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Atoms, Ions and Compounds > Atomic Structure and Isotopes > Flashcards

Atomic Structure and Isotopes Flashcards

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Organic Chemistry 101 flashcards
1
Q

What is an isotope?

A

An atom with the same number of protons (of the same element) but a different number of neutrons

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2
Q

What is the formula of a sulfate?

A

SO4

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3
Q

What is the formula of a nitrate?

A

(NO3)

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4
Q

What is the formula of a hydroxide?

A

(OH)

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5
Q

Give the definition of relative atomic mass

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon 12

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6
Q

Give the definition of the relative isotopic mass

A

The mass of an isotope relative to 1/12 of the mass of an atom of carbon 12

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7
Q

What is avogadros constant?

A

6.02 x 1023

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8
Q

How do you calculate the numbers that will be in the empirical formula

A
  1. You find the moles of each of the atoms in the element
  2. Divide each of the moles by the smallest moles
  3. That will give you the ratio
  4. Use this to write the empirical formula
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9
Q

The little numbers in the empirical formula of a compound must always be [blank]

fill in the blank

A

The little numbers in the empirical formula of a compound must aways be whole numbers

!!! so if you get a decimal number ending in .5 DOUBLE EVERYTHING, and if its a decimal that can easily be rounded ROUND IT NOWWWWW

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10
Q

Which type of structure is written using empirical formula?

A

GIANT STRUCTURES (Covalent AND Ionic)

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11
Q

Which type of structure is written using molecular formula?

A

Simple/small covalent bonds

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12
Q

How do you calculate the molecular formula?

A
  1. Calculate the empirical formula of the compound
  2. Calculate the Mr of the compound using this empirical formula
  3. Divide the given relative molecular molar mass by the Mr (molar mass) of the empirical formula
  4. Multiply the quotient by the Mr of the empirical formula
  5. Et voila! you have your molecular formular
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13
Q

How do you use the empirical formula to calculate the molecuar formula?

A
  1. You divide the given relative molecular Mr by the Mr of the compound which is found using the empirical formula
  2. Then multiply each subscript in the empirical formula by this quotient to find the molecular formula
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14
Q

What is Avogadro’s LAW

not constant but his LAW

A

In room temperature and pressure, one mole of gas occupies 24 dm3

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15
Q

In what conditions does Avogadro’s LAW not work

A

When it is not room temperature and pressure

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16
Q

What is the equation for Avogadro’s Law?

A

moles of GAS= volume/24dm3
or
volume= moles of GAS x 24dm3

or 24000cm3 bc that equals 24dm3

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17
Q

What is the equation for ideal gas

A

pV=nRT

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18
Q

What does p stand for in the ideal gas equation?

A

Pressure

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19
Q

What are the units of pressure in the ideal gas equation?

A

Pa, Pascals

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20
Q

How many Pascals in 1 Atmosphere?

A

101325 Pascals

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21
Q

How many atmospheres in 101325 Pascals?

A

1 Atmosphere

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22
Q

What does the V stand for in the ideal gas equation?

A

Volume

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23
Q

What is the unit for volume in the ideal gas equation

A

1 metre3

24
Q

How many dm3 in 1m3?

A

1000 dm3

25
Q

What does the n stand for in the ideal gas equation?

A

Moles

26
Q

What does R stand for in the ideal gas equation?

A

Gas constant

27
Q

What is the Gas constant

a number

A

8.314

28
Q

What does the T stand for in the ideal gas equation?

A

Temperature

29
Q

What are the units for temperature in the ideal gas equation?

A

K, Kelvin

30
Q

How many Kelvin in 0 degrees Celcius?

A

273 Kelvin

31
Q

How do you convert from degrees Celcius to Kelvin?

A

Add 273

32
Q

What is the symbol for ammonia?

A

NH3

33
Q

What is the symbol for sulfuric acid?

A

H2SO4

34
Q

Give the definition of a salt

A

When the H+ ion in an acid is replaced by a metal ion

35
Q

How do you identify what the base is in a neutralisation reaction?

A

It accepts H+ ions

36
Q

What is a base?

A

Chemicals that neutralise acids producing salt and water

37
Q

What does the large dot in a hydrated salt formula show?

A

It shows that the water molecules are bound up in the ionic lattice

38
Q

How do you calculate the formula of a hydrated salt?

A
  1. Work out the moles of the salt and the water
  2. Divide both of the moles by the smallest one
  3. You then use this to show the whole number ratio

if its .5, double everything, if its a roundable number, round itttt!

39
Q

What is the definition of percentage uncertainty?

A

The uncertainty in your measurements expressed as a percentage of the results

40
Q

What is the equation to calculate percentage uncertainty?

A

(total uncertanty/result) x 100

41
Q

What is the units for moles in the m=cxv equation?

A

dm3

1dm3</sup=1000cm3

42
Q

What are units for concentration in the m=c x v equation?

A

M or moles/dm3

43
Q

How many mL in 1cm3

A

1mL=1cm<sup.3</sup>

44
Q

What do you calculate when you asked to find the volume of a subtance at room temperature and pressure?

A

Mole x 24dm3

or 24000cm3

45
Q

Give the definition of empirial formula

A

The simplest whole number ratio of atoms/moles/elements

46
Q

Name four common cations and anions

A

1.Ammonium
2.Nitrate
3.Sulphate
4.Phostphate

47
Q

Give the equation for ammonium

A

NH4+

cation

48
Q

Give the equation for nitrate

A

NO3-

Anion

49
Q

Give the equation for sulphate

A

SO42-

Anion

50
Q

What is an alkali?

A

A soluble base which releases OH-

51
Q

How do you use the total Mr to find the formula of a compound

A

Using the iterative method
1. Identify which atoms are in the compound
2. Subtract the first one’s Mr by the total calculated Mr
3. Then divide this answer by the second atom’s Mr
4. If the number is a whole number then that is the number of the second atom there is in the compound and the first number is just what you multiplied the Mr of the first atom with.
5. It is iteratie because you just try this with ascending multiples of the 1st atoms Mr, until you get a whole number when you divide that answer by the 2nd number’s Mr

lol its very long

52
Q

Give the equation for a phosphate

A

PO43

53
Q

Give an example of an alkali

A

OH-

54
Q

Give an example of an acid

A

H+

55
Q

Metal + acid -> [blank] + [blank]

fill in the blank

A

Metal + acid -> salt + hydrogen

56
Q
A

Atoms, Ions and Compounds (2 decks)

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