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Chemistry > Atomic Structure + The Periodic Table > Flashcards

Atomic Structure + The Periodic Table Flashcards

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1
Q

What do atoms contain?

A

Electrons
Protons
Neutrons

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2
Q

What is the Nucleus?

A
  • made of of a proton and a neutron
  • positive charge
  • centre of the atom
  • almost all of the mass
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3
Q

What are the Relative masses and charges for Protons, Neutrons and Electrons?

A

Proton: 1, +1
Neutrons: 1, 0
Electrons: 0, -1

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4
Q

What is the electron?

A
  • Revolve around the nucleus on electron shells
  • negatively charged
  • very small
  • virtually no mass
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5
Q

What sub-atomic particle decided what type of atom an atom is?

A

The proton

  • number of protons
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6
Q

What is an element?

A

a substance that only contains atoms all with the same number of protons

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7
Q

What are Isotopes?

A

A group of atoms with the same number of protons but a different number of neutrons

  • different forms of the same element
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8
Q

What are Compounds?

A

Substances formed with two or more elements, held together by chemical bonds

  • When elements react, atoms combine with other atoms
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9
Q

What is a Mixture?

A

2 or more elements or compounds that aren’t chemically bonded

  • no chemical bond between different components in the mixture
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10
Q

How can mixtures be separated?

A

Physical methods
- filtration,
- crystallisation
- simple distillation
- fractional distillation
- chromatography

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11
Q

What are some examples of mixtures?

A
  • Air
  • Crude oil
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12
Q

What did John Dalton theorise about atoms at the Start of the 19th Century?

A
  • atoms were solid spheres
  • different spheres make up different elements
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13
Q

What did JJ Thompson conclude in 1897 about atoms?

A
  • atoms weren’t solid spheres
  • atoms contained a smaller negatively charged particle-> electron
  • Plum Pudding Model- positive charged atom with negative electrons
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14
Q

What did Ernst Rutherford prove in 1909 about the atom?

A
  • Alpha particle scattering experiments: Fired positively charged alpha particles at a thin sheet of gold
  • some particles deflected more than expected, even backwards (disproved plum pudding model)
  • Nuclear Model of the Atom
  • tiny positive nucleus, cloud of negative electrons surround
  • atoms are mostly empty space
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15
Q

What is an alpha particle?

A

The nucleus of a helium atom

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16
Q

What did Bohr discover about the nuclear model?

A
  • Nuclear model of the atom-> electrons and positive nucleus would attract, atom would collapse
  • Electrons were fixed on shells, orbiting at a fixed distance
17
Q

What did Rutherford further discover AFTER Bohr’s electron shells?

A
  • The nucleus can be divided into smaller particles, same charge as the hydrogen nucleus-> called Protons
18
Q

Finally, what did James Chadwick discover about the atom?

A

20 years AFTER the discovery of the nuclei
- provided evidence of a neutral particle in the nucleus-> Neutrons

19
Q

What is the order of the discoveries to do with the Atom?

A

John Dalton- Atoms
JJ Thompson- Electrons
Ernst Rutherford- Nucleus
Bohr- Electron Shells
Rutherford- Protons
James Chadwick- Neutrons

20
Q

Where are the lowest energy levels located on the atom?

A

closest to the nucleus

  • filled first
21
Q

In the early 1800’s, how were Elements arranged?

A

By Atomic Weight

The other obvious way:
By Physical and Chemical properties

22
Q

What was wrong with early periodic tables?

A
  • Some elements were placed in the wrong group-> order of atomic weight
  • The tables weren’t complete
23
Q

What did Dmitri Mendeleev discover about the periodic table in 1869?

A

He took the 50 known elements and arranged them with gaps, predicting new elements

-Ordered them in atomic weight but moved some to take into account chemical properties
- Gaps left to make sure the right elements stayed with the right groups, predicting what was going to be in the gaps

24
Q

How is the Modern Periodic table ordered?

A
  • in increasing atomic number, thus repeating patterns of elemental properties
  • can see which elements are metals and non-metals
  • similar propertied form columns (groups)-> how many electrons in the outer shell
  • ## rows-> periods, accounts for how many electron shells the atom has.
25
Q

What is the trend of reactivity in Group 1?

A

The elements react more vigorously as you go down the group

26
Q

What is the trend of reactivity in Group 7?

A

The elements become less reactive as you go down the group

27
Q

What are Transition metals?

A
  • typical metal properties
  • can have more than 1 ion
  • often coloured
  • good catalysts
28
Q

What are the properties of Group 1 elements?

A
  • 1 electron in the outer shell, highly reactive
  • soft, low density
  • increasing reactivity as you go down
  • lower melting and boiling points as you go down
  • higher relative atomic mass

React with water-> vigorous, produce Hydrogen gas + metal hydroxides (alkali solutions)
- more energy released + more reactive as you go down

React with Chlorine-> vigorous, produce white metal chloride salts
- more vigorous as you go down

React with Oxygen-> form metal oxide (lithium oxide, sodium oxide or sodium peroxide)

29
Q

What is the difference between Group 1 metals and the Transition metals?

A

Group 1 = much more reactive, more vigorous reaction

  • less dense, strong hard
  • lower melting points
30
Q

What are the properties of Group 7 elements?

A

Halogens
All exist as diatomic molecules

  • less reactive as they go down
  • higher melting and boiling points as you go down
  • higher relative atomic mass as you go down

Form ionic bonds with metals-> Halides

31
Q

What are the coloured vapours of the Halogens?

A

Fluorine-> reactive, poisonous, yellow gas
Chlorine-> reactive, poisonous, dense green gas
Bromine- dense, poisonous red-brown volatile liquid
Iodine-> dark grey solid or purple vapour

32
Q

What are the properties of Group 0 elements?

A

Noble gases
8 electrons in outer shell, fully reacted (helium has 2)
Inert- unreactive
Monatomic gases- single, not bonded

colourless at room temperature
non flammable

Boiling and melting points increase as you move down
Increasing relative atomic mass as you go down

Chemistry (13 decks)

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