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Chemistry > Atomic structures > Flashcards

Atomic structures Flashcards

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1
Q

What is a mixture?

A

When two or more elements or compounds are mixed together but aren’t chemically bonded

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2
Q

What is an element?

A

A pure substance made up of only one type of atom

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3
Q

What is a compound?

A

A substance that is made up of two or more atoms which are chemically bonded together

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4
Q

What does soluble means?

A

When something can dissolve

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5
Q

What does insoluble mean?

A

When something is unable to dissolve

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6
Q

Name the subatomic particles

A

Electron
Proton
Neutron

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7
Q

What does the mass tell us?

A

Protons+ neutrons

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8
Q

What does the atomic number tell us?

A

Protons which is the same as electrons

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9
Q

What is periodic table arranged in?

A

Atomic number (protons)

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10
Q

What is an isotope?

A

A version of the same element but with a different number of neutrons

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11
Q

What is the relative mass of a proton?

A

1

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12
Q

What is the relative mass of a electron?

A

Very small

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13
Q

What is the relative mass of a neutron?

A

1

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14
Q

What is the electric charge of a proton?

A

+1

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15
Q

What is the electric charge of a electron?

A

-1

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16
Q

What is the electric charge of a neutron?

A

0

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17
Q

When did Mendeleev organise the periodic table?

A

1869

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18
Q

What did Mendeleev organise the periodic table according to?

A

To the element’s atomic mass

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19
Q

How did Mendeleev group the elements?

A

Corresponding to their chemical properties

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20
Q

Why did Mendeleev place the alkaline metals in one group together?

A

Because they had similar properties

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21
Q

Why are transition metals placed between groups 2 and 3?

A

Because they have a similar number of electrons in their third shell

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22
Q

Why did Mendeleev leave gaps?

A

For missing elements

23
Q

How created the table we use today?

A

Henry Mosely

24
Q

When did Henry Mosely produce the table we use today?

A

1914

25
Q

How did Mosely organise the elements?

A

According to their atomic number

26
Q

What did Mosely add to the table?

A

The noble gases

27
Q

Who first organised the periodic table according to their atomic mass?

A

John Newland

28
Q

When was the electron discovered and who by?

A

J.J Thompson and in 1897

29
Q

What did J.J Thompson create?

A

The plum pudding model- he imagined the atom was positively charged with electrons stuck in it

30
Q

Who tested J.J Thompson’s theory and when?

A

1991 Rutherford

31
Q

How did Rutherford test Thompson’s theory?

A

He fired particles at atoms however some bounced off funny not centred

32
Q

When was the proton and neutron discovered and by who?

A

By Chadwick in 1932

33
Q

What reaction would take place with the hot tungsten was surrounded by air?

A

It would react with oxygen and burn out

34
Q

What is Rn used for?

A

Radiotherapy

35
Q

What is Kr and Xe used for?

A

Lasers

36
Q

What are metals?

A

They losers because they want to react to achieve a full outer shell so they have to give away their electrons

37
Q

Name some properties of a metal

A

Good conductor of heat and electricity
High density
Strong
solid

38
Q

Name some properties of a non metal

A

Poor conductor of heat and electricity
Low density
Soft
Solid, liquid or gas

39
Q

What elements are the halogens?

A

Chlorine, fluorine, bromine, iodine and astatine

40
Q

What metals do the halogens react with ?

A

Alkali metals to form halide ions with a charge of -1

41
Q

What happens when you go down group 7?

A

The reactivity decreases

42
Q

Why does the reactivity of group 7 decrease as you go down?

A

As you go down the group you gain shells and for non metals to react they need to gain electrons. So it is harder to gain electrons because it is further away from the nucleus

43
Q

What happens when you go down group 1?

A

The reactivity increases

44
Q

Why does the reactivity of group 1 increase as you go down?

A

Because for metals to gain a full outer shell they lose electrons so when you go down the group the number of shells increase so the nucleus attraction is weaker. So it is easier to lose electrons

45
Q

What are the key properties of the alkali metals?

A

Low density
Soft
Float

46
Q

What do alkali metals react with?

A

Oxygen and hydrogen to form a hydroxide

47
Q

What is displacement?

A

When a more reactive metal displaces a less reactive metal

48
Q

What is oxidation?

A

Loss of electrons

49
Q

What is reduction?

A

Gain of electrons

50
Q

Acid + metal equals

A

Soluble salt + hydrogen

51
Q

What type of ion does all acids contain?

A

Hydrogen ions

52
Q

What happens when acids are dissolved in water?

A

They fully ionise to release H+ ions into a solution, making it strong

53
Q

Insoluble base (oxide) + acid equals

A

Soluble salt + water

54
Q

Insoluble salt (carbonate) + acid equals

A

Soluble salt + water + carbon dioxide

Chemistry (11 decks)

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