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Chemistry ;) > 3.1.1 Atomic Structure > Flashcards

3.1.1 Atomic Structure Flashcards

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1
Q

what is the relative charge of a proton?

A

+1

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2
Q

what is the mass of a proton?

A

1

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3
Q

what is the relative charge of an electron?

A

-1

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4
Q

what is the relative mass of an electron

A

1/1836

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5
Q

what is the relative charge of a neutron?

A

0

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6
Q

what is the relative mass of a neutron?

A

1

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7
Q

what does the nucleus of an atom contain?

A

protons
neutrons

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8
Q

what orbits around an atom?

A

electrons

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9
Q

what is the force of attraction held between protons and neutrons?

A

nuclear force

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10
Q

what is the force present between protons and electrons?

A

electrostatic force

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11
Q

what is the relative charge of an atom of an element?

A

neutral

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12
Q

what letter is the mass number represented by?

A

A

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13
Q

what letter is the atomic number presented as?

A

Z

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14
Q

what is the atomic number?

A

the number of protons+electrons

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15
Q

what is the mass number?

A

total number of neutrons and protons in a nucleus

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16
Q

how can you find the number of neutrons?

A

mass number - atomic number

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17
Q

what are the stages of time of flight mass spectrometer

A

ionisation
acceleration
ion drift
ion detection
data analysis

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18
Q

why is the sample held within a vacuum

A

so that arent react with the gases in the atmosphere.

19
Q

what occurs during ionisation. (TOF)

A

converts the atoms to positive ions by knocking off an electron.

20
Q

what is electrospray ionisation?

A

sample is placed in a volatile solvent
is forced through a fine needle: giving fine mist/aeorsal
tip of needle has high voltage
sample gains a proton H+

21
Q

what is electron impact?

A

electron gun forces high energy electron towards sample
knocks out an electron
forms positive ion

22
Q

what is the general formula of an atom losing an electron
1st ionisation energy

A

X(g)–> X+(g) + e-

23
Q

what happens when the ions are attracted to negatively charged plate?

A

they accelerate towards the plate

24
Q

what is the kinetic energy of the ions

A

it is constant.

25
Q

will smaller ions have a greater speed

A

yes

26
Q

what is speed of the ions in the ion drift?

A

smaller ions move faster
larger ions move slower

27
Q

what occurs during ion detection?

A

the ions pick up an electron
which causes a current to flow

28
Q

what does the flow of current represent?

A

size of current is proportional to the abundance of the isotope

29
Q

what happens when a molecule interacts with electron impact?

A

causes fragmentation

30
Q

what is the mass spectrometer used for?

A

relative abundance of isotopes
relative isotopic mass

31
Q

how can we find the relative isotopic mass

A

isotopic mass*relative abundance / total relative abundance

32
Q

what are the names of the sub shells/ orbitals

A

s,p,d,f

33
Q

how many electrons does a s-orbital hold?

A

2

34
Q

how many electrons does the p orbital hold

A

6

35
Q

how many electrons does the d orbital hold?

A

10

36
Q

what is the first ionisation energy?

A

energy required to remove 1 mole of an electron from a mole of atoms in its gaseous state
measured in kJ/mol

37
Q

what is an example of the 2nd ionisation energy?

A

X+ –> X2+ +2e-

38
Q

what factors affect ionisation energy?

A

nuclear charge
atomic radius
shielding

39
Q

what is the trend in ionisation energy in period 3

A

increases
-across the group nuclear charge increases (proton no. IN)
-electrons have greater attraction to +ve nucleus
-decreases atomic radius
-same orbitals

40
Q

how does sulfur deviate from the trend in ionisation energy?

A

DECREASES
electrons are paired in the same p orbital
repulsion between them
less energy required to break forces

41
Q

what is the trend in first ionisation energies as you go down the group?

A

DECREASES
atomic radius increases
outermost electron further away from nucleus
more shielding
weaker attraction to nucleus.

42
Q

what is the relative atomic mass

A

the average mass of an atom compared to 1/12 of the mass of the atom carbon.

43
Q

in what ways are isotopes the same?

A

same electronic configuration.

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