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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

Atomic Structure: The Atom

What are the Subatomic Particles?

A
  • Protons
  • Electrons
  • Neutrons
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2
Q

Atomic Structure: The Atom

What is the Relative Mass of a Proton?

A

1

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3
Q

Atomic Structure: The Atom

What is the Relative Charge of a Proton?

A

+1

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4
Q

Atomic Structure: The Atom

What is the Relative Mass of an Electron?

A

0

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5
Q

Atomic Structure: The Atom

What is the Relative Charge of an Electron?

A

-1

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6
Q

Atomic Structure: The Atom

What is the Relative Mass of a Neutron?

A

1

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7
Q

Atomic Structure: The Atom

What is the Relative Charge of a Neutron?

A

0

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8
Q

Atomic Structure: The Atom

Which one’s greather Atomic number or Mass number?

A

Mass number

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9
Q

Atomic Structure: The Atom

What is the Atomic Number?

A

Proton number

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10
Q

Atomic Structure: The Atom

What is the Mass Number?

A

Total number of protons & neutrons

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11
Q

Atomic Structure: Isotopes

What is an Isotope?

A

Atoms with the same atomic number but different mass number

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12
Q

Atomic Structure: Isotopes

Which properties do Isotopes share?

A

Chemical
↳ have the same electron configuration

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13
Q

Atomic Structure: Isotopes

Which properties in Isotopes differ?

A

Physical
↳ depend on its mass

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14
Q

Atomic Structure: Relative Mass

What is the Relative Atomic Mass?

A

Average mass of an atom compared to 1/12 of carbon 12

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15
Q

Atomic Structure: Relative Mass

What is the Relative Isotopic Mass?

A

Average mass of an isotope compared to 1/12 of carbon 12

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16
Q

Atomic Structure: Relative Mass

What is meant by the term ‘Abundance’?

A

How much

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17
Q

Atomic Structure: Relative Mass

How would you workout the Ar from Isotopic Abundances?

A
  • Multiply each relative isotopic mass by its % relative isotopic abundance
  • Add them up
  • Divide by 100
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18
Q

Atomic Structure: Mass Spectra

What does the Mass Spectra show?

A
  • Relative Isotopic Masses
  • Abundances of diff elements
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19
Q

Atomic Structure: Mass Spectra

What does the y-axis show?

A

The abundance of ions

Often as %

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20
Q

Atomic Structure: Mass Spectra

What does the Height of the peak show?

A

Relative Isotopic Abundance

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21
Q

Atomic Structure: Mass Spectra

What does the x-axis show?

A

m/z or the Relative Isotopic Mass

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22
Q

Atomic Structure: Mass Spectra

How would you workout the Relative Atomic Mass from a Mass Spectra graph?

A
  • Multiply each Relative Isotopic Mass by its Relative Isotopic Abundance
  • Add them up
  • Divide by the sum of Isotopic Abundances
23
Q

Atomic Structure: Mass Spectra

How would you workout the Relative Abundance for Diatomics?

A
  • Express each % as a decimal
  • Make a table showing each possible mol
  • Add together any duplications
24
Q

Atomic Structure: Mass Spectra

How would you workout the Mass Spectrum for Diatomics?

A
  • Divide all Relative Abundances by the smallest one
    ↳ works out the smallest whole number ratio
25
Q

Atomic Structure: Electron Structure

What is meant by the term ‘Configuration’?

A

Arrangement

26
Q

Atomic Structure: Electron Structure

What are the 4 Subshells?

(blocks)

A
  • S
  • P
  • D
  • F
27
Q

Atomic Structure: Electron Structure

What is an Orbital?

A

Space where you find electrons

28
Q

Atomic Structure: Electron Structure

How many electrons can each orbital hold?

A

Level 1 (s) = 2
Level 2 (s+p) = 8
Level 3 (s+p+d) = 18
Level 4 (spdf) = 32

29
Q

Atomic Structure: Electron Structure

What is S Block Shape?

A

Spherical

30
Q

Atomic Structure: Electron Structure

What is the P Block Shape?

A

Dumbbell

31
Q

Atomic Structure: Electron Configuration

What are its Rules?

A
  1. Electrons enter the lowest available energy level
  2. No 2 electrons can have the same spin
  3. When in orbitals of equal energy, electrons will try to remain unpaired
32
Q

Atomic Structure: Electron Configuration

How would u formulate a Condensed one?

A
  1. Locate element of choice
  2. Find noble gas that comes DIRECTLY before your element
  3. Put the chemical symbol of that noble gas in squared brackets
  4. Complete the rest of the configuration
33
Q

Atomic Structure: Electron Configuration

What’s Chronium’s EC?

