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Chemistry Year 13 > 1.1- Formulas, Equations and Amounts of Substance > Flashcards

1.1- Formulas, Equations and Amounts of Substance Flashcards

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1
Q

Element definition

A

A substance that consists of only one type of atom and cannot be broken down into anything simpler by chemical means

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2
Q

Compound definition

A

A substance that consists of two or more elements chemically combined

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3
Q

Mixture definition

A

Consists of two or more substances that are easy to separate

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4
Q

Molecule definition

A

Is the particle that consists of two or more atoms chemically bonded together (The atoms can be the same or different)

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5
Q

Diatomic molecules definition

A

Means that there are two atoms covalently bonded in a molecule e.g Hydrogen, oxygen, bromine and iodine

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6
Q

Molecular ion definition

A

Two or more atoms covalently bonded with an overall charge

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7
Q

Monatomic definition

A

Consists of 1 atom e.g noble gases

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8
Q

Isotope definition

A

Atoms which have the same atomic number but a different mass number (contain the same number of protons but a different number of neutrons)

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9
Q

Atomic number

A

The number of protons in the nucleus of an atom

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10
Q

Mass number definition

A

The total number of protons and neutrons in the nucleus of an atom

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11
Q

Allotropes definition

A

Are different forms of the same element in the same physical state e.g graphite and diamond

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12
Q

Melting point definition

A

Is the temperature at which a solid changed to a liquid

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13
Q

Boiling point definition

A

The temperature at which a liquid is changed to a gas

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14
Q

Sublimation definition

A

Is the direct charge from a solid to a gas

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15
Q

Mole definition

A

The amount of substance which contains the avogadro constant of atoms, molecules or groups of ions

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16
Q

Molar mass definition

A

The mass of one mole of a substance

17
Q

RAM definition

A

The average (weighed mean) mass of an atom of an element relative to one twelfth of the mass of an atoms of carbon 12

18
Q

Relative molecular mass (RMM) definition

A

The average (weighed mean) mass of a molecule relative to one twelfth of the mass of an atom of carbon 12

19
Q

RFM definition

A

The average (weighed mean) mass of a formula unit relative to one twelfth of the mass of an atom of carbon 12

20
Q

RIM (relative isotopic mass) definition

A

The mass of an atom of an isotope of an element relative to one twelfth of the mass of an atom of carbon 12

21
Q

When naming non-metal compounds the element in each compounds can be described by using a ______ such as…. (1-6)

A

Prefix
Mon= 1 e.g CO Carbon MONoxide
Di=2
Tri= 3 e.g BF3 boron TRIfluoride
Tetra=4
Penta=5
Hexa=6

22
Q

If a substance IS soluble ___ is used
If a substance IS INsoluble then __ is used

A

(aq)
(S)

23
Q

What substances are soluble (aq)

A
  • ALL SODIUM, POTASSIUM AND AMMONIUM SALTS

-ALL NITRATES

-MOST CHLORIDES, BROMIDES AND IODIDES EXCEPT SILVER AND LEAD CHLORIDES, BROMIDES AND IODIDES

-MOST SULFATES EXCEPT LEAD AND BARIUM SULFATES. CALCIUM SULFATE IS SLIGHTLY SOLUBLE

24
Q

What substances are soluble (aq)

A
  • ALL SODIUM, POTASSIUM AND AMMONIUM SALTS

-ALL NITRATES

-MOST CHLORIDES, BROMIDES AND IODIDES EXCEPT SILVER AND LEAD CHLORIDES, BROMIDES AND IODIDES

-MOST SULFATES EXCEPT LEAD AND BARIUM SULFATES. CALCIUM SULFATE IS SLIGHTLY SOLUBLE

25
Q

insoluble substances (used solid state symbol)

A

-MOST CARBONATES EXCEPT SODIUM, POTASSIUM AND AMMONIUM CARBONATES

-MOST HYDROXIDES EXCEPT SODIUM, POTASSIUM AND AMMONIUM HYDROXIDES

-MOST OXIDES EXCEPT SODIUM, POTASSIUM AND CALCIUM OXIDES WHICH REACT WITH WATER

26
Q

Steps to doing ionic equations

A

Step 1: Write down word equation
Step 2: Balance the symbol equation
Step 3: Split ionic compounds (aqueous) into ions [see soluble and insoluble rules]
Step 4: Remove same ions that repeat on each side of the equation
Step 5: rewrite with remaining ions and elements

27
Q

With ionic equations as well as balancing the elements it is necessary to balance the ________

A

Charges

28
Q

Molar mass definition

A

Is the mass of one mole of a substance

(One mole of any substance contain 6.02 x 10 to the power of 23 particles known as Avogadro constant)

29
Q

Avogadro constant definition

A

Number of atoms in 12.000g of carbon 12

(6.02 x 10 to the power of 23)

30
Q

Avogadro’s number triangle

A

The number of particles= number of moles x Avogadro’s constant

31
Q

Example question: How many ions are there in 2 mol of magnesium sulfate?

A

-Mg2+ and SO4 to the power of 2- are the two ions

Therefore the number of ions /particles = moles x Avo constant

2x2x6.02x (10 to the power of 23)

32
Q

When given the masses of both reactants you need to work out which one is the limiting reactant, so what is the steps?

A

1.) using what is provided in the question, figure out the moles of each reactant
2.) Figure out which one is limiting by which ever is the smallest amount of moles, ensure to check the number in front of reactant in the question as you will need to divide the moles by the number in front
3.) Whatever is the smallest reactant’s moles you should use it to figure out the missing mass of the products (remember to multiply or divide the moles according to the number in front of the products)

33
Q

Anhydrous salt definition

A

A salt which contains no water of crystallisation

34
Q

Hydrated salt definition

A

A salt which contains water of crystallisation

35
Q

Water of crystallisation definition

A

Water chemically bonded within a crystal structure

36
Q

% of water equations

A

% of water= number in front of water x 18 divided by total rfm (including 18 x number in front of water) x100

37
Q

How to work out formulae of hydrated salt (find x)

A

1.) find 2 masses, the anhydrous salt and the mass of water which is found by hydrated salt - anhydrous salt). The masses can also be found through percentage 51%=51g if you had 100g of the substance
2.) calculate the moles of each
3.) divide by the smallest moles to produce ratio

38
Q

Density equation

A

D= mass divided by volume

Chemistry Year 13 (10 decks)

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