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chem Flashcards

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1
Q

what are Elements ?

A

They are a single type of atom

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2
Q

what are compounds ?

A

2 or more elements that are chemically bonded

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3
Q

where are electrons located and what is the mass and charge of it ?

A

on outer shell –> mass = 1/2000 , charge = -1

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4
Q

where are protons located and what is the mass and charge of it ?

A

in the middle (nucleus) –> mass = 1 , charge = +1

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5
Q

where are neutrons located and what is the mass and charge of it ?

A

in the middle (nucleus) –> mass = 1 , charge = 0

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6
Q

How can we tell if the number is an atomic number and what does it represent ?

A

smaller number = protons and electrons (not added)

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7
Q

How can we tell if the number is an mass number and what does it represent ?

A

larger number = protons + neutrons

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8
Q

who discovered protons ?

A

Rutherford

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9
Q

who discovered neutrons ?

A

James Chadwick

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10
Q

who discovered nucleus ?

A

Rutherford

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11
Q

who discovered electrons ?

A

J.J. Thomson

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12
Q

who discovered the current model we know today ?

A

Bohr

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13
Q

Tell me 3 things about Dmitri Mendeleev’s table and what has changed ?

A
  • was sorted by mass and similar patterns
  • left gaps
  • he predicted properties
    (but now we arrange it in electronic arrangements – subtle difference)
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14
Q

what it the formula for
- Carbon dioxide
- water
- oxygen gas
- hydrogen gas
- nitrogen gas
- ammonia
- hydrochloric acid
- sulfuric acid

A
  • CO2
  • H2O
  • O2
  • H2
  • N2
  • NH3
  • HCI
  • H2SO4
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15
Q

Tell me 5 things about Halogens.

A
  • In group 7
  • Non metals
  • Only need to gain one electron so very reactive
  • Most reactive on top and least reactive in bottom
  • Low boil on top and high boil on bottom
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16
Q

Tell me 4 things about alkali metals.

A

– group 1
- least reactive on the top but most reactive in the bottom
- high melting point on the top but low melting point in the bottom
- Soft grey metal – need to be kept in oil so it doesn’t react with oxygen or water in the air

17
Q

Tell me 3 things about Nobel gases.

A
  • group 8/0
  • Has full outer shell
  • meaning it’s Unreactive
18
Q

what does the state symbol (Aq) stand for ?

A

aqueous

19
Q

From it’s structure why can pure metals conduct electricity and can conduct heat ?

A

Pure Metals are made up of positive atoms in a sea of delocalized electrons which are free to move meaning the metals can conduct electricity and be a really good source of conducting heat.

20
Q

Are pure metals soft or hard ? why ?

A

Pure metal has layers that can slide across each other and because of this they are soft.

21
Q

Are alloys soft or hard ? why ?

A

Alloys either have no layer or distorted layer and they cannot slide meaning they are hard.

22
Q

Explain the structure of an alloy ?

A

An alloy has the same things as a pure metal (positive atoms in a sea of delocalized electrons) but it also includes another metal or e.g. carbon that is alloyed with.

23
Q

what’s the molecule formula for Octane ?

A

C8H18

24
Q

what’s the molecule formula for hexane ?

A

C6H14

25
Q

what’s the molecule formula for methane ?

A

CH4

26
Q

what’s the molecule formula for Decane ?

A

C10H22

27
Q

what’s the molecule formula for heptane ?

A

C7H16

28
Q

what’s the molecule formula for propane ?

A

C3H8

29
Q

what’s the molecule formula for ethane ?

A

C2H6

30
Q

what’s the molecule formula for pentane ?

A

C5H12

31
Q

what’s the molecule formula for nonane ?

A

C9H20

32
Q

what’s the molecule formula for butane ?

A

C4H10

33
Q

what are the properties of transition metals ?

A
  • good conductor
  • shiny
  • hard
34
Q

what are the uses of transition metals ?

A
  • jewellery
  • wires
  • sculptures
35
Q

what are the colours of transition metals ?

A
  • copper = blue
  • iron (II) = light green
  • iron (III) = orangey brown (rust)
  • cobalt = deep rich blue
36
Q

why do group 1 elements become more reactive as you go down the line ?

A

As you move down the group the outer electrons is further away from the nucleus so it is less strongly attracted to the nucleus and is more easily lost .

37
Q

Define what is meant by the term isotope.

A

Atoms of the same element that have different numbers of neutrons.

38
Q

Define relative atomic mass.

A

The average value that takes into account the abundance of the isotopes of the element.

gcse (14 decks)

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