass of electrons ?

A

1/2000 (sometimes taken as 0)

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13
Q

What is the relative mass of Protons and Neutrons ?

A

Both 1

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14
Q

What charge do atoms have?

A

Atoms are neutral because they have the same number of protons as electrons.The charge of Electrons and protons are the same but opposite so they cancel out.

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15
Q

What charge does an ion have?

A

The number of protons doesn’t equal the number of electrons which means it has an overall charge.

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16
Q

What does a nuclear symbol of an atom tell you?

A

It tells you its atomic (proton)number and mass number

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17
Q

What does the atomic number tell you?

A

(Small number)Atomic number tells you how many protons there are

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18
Q

What does the mass number tell you?

A

(Big number)the total number of protons and neutrons in the atom

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19
Q

How do you find the amount of neutrons?

A

Subtract the atomic number from the mass number

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20
Q

What is an element?

A

An element is a substance made up of atoms that all have the same number of protons in their nucleus.

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21
Q

What are isotopes?

A

They are different forms of the same element,which have the same number of protons but a different number of neutrons.

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22
Q

What is the formula to work out the relative formula of an element?

A

Relative atomic mass =sum of (isotope abundance x isotope mass number) / sum of abundance of all the isotopes

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23
Q

How are compounds formed?

A

They are formed from two or more elements, which are each in fixed proportions throughout the compound and they’re held together by chemical bonds

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24
Q

What does making bonds involve?

A

It involves atoms giving away, taking or sharing electrons.(Only electrons are affected)

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25
Q

What is ionic bonding?

A

A compound formed from a metal and a non-metal consists of ions.The metal atoms lose electrons to form positive ions and the non-metal atoms gain electrons to form negative ions.The opposite charges of the ions means that they’re strongly attracted to each other.

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26
Q

What is covalent bonding?

A

A compound formed from non-metals consists of molecules. Each atom shares an electron with another atom

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27
Q

What is a formula?

A

compounds represented by symbols (like elements)(e.g CO)

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28
Q

What is on the left and right of a chemical equation?

A

Molecules on the left hand side of the equation are called reactants because they react with eachother

Molecules on the right hand side of the equation are called products because they’ve been produced from the reactant

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29
Q

What are mixtures?

A

A subtance made from mixing two or more different substances together but are not chemically bonded

30
Q

How can you seperate mixtures?

A

Mixtures can be either elements or compounds, they can be seperated out by physical methods such as filtration, crystalistation, simple distillation, fractional distillation and chromotography

31
Q

What are the properties of a mixture?

A

The propertiese of a mixture are the propertiese of the seperate parts.

32
Q

What is Filtration used for?

A

filtration is used if your product is an insolube solid that needs to be seperated from a liquid reaction mixture.It can also be used in purfication aswell, solid impurities in the reaction mixture can be seperated out.

33
Q

What are two ways you can seperate a solube salt from a solution?

A

Evporation and evaporation

34
Q

What does the plum pudding model show?

A

Shows the atom as a ball of positive charge with electrons stuck in it

35
Q

What did JJ thomsom conclude from his experiments?

A

That atoms weren’t solid spheres. His measurements of charge and mass showed that an atom must contain even smaller, negatively charged particles(electrons)

36
Q

What was Rutherford’s experiment?

A

They fired positively charged alpha particles at an extremely thin sheet of gold.

37
Q

What did Rutherford’s experiment show?

A

some particles were deflected more than expected and a small number were deflected backwards, so the plum pudding couldn’t be right.

38
Q

What was Rutherford conclusion from his experiment?

A

That theres a tiny, positively charged nucleus at the centre where most the mass is concentrated. And a cloud of negative electrons surround this nucleus so the atom is mainly empty space.

39
Q

What did Bohr’s Nuclear model suggest?

A

that all the electrons were contained in shells, he proposed that electrons orbit the nucleus in fixed shells that aren’t anywhere in between.

40
Q

What did Further experiments by Rutherford show?

