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Chemistry > foundations in chem 2.1.1 & 2.1.2 > Flashcards

foundations in chem 2.1.1 & 2.1.2 Flashcards

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1
Q

what was stated in Dalton’s atomic theory

A
  • Atoms are tiny particles made of elements
  • atoms cannot be divided
  • all atoms in an element are the same
  • Atoms of one element are different to those of a different element
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2
Q

What did Thompson discover about electrons?

A

They have a negative charge.
They can be deflected by a magnet and an electric field.
They have a very small mass

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3
Q

Explain the plum pudding model?

A

Atoms are made up of negative electrons floating around in a sea of positive charge.

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4
Q

What were Rutherford’s proposal after the gold leaf experiment?

A

Most of the mass and positive charge of the atom was in the nucleus
Electrons orbit the nucleus
Most of the atoms volume is in the space between the nucleus and the electrons
Overall positive and negative charges must balance.

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5
Q

Explain the current model of the atom?

A

Protons and neutrons are found in the nucleus.
Electrons orbit in shells
Nucleus is tiny compared to the total volume of an atom
Most of the atoms mass is in the centre nucleus
Most of the atom is empty space between the nucleus and the electrons

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6
Q

What is the charge of a proton ?

A

+1

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7
Q

what is the charge of an electron?

A

-1

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8
Q

What particle has the same mass as a proton?

A

neutron

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9
Q

Which two particle make up most of an atoms mass?

A

proton, neutron

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10
Q

Which letter is used to represent the atomic number of an atom?

A

Z

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11
Q

What does the atomic number tell us about the element?

A

Atomic number = Number of protons in an atom

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12
Q

Which letter represents the mass number?

A

A

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13
Q

How is mass number calculated?

A

number of protons + number of neutrons

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14
Q

How do you calculate number of neutrons?

A

mass number - atomic number

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15
Q

Define isotope

A

Atoms of the same element but with a different number of nuetrons

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16
Q

Why do the different isotopes of the same element react in the same way?

A

Neutrons have no impact on the chemical reactivity
Reactions involve electrons and isotopes have the same number of electrons in the same arrangement

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17
Q

What are ions?

A

Charged particles that are formed when an atom looses or gains electrons

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18
Q

what is the charge of an ion when the particle gains an electrons?

A

negative
anion

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19
Q

What is the unit used to measure atomic mass called?

A

Unified atomic mass unit (U)

20
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared with one twelfth of the mass of an atom of carbon 12

21
Q

Units of relative atomic mass?

A

No units

22
Q

Define relative isotopic mass?

A

The mass of an atom of an isotope compared with one twelfth of the mass of an atom of Carbon 12

23
Q

The relative isotopic mass is the same as which number

A

mass number

24
Q

What two assumptions are made when calculating mass number?

A

Contribution of the electron is neglected
Mass of both proton and neutron is taken as 1.0 U

25
Q

How to calculate the relative molecular mass and regular formula mass?

A

Both can be calculated by adding the relative atomic masses of each of the atom making up the molecule or formula

26
Q

What are the uses of mass spectrometry?

A

Identify unknown compounds
Find relative abundance of each isotope in an element of an element
Determine structural information

27
Q

How does a mass spectrometer work?

A

The sample is made into positive ions
They pass through apparatus and are separated according to mass to charge ratio
A computer analyses the data and produces a mass spectrum

28
Q

How is the group number related to the number of electrons?

A

group number = the number of electrons on the outer shell

29
Q

Does the group number indicates horizontal or vertical column in the periodic table?

A

Vertical column

30
Q

Do metals usually gain or loose electrons?

A

loose electrons

31
Q

What are the 4 elements that don’t tend to form ions and why?

A

buryllium , boron, carbon , silicon
requires a lot of energy to transfer outer shell electrons

32
Q

what are molecular ions?

A

covalently bonded ions atoms that loose or gain electrons

33
Q

What is the charge of a ammonium -ion

A

NH4+

34
Q

Hydroxide ion??

A

OH/-

35
Q

Nitrate ion ?

A

NO/3-

36
Q

Carbonate ion ?

A

CO3/2-

37
Q

Sulfate ion?

A

SO4/2-

38
Q

What is an empirical formula?

A

Simplest whole number ratio of atoms of each element present in a compound

39
Q

How do you calculate empirical formula?

A

Divide the amount of each element by its molar mass
Divide the answers by the smallest answers obtained
If it is a decimal then divide by a suitable number to make it into a whole number

40
Q

phosphate ion

A

PO4 charge = 3-

41
Q

Nitride ion

A

N charge 3-

42
Q

Ammonium

A

NH4 charge +1

43
Q

dichromate

A

Cr2O7 charge 2-

44
Q

what are the names of some acids?

A

hydrochloric HCl
nitric acid = HNO3
sulphuric acid = H2SO4
ethanoic acid CH3COOH = weak acid so
double arrow

45
Q

What are the names of some Bases?

A

carbonates = K2CO3
hydrogen carbonates = NaHCO3
metal oxides = MgO
metal hydroxides = NaOH
Ammonia = NH3

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