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Chemistry Flashcards

1
Q

Periodic Table

A

A table of all known elements in the world

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2
Q

What are Noble Gases

A

Elements which have a full outer shell (valence shell) and as a result they generally are unreactive

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3
Q

What are salts?

A

Basically a salt is a compound consisting of a metal and a non-metal

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4
Q

Characteristics of metals

A

Lustre, often conducts heat and electricity, malleable, prefers to donate electrons rather than recieve them

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5
Q

What scale is used for Acids and Bases and characteristics of the scale

A

The pH scale is used. Goes from 1 to 14. 1 - 7 is for acids while 7-14 is for bases. Neutral is number 7 on the pH scale. The word pH means ‘concentration of Hydrogen’

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6
Q

What is the outermost shell called and what does it often determine?

A

The outermost shell is called the Valence Shell and the valence shell tends to determine how an element will react

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7
Q

What is a Covalent Compound?

A
  • Compound created when atoms share electrons
  • Normally occurs between two Non-Metals
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8
Q

When an atom gains a charge by losing or gaining electrons it is called an ???

A

ion rather than an atom

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9
Q

Atom

A

Smallest particle in an element. A basic building block of matter

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10
Q

Element

A

A substance made from only one type of atom

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11
Q

Molecules

A

Structures created when atoms combine in chemical reactions. Smallest units of a compound.

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12
Q

Compounds

A

Substances which are created when two or more elements chemically combine. Made up of molecules.

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13
Q

Mixture

A

A substance created when two or more elements are physically mixed but do not chemically combine

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14
Q

Alloy

A

A mixture of at two or more substances, one of which is a metal.

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15
Q

What is an Isotope?

A

Refers to different forms of the same element which are the same aside from the amount of neutrons they have.

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16
Q

What is an Ionic Compound?

A

A compound created when atoms donate electrons to other atoms in such a way that they gain full outer shells. Typically they form between a metal donater and a non-metal reciever. This donating and recieving of electrons causes the atoms to become ionic and have alternate charges, causing them to attract and combine

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17
Q

What are Cations and Anions

A

Cations are positive Ions
Anions are negative Ions

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18
Q

What are Metallic Lattices?

A

One or more metals in a known ratio. In a metallic lattice the metals pool their electrons and share them communally

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19
Q

What are Covalent Lattices?

A

Covalent Bonds between many atoms which create regular, repeating structures

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20
Q

What is Hydroxide

A

A Polyatomic Ion. Chemical Symbol: OH with a charge of -1

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21
Q

What is Nitrate?

A

A Polyatomic Ion. Chemical Symbol: NO3 with a charge of -1

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22
Q

What is Sulfate

A

A Polyatomic Ion. Chemical Symbol:SO4 with a charge of -2

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23
Q

What is Carbonate?

A

A Polyatomic Ion. Chemical Symbol: CO3 with a charge of -2

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24
Q

What is Phosphate?

A

A Polyatomic Ion. Chemical Symbol: PO4 with a charge of -3

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25
Q

What is Ammonium

A

A Polyatomic Ion. Chemical Symbol: NH4 and with a charge of +1

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26
Q

What are Polyatomic Ions

A

Polyatomic Ions are what happens when a group of atoms comes together and that whole group has a charge. Polyatomic Ions can be treated as an individual atom in many chemical equations.

27
Q

What is the Law of Conservation of Mass?

A

The LoCoM states that matter is neither created nor destroyed in a chemical reaction. So when you do a chemical equation, every atom on the LHS should be on the RHS.

28
Q

Why did it take so long for the Law of Conservation of Mass to be discovered?

A

The reason LoCoM took so long to be discovered may be because it is hard to observe. Sometimes atoms may appear to have been destroyed when in reality they reacted and then dissipated away.

29
Q

What is Enthalpy?

A

In increase of decrease in energy

30
Q

Exothermic Reaction

A

A chemical reaction in where the chemical energy, from chemical bonds, of the product is less than the starting energy. The lost energy is dissipated into the surroundings. Exothermic Reactions can be identified as they often emit heat, light or sound

31
Q

Endothermic Reaction

A

A chemical reaction where the chemical energy, from the chemical bonds, of the product is greater than the starting energy. The extra energy is gained from the surrounding environment. Endothermic Reactions can be identified as they typically decrease the heat of their surroundings

32
Q

What is Entropy?

A

A measure of a chemical’s randomness. The universe tends towards instability or spreading out or higher entropy. For example Exothermic reactions are when energy is lost to the environment and so they are the most common reaction as they require less activation energy. Thus the universe tends to a reaction where energy is lost

33
Q

Combustion Reaction

A

Reaction which is characterised by combustion (flame, heat). It is a rapid Exothermic Reaction. The reactants of a Combustion reaction are always O2and a Hydrocarbon and they always produce water and CO2 as their product

34
Q

What is Activation Energy?

A

The minimum amount of extra energy required to initiate a chemical reaction. It can be thought of as a barrier or hump that must be overcome to start the reaction. Activation Energy is why reaction graphs have humps.

