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Chemistry > C1&2 (Atoms, Elements And Compounds) > Flashcards

C1&2 (Atoms, Elements And Compounds) Flashcards

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1
Q

What is an element

A
  • simple substance
  • cannot be split up smaller through chemical reactions
  • particles that make up an element are called atoms (same kind)
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2
Q

What is an atom

A
  • smallest part of an element which can exist

- protons, neutrons and electrons are subatomic particles

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3
Q

Where are protons, neutrons and electrons found?

A

Protons and neutrons- nucleus

Electrons- outer shell/ energy level

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4
Q

Protons, neutrons and electrons relative charge and mass

A

Protons- RC +1 RM 1
Neutrons- RC 0 RM 1
Electrons- RC -1 RM 1/2000

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5
Q

Radius of an atom and the nucleus

A

Atom- 0.1 nm

Nucleus- 1/10,000

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6
Q

Molecules

A

A group of atoms covalently bonded

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7
Q

Noble gasses= monatomic elements

A
  • consisting of a single atom (goes around on its own)
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8
Q

Diatomic elements

A
  • consisting of two atoms covalently bonded
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9
Q

Polyatomic elements

A
  • consisting of multiple atoms covalently bonded
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10
Q

What is a mixture?

A
  • two or more elements or compounds not chemically bonded

- chemical properties are unchanged in each mixture

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11
Q

What are isotypes?

A

Atoms of the same element that have a different number of neutrons

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12
Q

What is the Plum Pudding model?

A
  • J J Thompson

- atom is a ball of positive and negative charge

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13
Q

What is the nuclear model?

A
  • dense positive centre

- with negative charge randomly around it

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14
Q

Niels Bohr work?

A

Adapted the nuclear model to suggest the electrons orbit the centre

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15
Q

What is an ion?

A
  • charged atom or group of atoms

- gaining or loosing an electron

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16
Q

Periodic table: 1808 John Dalton

A
  • ordered elements through the atomic weight
17
Q

Periodic table: John Newlands 1864

A
  • ordered the elements in order of mass

- didn’t leave space for predicted elemente

18
Q

Periodic table: 1869 Dimitri Mendeleev

A
  • periodic table know today
  • atomic mass and columns for similar properties
  • left space for predicted elements
19
Q

Properties of metals

A
  • malleable
  • good conductors of electricity
  • high melting point
  • sonorous (ring when hit)
  • solid at room temperature
20
Q

Properties of Non-Metals

A
  • non malleable (brittle)
  • not good conductors
  • negative ions
  • low melting point
  • gas or liquid state
21
Q

Reaction in Group 1 elements

A

Alkali Metals

  • extremely reactive
  • donate their outer most electron (positive ion)
  • more outer most shell, electrostatic attraction weakens
  • react with oxygen to form a base
  • react with water to produce alkali or hydrogen gas
22
Q

Physical properties of halogens

A
  • low melting point, increases going down
  • poor conductors of electricity
  • as it goes down you gain an electron, less energy levels means it is easier to grab an electron
  • minus 1 charge
23
Q

Displacement theory

A

If the metal halide is mixed with the more reactive hydrogen, the extra electron will transfer from less reactive to more reactive.

24
Q

Properties of transition metals

A
  • good conductors
  • less reactive then group 1
  • high density
  • can be used as catalysts
  • high melting point
  • reacts slowly with air and water
  • malleable and ductile
  • lustrous
  • harder then group 1
  • they make coloured compounds
  • have different ion charges
25
Q

3 uses of transition metals?

A
  • gold used for jewellery as it is shiny and malleable
  • copper is used for cables as it is highly dense and good conductors of electricity
  • titanium used for hip replacements as they have a low density
26
Q

What are ions?

A

This is when the element does not have the same number of valence electrons and elements have different oxidation state

27
Q

Why do ions bond?

A
  • They want to become like the Noble gasses and have a full amount of valence electrons in their outer most shell
  • create a stable electronic configuration
28
Q

What would calcium chloride (ca^2+ cl^-) become?

A

Cacl2

29
Q

What would (FE^3+ SO4^2-) become?

A

FE2(SO4)3

30
Q

Describe the term giant lattice structure

A
  • the ionic bond between the charged particles result in this structure
  • the electrostatic force is equal in all directions, this is why the ions in the structure are held strongly

Chemistry (13 decks)

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