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A Level Chemistry > Chapter 2 - Atoms, ions and compounds (MODULE 2) > Flashcards

Chapter 2 - Atoms, ions and compounds (MODULE 2) Flashcards

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1
Q

What two subatomic particles are located in the nucleus

A

protons and neutrons

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2
Q

Where do electrons exist in an atom

A

in shells around the nucleus

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3
Q

What are the relative masses of each subatomic particle

A

protons: 1
neutrons: 1
electrons: 0

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4
Q

What are the relative charges of subatomic particles

A

proton: 1
neutron: 0
electron: -1

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5
Q

How do neutrons benefit the atom

A

holds the nucleus together, despite the electrostatic forces of repulsion between protons

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6
Q

How is the periodic table organised

A

in order of atomic number (number of protons)

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7
Q

What are isotopes

A

atoms of the same element but with different amounts of neutrons

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8
Q

How are isotopes represented in chemical notation

A

with mass number, atomic number and chemical symbol. Alternatively can be shown with just mass number

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9
Q

do different isotopes of an element have different reactions

A

no

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10
Q

What is heavy water

A

water with the isotope ‘deuterium’ of hydrogen, which has a mass number of 2

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11
Q

What are ions

A

a charged atom, with a different amount of protons and electrons

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12
Q

What are cations

A

positive ions, which have fewer electrons than protons

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13
Q

what are anions

A

negative ions, which have more electrons than protons

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14
Q

Why can’t mass of atoms be measured simply by adding masses of all the subatomic particles

A

because some mass is lost due to the strong force holding the nucleus together

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15
Q

How is atomic mass calculated

A

‘u’ - the mass of 1/12 of an atom of carbon-12. this is a standardized unit

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16
Q

Why does relative mass have no unit

A

because it is the ratio of two masses

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17
Q

What is relative isotopic mass

A

the mass of an isotope relative to 1/12 of the mass of carbon-12

18
Q

What is relative atomic mass

A

the average mass of an atom relative to carbon-12, weighing in all isotopes of the element

19
Q

how can finding percentage abundances of isotopes be done experimentally

A

by using a mass spectrometer

20
Q

What is the basic method that mass spectrometers use

A
  1. place sample in mass spectrometer
  2. vaporise and ionise sample to make positive ions
  3. accelerate ions. Heavier ions move slower and so isotopes are separated
  4. ions are detected on a mass spectrum as a mass: charge ratio
21
Q

what is the calculation to work out relative atomic mass

A 
                          100
22
Q

How do atoms on the left of the periodic table react (electrons)(ionic)

A

lose electrons and become cations

23
Q

How do atoms on the right of the periodic table react (electrons)(ionic)

A

gain electrons and become anions

24
Q

What charge do different atoms produce

A

group 1 - (1+)
…
group 7 (1-)
group 8 - (0)

transition metals can form several charges

25
Q

What are binary compounds

A

compounds with only 2 elements

26
Q

How are binary compounds named

A

first atom, but change end of last atom to -ide (e.g. sodium oxIDE)

27
Q

what are polyatomic ions

A

ions with atoms of more than one element

28
Q

What is the
- formula
- charge
of an ammonium ion

A

NH4
1+

29
Q

What is the
- formula
- charge
of a hydroxide ion

A

OH
-1

30
Q

What is the
- formula
- charge
of a nitrate ion

A

NO3
-1

31
Q

What is the
- formula
- charge
of a nitrite ion

A

NO2
-1

32
Q

What is the
- formula
- charge
of a hydrogencarbonate ion

A

HCO3
-1

33
Q

What is the
- formula
- charge
of a manganate (VII) / permanganate ion

A

MnO4
-1

34
Q

What is the
- formula
- charge
of a carbonate ion

A

CO3
2-

35
Q

What is the
- formula
- charge
of a sulfate ion

A

SO4
2-

36
Q

What is the
- formula
- charge
of a sulfite ion

A

SO3
2-

37
Q

What is the
- formula
- charge
of a dichromate (VI) ion

A

Cr2O7
2-

38
Q

What is the
- formula
- charge
of a phosphate ion

A

PO4
3-

39
Q

what are diatomic molecules

A

molecules containing 2 atoms bonded together

40
Q

Which elements exist as small molecules
- what are the formulas

A

H2
N2
O2
F2
Cl2
Br2
I2
P4
S8 / S

41
Q

What are the four state symbols

A

solid (s)
liquid (l)
gas (g)
aqueous (aq)

A Level Chemistry (16 decks)

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