35
Q

Properties of Ionic Compounds

A
  • Arrange in lattices where each Ion affects all the ions around them
  • High melting and boiling points. This is linked to the strength of chemical bonds which is strong in ionic bonds
  • Ability to conduct electricity when melted or dissolved in water. This is because the charged particles can flow freely when the compound is in these states
36
Q

Properties of Acids

A

-Acids are substances which donate a proton and most often contain a hydrogen ion, (or proton).
-Sour
-Corrosive
-pH under 7

37
Q

Properties of Bases

A

-Bases are substances which prefer to recieve a proton. They most often contain a hydroxide ion.
-Soapy, Slippery and Bitter
-Caustic (similar to corrosive)
-pH above 7

38
Q

Neutralisation Reactions

A

A reactions between Acids and Bases which counteract each other.
-HA + BOH -> H20 + AB
- Acid + Base -> Water + Salt

39
Q

Precipitation Reactions

A

A type of Double Displacement Reaction. A type of reaction that results in a dissolved solute becoming an insoluble solid.
- Solid is called the precipitate
- Carbonates and Hydroxides are insoluble in water (mostly)
- Nitrate, sodium and chloride salts are soluble (mostly)

40
Q

Antacids

A

Weak bases that counteract excess acid. Typically used to tackle indigestion when the stomach makes too much acids

41
Q

Examples of Bases

A

NaOH, most cleaning products are Bases

42
Q

Examples of Acids

A

HCL - Hydrochloric
H2SO4 - Sulfuric
HNO3 - Nitric
CH3OOH - Ethanoic Acid or Vinegar. (The last hydrogen atom wants to break off so it works independently from the rest of the equation
H3PO4 - Phosphuric Acid

43
Q

Acid + Metal Reactions

A

HA + M -> H2 + MA
Acid + Metal -> Hydrogen Gas + Salt

44
Q

Acid + Carbonate Reaction

A

HA + BCO3 -> CO2 + H2O + AB
Acid + Carbonate -> Carbon Dioxide + Water + Salt
Carbonate is any molecule with the Carbonate polyatomic ion

45
Q

Metal + Water Reactions

A

M + H2O -> H2 + MOH
Metal + Water -> Hydrogen Gas + Strong Base
Here water acts as a weak acid that reacts to form a conjugate strong base.

46
Q

What is the Group and the Period on the Periodic Table

A

Groups are columns. They show number of electrons in outer shell.
Periods are Rows. They show number of shells an atom has

47
Q

What are the Alkali Metals?

A

Generally considered the most reactive elements in the periodic table due to having 1 electron in outer shell. The higher the period the more reactive and unstable the element is.

48
Q

What is the basic Yr10 rule regarding electron arrangements in shells.

A

1st: 2
2nd: 8
3rd: 8
4th: 18
5th: 18
6th: 32

49
Q

What is a solution, solvent and solute?

A

A solution is a substance where dissolved solute is distributed equally in another substance called a solvent

50
Q

What is an aqueous solution?

A

A solution where the solvent is water

51
Q

OIL RIG

A

Oxidation Is Loss, Reduction Is Gain

52
Q

What are RedOx Reactions

A

A RedOx reaction is also called a Reduction-Oxidation reaction and it is any reaction that involves the transfer of electrons.
It is really two simultaneous reactions, Oxidation: the loss of electrons and Reduction: a gain in electrons.

53
Q

What is an Oxidiser

A

A substance which causes another substance to undergo Oxidation.

54
Q

What is a reducer (reducing agent)

A

A substance which causes another substance to undergo reduction

55
Q

What are Oxidation States?

A
  • When an atom is charged it is said to have an oxidation state.
  • Generally the oxidation state is equal to the charge
56
Q

Explain Decomposition Reactions and include examples

A

A reaction where a heavy substance decomposes into two lighter substances. These are endothermic reactions.
General Form: AB = A + B
Example: CuCO3 = CuO + CO2

57
Q

Explain Synthesis Reactions and Include Examples

A

A reaction where two substances react to form a heavier compound. Exothermic reaction.
General Form: A + B = AB
Example: H2 + O2 = H20

58
Q

Explain Single Displacement Reactions with Examples

A

A type of RedOx reaction where a more reactive metal displaces a less reactive metal and takes its place in a compound
General Form: AB + C = CB + A
Example: Cu + AgNO3 = Ag + Cu(NO3)2

59
Q

Explain Double Displacement Reactions with Examples

A

A reaction where the metals in two ionic compounds swap places.
General Form: AB + CD = AD + CB
Example: NaCl + AgNO3 = NaNO3 + AgCl

60
Q

Explain Corrosion Reactions with examples

A

A chemical reaction that results in the wearing away of metal due to the combination of that metal with oxygen.
A type of RedOx and Synthesis Reaction
Example: Zn + O2 = ZnO

61
Q

What is Radioactive Decay?

A

When the nucleus of an atom breaks down. This causes the emission of radiation and results in the element becoming another more stable element

62
Q

What is an Alkali?

A

A Base which is dissolved in water

63
Q

What are all the Diatomic Elements?

A

Hydrogen
Nitrogen
Oxygen
Fluorine
Bromine
Chlorine
and Iodine

64
Q

What are the only Transition Metals with fixed Charges

A

Zn (Zinc) = +2
Cd (Cadmium) = +2
Ag (Silver) = +1

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