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chemistry > C2 - Atoms, ions and compounds > Flashcards

C2 - Atoms, ions and compounds Flashcards

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1
Q

What is the structure of an atom?

A

-Central nucleus consisting of protons and neutrons
-Electrons orbiting nucleus in shells

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2
Q

What is the charge of a proton?

A

+1

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3
Q

What is the charge of a electron?

A

-1

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4
Q

What is the charge of a neutron?

A

Neutral

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5
Q

What is the relative mass of a proton?

A

1

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6
Q

What is the relative mass of a electron

A

1/2000
1/1836

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7
Q

What is the relative mass of a neutron?

A

1

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8
Q

Where is the majority of an atom’s mass?

A

Nucleus

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9
Q

What is the overall charge of an atom?

A

0

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10
Q

What is the role of neutrons in an atom?

A

“provide glue that holds nucleus together despite electrostatic repulsion between oppositely charged protons and electrons”

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11
Q

What is the atomic number

A

Number of protons in the nucleus of an atom
Z

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12
Q

What’s an isotope

A

Atoms of the same element with different numbers of neutrons and different atomic masses

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13
Q

What is mass number?

A

Sum of protons and neutrons in the nucleus
A

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14
Q

How is an isotope represented

A

With its mass number

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15
Q

How does the reactivity of isotopes differ?

A

Same number of electrons
So same chemical reactions

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16
Q

What is an ion?

A

Positively or negatively charged atoms or group of atoms where the number of electrons is different from the number of protons

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17
Q

What are cation?

A

Positively charged ions

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18
Q

What are anions?

A

Negatively charged ions

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19
Q

What is mass defect

A

Small amount of mass lost due to the strong nuclear force holding together protons and neutrons

20
Q

Why is mass unit, u, used?

A

Working in kg would be awkward

21
Q

What is mass of carbon-12

A

12 atomic mass units (u)

22
Q

What is relative isotopic mass?

A

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

23
Q

What is relative atomic mass?

A

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

24
Q

What is relative formula mass?

A

Weighted means mass of the formula unit of a compound compared with 1/12th of the mass of an atom of carbon-12

25
Q

What is relative molecular mass

A

Mr
Weight mean mass of a molecule of a compound compared with 1/12th of the mass of an atom of carbon-12

26
Q

What does the weighted mean mass take into account

A

Percentage abundance of each isotope
Relative isotopic mass of each isotope

27
Q

How is the percentage abundance of isotopes in a sample of an element found experimentally

A

Using a mass spectrometer

28
Q

How does a mass spectrometer work?

A

1) Sample place in the mass spectrometer
2) Sample vaporised and ionised to form positive ions
3) Ions accelerated
4) Heavier ions move slower and are more difficult to deflect so ions of isotope are separated
5) Ions are detected on a mass spectrum as a mass to charge ratio m/z
6) Greater abundance, larger signal

29
Q

M/z ratio formula

A

Relative mass of ion/ relative charge of ion

30
Q

How do you calculate relative atomic mass from abundance of isotopes

A

( Percentage adundance x atomic mass ) / 100

31
Q

What is a binary compound

A

A compound containing two elements onky

32
Q

What is a polyatomic ion

A

Ion containing more than one atom

33
Q

Ammonium ion formula

A

NH4+

34
Q

Hydroxide ion formula

A

OH-

35
Q

Nitrate ion formula

A

NO3-

36
Q

Nitrite ion formula

A

NO2-

37
Q

Hydrogen carbonate ion formula

A

HCO3 -

38
Q

Manganate (VII) ion formula
Permanganate ion

A

MnO4 -

39
Q

Carbonate ion formula

A

CO3 2-

40
Q

Sulfate ion formula

A

SO4 2-

41
Q

Sulfite ion formula

A

SO3 2-

42
Q

Dichromate (VI) ions formul

A

Cr2O7 2-

43
Q

Phosphate ion formula

A

PO4 3-

44
Q

Zinc ion formula

A

Zn 2+

45
Q

Silver ion formula

A

Ag +

46
Q

What is a formula unit?

A

Compound worked out from ionic charge ?

47
Q

States in equations

A

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

chemistry (21 decks)

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