A
  • Donate one of their 4s electron to their 3rd shell
    ↳ more stable with a full/half full d-shell
34
Q

Atomic Structure Electron Configuration

What’s Copper’s EC?

A
  • Donate one of their 4s electron to their 3rd shell
    ↳ more stable with a full/half full d-shell
35
Q

Atomic Structure: Electron Configuration

What are Isoelectric Ions?

A

Different charged ions with the same electron configuration

36
Q

Atomic Structure: Atomic Emission Spectra

What happens when an electron is given EMR?

A

It absorbs the heat
↳ giving it enough energy to jump to a higher QL

37
Q

Atomic Structure: Atomic Emission Spectra

What happens to that same electron over time?

A

It will fall back to its OG QL
↳ releasing heat

38
Q

Atomic Structure: Ionisation Energies

What is meant by the term ‘Ionisation Energy’?

(endo)

A

Amount of energy needed to remove electrons from atoms

39
Q

Atomic Structure: Ionisation Energies

What is the 1st Ionisation Energy?

A

Energy required to remove ONE MOLE of electrons from ONE MOLE of gaseous atoms to form ONE MOLE of gaseous positive ions

40
Q

Atomic Structure: Ionisation Energies

What are the factors affection Ionisation energy?

A
  • Atomic Radius : smaller = greater attraction to nucleus
  • Nuclear Charge : more electrons = greater pull from nucleus
  • Shiedling : less pull from nucleus : blocked by inner electrons
41
Q

Atomic Structure: Ionisation Energies

What happens to the Ionisation Energy as u go Down a group?

A

Decreases

42
Q

Atomic Structure: Ionisation Energies

Why does the Ionisation Energy decrease going Down a group?

A
  • Down a group, the bigger the Atomic Radius
    ↳ has more shells
  • Less Nuclear Charge
    ↳ easier to remove outer electrons : Shielding
43
Q

Atomic Structure: Ionisation Energies

What is meant by Successive Ionisation Energy?

A

As you ionise something successively, you ionise it more than once

44
Q

Atomic Structure: Ionisation Energies

Why is the Successive Ionisation Energy higher?

A
  • Positively charged ions have a greater number of protons than electrons
    ↳ more energy is needed : as you’re staring from a positive level rather than neutral
45
Q

Atomic Structure: Ionisation Energies

What is meant by the term ‘2nd Ionisation Energy’?

A

Energy required to remove ONE MOLE of electrons from ONE MOLE of gaseous ions to form ONE MOLE of TWO gaseous positive ions

46
Q

Atomic Structure: Ionisation Energies

How would u workout an element’s group using a table with its data values?

A
  1. Locate the biggest adjacent numeric jump
  2. Element’s group is based on where the jump starts
47
Q

Atomic Structure: Periodicity

What is meant by the term ‘Periodicity’?

A

Trends

48
Q

Atomic Structure: Periodicity

What happens to the Atomic Radius across a period? Why?

Size of the atom

A

DECREASES
↳ because the nuclear charge increases & attracts the outer electrons closer to the nucleus

49
Q

Atomic Structure: Periodicity

What happens to the Ionisation Energy across a period? Why?

General trend of ionisation across QL 2 & 3

A

GENERALLY INCREASES
↳ proton number increases : stronger nuclear charge

50
Q

Atomic Structure: Periodicity

Why is there a drop in energy between Mg & Al?

A
  • Further away from the nucleus, the more energy that electron has
    ↳ has less attraction from nucleus
  • Its outershell is shielded by the inner elecrons
    ↳ this makes the outershell of electrons to be lost easily
  • Therefore it is easier to remove that outshell which requires less heat
51
Q

Atomic Structure: Periodicity

Why is there a drop in energy between P & S?

A
  • Sulfur refills its 1st orbital due to its configuration
  • When electrons are paired they exert a force of repulsion
    ↳ this force is enough to make the energy drop
52
Q

Atomic Structure: Periodicity

What happens to the Mp/Bp across a period? Why?

(For metals)

A

INCREASES
* metallic bonds get stronger

53
Q

Atomic Structure: Periodicity

What happens to the Mp/Bp across a period? Why?

(For non-metals)

A

DECREASES
* LFs are weak & easy to overcome

54
Q

Atomic Structure: Periodicity

What happens to Mp/Bp when the Atomic radius increases?

A

INCREASES
* there are more electrons : more LFs
↳ more energy needed to break bonds

Chemistry (13 decks)

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