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Chemistry > Booklet 1 - structure > Flashcards

Booklet 1 - structure Flashcards

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1
Q

What is a atom?

A

Smallest part of an element that can exist. It cannot be divided

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2
Q

What is an element?

A

Substance that contains only one type of atom

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3
Q

What is a compound?

A

Substance that contains more than one type of atom, chemically bonded together

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4
Q

What are valencies?

A

Combining powers of atoms and can be used to work out the formula of compounds

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5
Q

What are radical groups?

A

Atoms that like to group together with other atoms and stay with each almost all the time including chemical reactions

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6
Q

What is a molecule?

A

Two or more atoms chemically bonded together

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7
Q

What is a mixture?

A

Two of more substances (elements or compounds) that are not chemically bonded together

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8
Q

What is the formula, valency and charge of Ammonium?

A

NH4 - 1 - postive 1

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9
Q

What is the formula, valency and charge of Sulfate?

A

SO4 - 2 = -2

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10
Q

What is the formula, valency and charge of Hydroxide?

A

OH - 1 = -1

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11
Q

What is the formula, valency and charge of Nitrate?

A

NO3 - 2 = -2

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12
Q

What is the formula, valency and charge of Carbonate?

A

CO3 - 2 =-2

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13
Q

What is the formula, valency and charge of Hydrogen Carbonate?

A

HCO3 - 1 = -1

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14
Q

How can mixtures be separated? (3 examples)

A

1) . Silicon dioxide from water by filtration
2) . Salt from water by evaporation or distillation
3) . Dyes in ink by chromotography

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15
Q

What’s the atomic number?

A

Number of protons

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16
Q

What can both protons and neutrons be called?

A

Nucleons as they both exist in the nucleus

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17
Q

What are the two most important thing about the atomic number?

A

1) . All elements of the same type have the same atomic number
2) . All atoms identity depends on the number of protons in its nucleus

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18
Q

What is an isotope?

A

Atoms of the same element, they have the same number of protons but different amount of neutrons so their mass number is different

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19
Q

What is the relative atomic mass?

A

An avergae value that takes account of the abundance of the isotopes of the isotopes if the element.

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20
Q

When is the arrangement of electrons most important?

A

When considering how an element reacts, or whether it will react at all

21
Q

What are the physical properties of Group 8/0 noble gases?

A
  • All unreactive, wont set on fire
  • the boiling points of the gases increase as you move down the group along with increasing relative atomic mass
  • they are colourless gases at room temperature
  • have ions with different charges
  • form coloured compounds
  • useful at catslysts
22
Q

Why don’t noble gases react?

A

Have full outer shells so do not need to move electrons between themselves and other atoms = already have stable electron configuration

23
Q

What the physical properties of Group 1 elements alkali metals?

A

Metals with low density
Soft and can be cut with a knife
Show a shiny interior that becomse dull on reaction with oxygen

24
Q

Why are Group 1 elements so reactive?

A

The outer electron is more easily lost as the attraction between the nucleus and the electron decreases, as the electron is futher away drom the nucleus the futher down you go

25
Q

Whay are the word and symbol equations of Group 1 elements reacting with water? (Lithium, sodium, potassium)

A

1). Lithium + water -> lithium hydroxide + hydrogen
2 Li + 2 H2O -> 2 LiOH + H2
2). Sodium + water -> sodium hydroxide + hydrogen
2 Na + 2 H2O -> 2 NaOH + H2
3). Potassium + water -> potassium hydroxide + hydrogen
2 K + 2 H2O -> 2 KOH + H2

26
Q

What is the pattern with group 1 element reactions?

A

All react to produce hydrogen gas and an alkali metal hydroxide

27
Q

What are the word equations for Group 1 elements reacting with chlorine?

A

1). Lithium + chlorine -> lithium chloride
2 Li + Cl2 -> 2 LiCL
2). Sodium + chlorine -> sodium chlorine
2 Na + Cl2 -> 2 NaCl
3). Potassium + chlorine -> potassium chloride
2 K + Cl2 -> 2KCl

28
Q

What are the word equations for Group 1 elements with oxygen?

A 
1). Lithium + oxygen -> lithium oxide
4 Li + O2 -> 2 Li2O
2). Sodium + oxygen-> sodium oxide
4Na + O2 -> 2 Na2O
3). Potassium + oxygen -> potassium oxide
4 K + O2 -> 2K2O
29
Q

What do all alkali metals that burn in oxygen form?

A

Metal oxides which are white solids

30
Q

What are the physical properties of Group 7 the halogens?

A

They are non metals and consist of molecules that are diatomic

31
Q

What happens to molecules futher down the group in Group 7?

A

The higher the mass of its molecules, its melting and boiling points also increase

32
Q

What is the reactivity of group 7 elements like?

A

Its harder to gain an extra electron, and its futher from the nucleus so it becomes LESS reactive as you go down the group

33
Q

What is a halogen that gains a electron called?

A

A halide ion

34
Q

What are the trends of Group 1 elements and Group 7 elements?

A

The bigger and more energy levels the atoms have:-

  • In Group 1 elements the more easily electrons are lost
  • In group 7 the less easily electrons are gained
35
Q

What happens to Group 1 elements the higher up the group an element is?

A

The lower its atomic number

36
Q

How many electrons are in Group 1 outer shell?

A

1 electrons

37
Q

How many electrons are in Group 8/0 outer shell?

A

Full 8 electrons

38
Q

How many electrons are in Group 7 outer shell?

A

7 electrons

39
Q

What are the two other trends for group 1 elements?

A
  • lower melting and boiling points

- higher relative atomic mass

39
Q

What is the trend for group one elements reacting with water?

A

The more reactive (lower down the group) an alkali metal is, rhe more violent the reaction
- the amount if energy given out by the reacrion increases down the group

39
Q

What are the trends of group 1 elements with chlorine?

A
  • when heated in chlorine gas they form white metal chloride salts
  • as you go down the group the reactivity increases so the reaction gets more vigorous
40
Q

Why do group 1 metals tarnish in air?

A

Upon reaction with oxygen, the metal reacts and forms a dull metal oxide layer

42
Q

What are the differences between group 1 and transition elements?

A
  • group 1 elements are much more reactive than transition metals, they react more vigorously with water, oxygen and group 7 elements
  • they’re also less dense, strong and hard than transition metals and have lower melting points
42
Q

What type of do halogens form when they react with metals?

A

Ionic bonds

43
Q

Why do Group 0 elements boiling points increase as you go down the group?

A

Due to an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome

44
Q

What can a more reactive halogen do?

A

Displace a less reactive halogen from an aqueous solution of its salt

45
Q

what are the relative charges of particles in the atom?

A
  • proton - +1
  • neutron - 0
  • electron - -1
46
Q

what are the relative masses of particles in the atom?

A
  • proton - 1
  • neutron - 1
  • electron - very small
47
Q

how can halogens share electrons with other non-metals?

A

via covalent bonding and make simple molecular structures

Chemistry (12 decks)

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