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Chemistry > Atomic Structure and Bonding > Flashcards

Atomic Structure and Bonding Flashcards

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1
Q

Plum Pudding model

A

Positive spheres with negative electrons inside of them

Produced by JJ Thompson

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2
Q

Rutherford experiment

A
  • fired positively charged particles at extremely thin gold foil
  • most passed through but some were deflected (small number deflected backwards)
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3
Q

Rutherford model

A

Atom has tiny, positively-charged nucleus at centre and was surrounded by “cloud” of negative electrons
Most of atom is empty space

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4
Q

Bohr Model

A

Electrons were fixed in orbits (shells)

Each shell has a fixed energy

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5
Q

Electron mass and charge

A
  1. 0005 mass

- 1 charge

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6
Q

Neutron mass and charge

A

1 mass

0 charge

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7
Q

Proton mass and charge

A

1 mass

+1 charge

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8
Q

Nucleus facts

A 
Middle of atom
Contains protons and neutrons
Positively-charged (due to protons)
Almost all the mass of the atom 
Nucleus is tiny
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9
Q

Electron facts

A 
Move around nucleus in shells
Negatively-charged
Tiny but cover a lot of space
Almost no mass
Size of shell determines size of atom
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10
Q

Why are atoms neutral?

A

The number of protons is equal to the number of electrons and the charge cancels out

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11
Q

Atomic number

A

Amount of protons

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12
Q

Mass number

A

Amount of protons and neutrons

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13
Q

Isotope facts

A

They are different forms of the same element

Have the same amount of atomic number but different mass number

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14
Q

Definition of relative atomic mass

A

average mass of an element’s atom when compared to its isotopes

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15
Q

How to work out relative atomic mass

A

Multiply each relative isotopic mass by their abundance
Add up,results
Divide by sum of abundance

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16
Q

Who made the first periodic table?

A

Dmitri Mendeleev

17
Q

How did Mendeleev arrange the elements?

A

Sorted them based on their properties and put them in columns
Some element weren’t in the correct column due to him having wrong isotopes

18
Q

Groups

A

Columns of elements with similar properties

Have the same outer shell electrons

19
Q

Period

A

Another full outer shell is added to each element descending

20
Q

Electron shell rules

A

Electrons always occupy shells
Lowest energy levels are always filled first
Only certain amount of electrons are allowed in each shell (2882)

21
Q

Definition of ion

A

Atom that has lost or gained electrons

They have charge

22
Q

Anion

A

Negative ion

23
Q

Cation

A

Positive ion

24
Q

Groups most likely to become ion and why

A

1, 2, 6, 7

They are closer to getting a fuller outer shell than other groups

25
Q

How do you form the formula of an ionic compound?

A

Find the charges of the ions in the compound

The amount of each ion is the other’s charge

26
Q

Between what elements does ionic bonding take place?

A

Metals and non-metals

27
Q

Ionic bonding method

A
  • metal atom loses an electron and donates it to non-metal atom
  • this makes the metal a cation and the non-metal an anion
  • due to electrostatic forces of attraction, they are strongly attracted to each other as they are opposite charges
28
Q

Ionic compounds properties

A

Regular lattice structure (due to ESFA)
High MP and BP (due to ESFA)
Only conducts electricity when dissolved / molten as free-flowing charged particles are present
Many dissolve easily

29
Q

Adv and disadv of 2D models

A

Simple
Shows what atoms are present
Shows how atoms are connected

Don’t show shape or substance nor sizes of atoms

30
Q

Adv and disadv of dot and cross diagrams

A

Shows how compounds / molecules are formed
Shows where electrons in bonds / ions come from

Don’t show size of atoms
Don’t show how they are arranged

31
Q

Adv and disadv of 3D models

A

Good for visualising structures
More realistic than 2D

Don’t show correct scales of atoms or ions

32
Q

Covalent bond

A

Strong bond formed when pair of electrons is shared between two atoms

33
Q

Simple molecular substances

A

Molecules containing a few atoms

34
Q

Properties of simple molecular substances

A
  • very strong covalent bonds but week forces of attraction between molecules
  • low MP and BP
  • most are gases or liquids in room temperature
  • no electric conductivity
  • the larger the molecule, the strong the intermolecular bonds
35
Q

Polymers

A

Molecules made up of long chains of covalently-bonded atoms

Formed by monomers

Chemistry (10 decks)

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