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A Level Chemistry OCR A > 2 - Atoms, Ions and compounds > Flashcards

2 - Atoms, Ions and compounds Flashcards

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1
Q

Define isotope

A

atoms of the same element with different numbers of neutrons and different masses.

// most elements are mixtures of isotopes

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2
Q

Mass of subatomic particles

A

Relative mass is used since subatomic particles have tiny masses.
Proton mass ~~ neutron mass
electrons have negligible mass

Proton = 1
Neutron = 1
Electron = 1/1836th mass of a proton

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3
Q

Charge of subatomic particles

A

Proton = +ve || +1
Neutron = neutral, no charge || 0
electron = -ve || -1

charge of proton is equal but opposite to charge of electron, so charges are balanced. Relative charges used.

proton actual charge = 1.6 x 10^-19C
electron actual charge = -1.6 x 10^-19C

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4
Q

Define atomic number

A

Number of protons in the nucleus of an atom.

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5
Q

Define mass number

A

The sum of the number of protons and neutrons in the nucleus - also known as nucleon number

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6
Q

Describe the atomic structure of atoms

A

Most of the atoms mass is in the nucleus. Nucleus contains neutrons and protons.
Atoms have the same number of protons and electrons, so total positive charge is cancelled by total negative charge of electrons. Overall atom is neutral.
Electrons are in shells around the nucleus.

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7
Q

Role of neutrons?

A

Neutrons can be thought of as providing the glue that holds the nucleus together despite electrostatic repulsion between the positively charged protons.
Most atoms contain same/ more neutrons than protons.
As the nucleus gets larger more neutrons are needed.

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8
Q

Define ion // atomic structure of ions

A

A charged atom or covalently bonded group of atoms where number of electrons is not equal to the number of protons.
Positive ions = CATIONS . Fewer electrons
Negative ions = ANIONS. More electrons

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9
Q

Chemical and physical properties of isotopes

A

Chemical properties depend on electrons -> number of neutrons = no effect on reactions of an element -> different isotopes of an element react similarly.

Isotopes may differ in physical properties - high MP, BP, density.

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10
Q

Define relative atomic mass

A

Weighted mean mass of an atom compared with 1/12th the mass of an atom of carbon-12

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11
Q

Define relative isotopic mass

A

Mass compared with 1/12th the mass of a carbon-12 atom

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12
Q

When is mass spectrometry used

A
  • For determination of relative isotopic masses and relative abundances of the isotope
  • for calculation of relative atomic mass of an element from relative abundance’s of its isotopes
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13
Q

Relative molecular mass vs relative formula mass

A

For simple molecules, relative molecular mass used

For compounds with giant structures, relative formula mass used

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14
Q

Nitrate ion

A

NO3 -

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15
Q

Carbonate ion

A

CO3 2-

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16
Q

Sulfate ion

A

SO4 2-

17
Q

Hydroxide ion

A

OH-

18
Q

Ammonium ion

A

NH4 +

19
Q

Zinc ion

A

Zn 2+

20
Q

Silver ion

A

Ag +

21
Q

Nitrite ion

A

NO2 -

22
Q

Hydrogencarbonate ion

A

HCO3 -

23
Q

manganate (VII) (permanganate) ion

A

MnO4 -

24
Q

Sulfite ion

A

SO3 2-

25
Q

dichromate (VI) ion

A

Cr2O7 2-

26
Q

phosphate ion

A

PO4 3-

27
Q

Binary compound

A

Contains 2 elements only

28
Q

Are nitrates soluble

A

Yes

29
Q

Are chlorides soluble

A

Yes, except AgCl and PbCl2

30
Q

Are Sulfates soluble

A

Yes, except BaSO4, PbSO4, SrSO4

31
Q

Are carbonates soluble?

A

No, except Group1 x NH4 +

32
Q

Metal + acid = ?

A

Metal + acid = salt + hydrogen

33
Q

Metal hydroxide + acid = ?

A

Metal hydroxide + acid -> salt + water

34
Q

Metal oxide + acid = ?

A

Metal oxide + acid -> salt + water

35
Q

Metal carbonate + acid = ?

A

Metal carbonate + acid -> salt + water + carbon dioxide

36
Q

How to determine relative atomic mass?

A

% of isotopes in sample of element can be found experimentally using mass spectrometer

  1. Sample placed in mass spectrometer
  2. Sample is vaporised
  3. Sample is ionised to form positive ions
  4. Ions are accelerated. Heavier ions move more slowly & more difficult to deflect than lighter ions, so ions if each isotope are separated.
  5. Ions detected on mass spectrum as mass-to-charge ratio (m/z). Each ion reaching detector adds to the signal. Greater abundance = larger signal.

mass-to-charge ratio (m/z) = relative mass of ion / relative charge on ion

A Level Chemistry OCR A (11 decks)

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