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Chemistry > Atomic structure & periodic table > Flashcards

Atomic structure & periodic table Flashcards

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1
Q

What is the mass and charge of

  • protons
  • neutrons
  • electrons
A

Proton : M= 1 C= +1
Electron: M= almost 0 C= -1
Neutron: M= 1 C= 0

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2
Q

What is meant by ‘atomic number’

A

The number of protons in the nucleus

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3
Q

What is meant by ‘mass number’

A

The total number of protons and neutrons in the nucleus

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4
Q

What is an isotope

A

An atom with the same atomic number but different mass number (same proton number different number of neutrons)

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5
Q

Define ‘ relative atomic mass’

A

The ‘mean mass’ of an atom of an element compared to 1/12th of the mass of an atom of carbon-12

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6
Q

Define ‘relative isotopic mass’

A

The mean mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon-12

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7
Q

When we talk about the ‘relative mass’ in general, what is meant?

A

Whenever we say relative mass of anything we are comparing the mass of an atom to the mass of a different atom.

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8
Q

How do you work out the ‘relative formula mass’ and when do we use this term ?

A
  • Work it out by adding all the relative atomic mass values of the atoms together.
  • We use it when referring to simple molecules
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9
Q

How do you work out the ‘relative molecular mass’ and when do we use this term ?

A
  • Work it out by adding all the relative atomic mass values of the atoms or ions present.
  • We use it when referring to giant covalent and ionic compounds
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10
Q

What does ‘Ar’ and ‘Mr’ stand for?

A

Ar refers to the relative atomic mass

Mr refers to the relative molecular mass

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11
Q

True or False:

The relative atomic mass of an ion is different to the relative atomic mass of the atom.

A

False - Electron number makes no difference to the mass number so the Ar of an ion is the same as the Ar of the atom.

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12
Q

What is meant by ‘ isotopic abundance’

A

the percentage of that isotope that exists in a naturally occurring sample

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13
Q

How to calculate the relative atomic mass of an element from its isotopic abundance?

A

Use the formula:
Relative atomic mass X isotopic abundance (do this for all the values and add them up) T
hen divide by sum of isotopic abundances

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14
Q

How to calculate the isotopic abundance using relative atomic masses:

A

Use the formula, rearrange to find X (missing value)
Relative atomic mass X isotopic abundance (do this for all the values and add them up)
Then divide by sum of isotopic abundances

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15
Q

What does the X axis of the mass spec tell us?

A

The X axis tells us the M/Z (mass to charge) ratio.

If the charge is +1, then this is the same as the relative isotopic mass.

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16
Q

What does the Y axis of the mass spec tell us?

A

The Y axis tells us the relative abundance (%) of the isotopes

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17
Q

What do mass specs do?

A

They measure the masses of atoms and molecules in samples

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18
Q

What is the ‘molecular ion peak’ aka ‘ The M peak’ and what does it tell us ?

A

It is the peak with the highest m/z charge and it tells us the molecular mass of a compound on a mass spec.

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19
Q

In what molecules do we have the M+1 peak and what causes it?

A

The M+1 peak tends to be found in molecules with a large mass and is caused by small samples of carbon-13 that may be present in the sample.

20
Q

What are the steps to predicting the mass spec of diatomic molecules?

A
  • Write out the different combinations of molecules that can be made using the different isotopes
  • Multiply the abundances of the different isotope to the combinations made
  • Add up the abundances for combinations that are the same
  • Divide all the abundances by the smallest number to make whole number ratios
  • Draw Mass spec according to the ratios produced
21
Q

What is an orbital?

A

A region within an atom that can hold 2 electrons with opposite spins

22
Q

What are 2 other words for electron shell?

A

Quantum shell

Energy level

23
Q

What are quantum shells divided into?

A

Sub-shells

24
Q

What are sub-shells made up of?

A

Orbitals

25
Q

What are the 4 sub-shells?

A

S sub-shell
P sub-shell
D sub-shell
F sub-shell

26
Q

How many electrons can each sub-shell hold?

A 
S = 2 electrons 
P= 6 electrons
D= 10 electrons
F= 14 electrons
27
Q

How many orbitals are in each sub-shell

A 
S = 1 orbital 
P= 3 orbitals 
D= 5 orbitals 
F= 7 orbitals
28
Q

How many electrons can an orbital hold?

A

2 electrons per orbital

29
Q

TRUE OR FALSE
‘The quantum shell closest to the nucleus has the highest energy level’
Give reasoning for answer

A

FALSE
The further away from the nucleus ,the higher the energy level, this is because it requires more energy to pull electrons from the positive force of the protons in the nucleus.

30
Q

Draw the shape of the S orbital

A

Spherical shape

31
Q

Draw the shape of the P orbitals

A 
PX= Horizontal dumbbell
PY= Vertical dumbbell
PZ= Diagonal dumbbell
32
Q

At what angle are the 3 P orbitals arranged ?

A

90 degrees angle

33
Q

What is ‘spin pairing’

A

The idea that electrons have to spin in opposite directions in orbitals

34
Q

How to electrons fill orbitals?

A

Electrons fill orbitals singly before pairing up

35
Q

Which energy levels fill up first?

A

Lowest energy levels fill up first

36
Q

When writing an electronic configuration what is included?

A
  • Number of the quantum shell
  • The sub-shell
  • Total Number of electrons in the sub-shell.
37
Q

How do we use group 8 elements to write electron configuration?

A

We use the group 8 element on the previous period (previous line) and write the element in brackets and continue the configuration of the desired element

38
Q

Where in the periodic table is the;

  • S block
  • D block
  • P block
  • F block
A

S block= metals (left hand side)
D block= transition metals (middle)
P block = right hand side
F block= bottom 2 rows under transition metals (lanthanide and actinide series)

39
Q

What is ionisation energy

A

The energy required to remove an electron from one mole of a gaseous atom of an element

40
Q

What is the trend across a group and along a period in regards to atomic radius and explain why this is the case

A

Down a group the atomic radius increases as there is an increase in quantum shells .
Across a period the atomic radius decreases because as you go along a period, the number of electron increase however they are on the same quantum shell. The concentration of protons in the nucleus also increases creating a ‘higher effective nuclear charge’(stronger force pulling electrons inwards)

41
Q

What is the trend with ionic atom radii in comparison to their respective atoms?

A

Anions(-) have larger ionic radii compared to their atoms due to more electron-electron forces spreading them further apart. and also more electrons than protons so protons cannot tightly pull the extra electrons to the nucleus

Cations(+) have a smaller ionic radii compared to their atoms as they experience less electron-electron repulsion and have more protons than electrons meaning they have stronger inward pull on the electrons more tightly.

42
Q

What is the mass of an electron?

A

1/2000

43
Q

What do we call the sub-atomic particles in the nucleus as a whole?

A

Nucleons

44
Q

In the periodic table, what is the larger number out of the 2 given for an element ?

A

Larger number = mass number (P+N)

Smaller number= atomic number (P)

45
Q

Describe arrangement of the periodic table now and before

A

Now;
- arranged in increasing order of atomic number (protons)

Before:
- arranged in order of atomic mass

46
Q

Why do isotopes react in the same way?

A

Because they have to be same electronic configuration (as electron number is the same)

47
Q

What chemical reaction can the student perform to determine which isotope is which?

A

No chemical reaction can be used to differentiate between isotopes . This is because they are chemically identical as they contain the same number of electrons.

Chemistry (10 decks)

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