A

that the nucleus can be divided into smaller particles, which each have the same charge as the hydrogen nucleus .These particles were named protons.

41
Q

How was the perodic table arranged in the early 1800s?

A

They were arranged by Atomic Mass

42
Q

How did Mendeleev arrange the periodic table and what did he do?

A

Mendeleev put the elements mainly in order of atomic mass but did switch that order if the peroperties meant it should be changed.He left gaps in the table to make sure that elements with similar properties stayed in the same groups.

43
Q

How is the modern periodic table arranged?

A

In order of atomic number

44
Q

What are in the colums ?

A

Elements with similar properties

45
Q

What are groups?

A

Depending on what group, it tells how many electrons are in the outer shell.

46
Q

What are periods?

A

each new peroid represents another full shell of electrons.

47
Q

What ions do metals form and where are they in the periodic table?

A

positive ions and they are towards the bottom and to the left.

48
Q

Where are non-metals located in the periodic table?

A

They are to the far right and top

49
Q

Why do atoms react?

A

They react to form a full outer shell, they do this by loosing gaining or sharing electrons.

50
Q

What are some properties of metal?

A

(All metals have metallic bonding which causes them to have similar basic physical properties )
They’re strong, but can be bent or hammered into different shapes
Good at conducting heat and electricity
High boiling and melting points

51
Q

Properties of non-metals?

A 
(dont have metallic bonding)
more brittle
aren't always solids at room-temp
low density
not good for conducting electricity
52
Q

What are transition metals?

A

They are in the centre of the peroidic table,they are typical metals

53
Q

Properties of transition metals

A

More than 1 ion
they are often coloured
they are good catalysts

54
Q

What are the alkali metals?

A

Lithium, sodium,potassium, rubidium, caesium and francium

55
Q

What do alkali metals have?

A

They have 1 electron on the outside so they are very reactive and gives them similar properties

56
Q

What are trends for the alkali metals as you go down group 1

A

Increasing reactivity
Lower melting and boiling points
Higher relative atomic mass

57
Q

What ions do group 1 metals form?

A

1+ ions

58
Q

What do group 1 metals react to form?

A

ionic compounds, white solids that dissolve in water to form colourless solutions

59
Q

What happens when group 1 metals react with water?

A

They react vigorously to produce hydrogen gas and metal hydroxides-salts that dissolve in water to produce alkaline solutions
More reactive lower down in the group

60
Q

What happens when group 1 metals react with chlorine?

A

React vigorously when heated in chlorine gas to form white metal chloride salts
More reactive lower down in the group

61
Q

What happens when group 1 metals react with oxygen?

A

They form metal oxide(different types of oxide with form depending on the group 1 metal)
Lithium reacts to form lithium oxide
Sodium reacts to form a mixture of sodium oxide and soidum peroxide
Potassium reacts to form potassium peroxide and potassium superoxide

62
Q

What are group 7 elements?

A

Halogens , non-metals with coloured vapours

63
Q

What happens as you go down group 7?

A

Become less reactive- harder to gain electrons because further away from nucleus
higher melting and boiling point
higher relative atomic mass

64
Q

How do halogens get a full outer shell?

A

They share electrons via covalent bonding

65
Q

What ions do halogens form?

A

1- ions called halides

66
Q

Can a more reactive halogen displace a less reactive one?

A

yes a displacement reaction can occur between a more reactive halogen and the salt of a less reactive one

67
Q

What are group 0 elements?

A

Noble gasses, they have eight electrons in their outer shell apart from helium which has 2. As is it generally stable they dont need to give up or gain an electron to become more stable.(they dont react much[inert])

68
Q

What do group 0 elements exist as?

A

monatomic gases - single atoms not bonded to each other

69
Q

Properties of noble gasses

A

colourless at room temp
non-flammable because inert
boiling point increase the lower in the group

70
Q

Why does the boiling point of noble gasses increase lower in the group?

A

There is an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome.

Chemistry (10 decks)

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