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Chemistry Module 2 > Chemistry Module 2 - Chapter 2 > Flashcards

Chemistry Module 2 - Chapter 2 Flashcards

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1
Q

What was stated in Dalton’s atomic theory? (4)

A
  1. Atoms are tiny particles made of elements.
  2. Atoms cannot be divided.
  3. All the atoms in a element are the same.
  4. Atoms of one element are different to those of other elements.
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2
Q

What did Thompson discover about electrons? (3)

A
  1. They have a negative charge.
  2. They can be deflected by magnets and electric fields.
  3. 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 moving around in a sea of positive charge.

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4
Q

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

A
  1. Most of the mass and positive charge of the atom are in the nucleus.
  2. Electrons orbit the nucleus.
  3. Most of the atom’s volume is the space between the nucleus and the electrons.
  4. Overall positive and negative charges must balance.
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5
Q

Explain the current model of the atom. (5)

A
  1. Protons and neutrons are found in the nucleus.
  2. Electrons orbit in shells.
  3. Nucleus is tiny compared to the total volume of atom.
  4. Most of atom’s mass is in the nucleus.
  5. Most of the atom is empty space between the nucleus and the electrons.
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6
Q

What is the charge of the proton?

A

1+

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7
Q

What is the charge of the electron?

A

1-

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8
Q

What is the charge of the neutron?

A

0

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9
Q

What is the relative mass of the proton?

A

1

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10
Q

What is the relative mass of the neutron?

A

1

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11
Q

What is the relative mass of the electron?

A

1/1840

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12
Q

What two particles make up most of the atom’s mass?

A

Protons + Neutrons

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13
Q

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

A

Z

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14
Q

What does the atomic number tell about an element?

A

Atomic number = number of protons in an atom.

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15
Q

What letter represents the mass number?

A

A

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16
Q

How is the mass number calculated?

A

Mass Number = number of protons + number of neutrons

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17
Q

How do you calculate the number of neutrons?

A

Number of neutrons = Mass number - Atomic Number

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18
Q

Define istope

A

Different forms of the same elements, with the same number of protons but a different number of neutrons.

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19
Q

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

A
  1. Neutrons have no impact on the chemical reactivity.
  2. Reactions involve electrons, isotopes have the same number of electrons in the same arrangement.
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20
Q

What are ions?

A

Charged particles that is formed when an atom loses of gains electrons.

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21
Q

What is the charge of the ion when electrons are gained or lost?

A

Gained = negative
Lost = positive

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22
Q

What are positive and negative ions called?

A

Positive ions = cations

Negative ions = anions

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23
Q

What is the unit used to measure atomic masses called?

A

Unified atomic mass unit = u

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24
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.

25
Q

What is the unit of relative atomic mass?

A

No units.

26
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.

27
Q

The relative isotopic mass is the same as which number?

A

Mass number.

28
Q

What two assumptions are made when calculating mass number?

A
  1. Contribution of the electron is neglected.
  2. Mass of both proton and neutron is taken as 1.0u.
29
Q

How do you calculate the relative molecular mass and relative formula mass?

A

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

30
Q

What are the uses of mass spectrometry? (3)

A
  1. Identify unknown compounds.
  2. Find the relative abundance of each isotope of an element.
  3. Determine structural information.
31
Q

How does a mass spectrometer work?

A
  1. The sample is vapourised and then ionised to form positive ions.
  2. They pass through the apparatus and are separated according to mass-to-charge ratio.
  3. A computer analyses the data and produces a mass spectrum.
32
Q

How do you calculate the mass-to-charge ratio? (m/z)

A

Relative mass of ion ÷ relative charge on ion

33
Q

How do you calculate the relative atomic mass?

A

sum of (isotope abundance x isotope mass) ÷ sum of all isotope abundances

34
Q

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

A

Group number = number of electrons in the outer shell.

35
Q

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

A

Vertical column.

36
Q
  1. Do metals usually gain or lose electrons?
  2. Do non-metals usually gain or lose electrons?
A
  1. Lose electrons
  2. Gain electrons.
37
Q

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

A

The elements are beryllium, boron, carbon and silicon.

Requires a lot of energy to transfer outer shell electrons.

38
Q

What are molecular ions?

A

Covalently bonded atoms that lose or gain electrons.

39
Q

How can you Predict Ionic Charges from the Positions of Elements in the Periodic Table?

A

Group 1 = 1+ (lose 1 electron).
Group 2 = 2+ (lose 2 electrons).
Group 3 = 3+ (lose 3 electrons).
Group 4 = Be, B, C & Si tend not to form ions, as it requires a lot of energy to transfer outer shell electrons.
Group 5 = 3- (gain 3 electrons).
Group 6 = 2- (gain 2 electrons).
Group 7 = 1- (gain 1 electron).

40
Q

What is the charge of the ammonium ion?

A

+1 = NH4(+)

41
Q

What is the charge of the nitrite ion?

A

1- = NO2(-)

42
Q

What is the charge of a hydrogencarbonate?

A

-1 = HCO3(-)

43
Q

What is the charge of manganate (VII) / permanganate?

A

-1 = MnO4(-)

44
Q

What is the charge of dichromate (VI)?

A

2- = Cr2O7(2-)

45
Q

What is the charge of a phosphate ion?

A

3- = PO4(3-)

46
Q

What is the charge of a hydroxide ion?

A

-1 = OH(-)

47
Q

What is the charge of a nitrate ion?

A

-1 = NO3(-)

48
Q

What is the charge of a carbonate ion?

A

-2 = CO3(2-)

49
Q

What is the charge of a sulphate ion?

A

-2 = SO4(2-)

50
Q

What is the charge of a zinc ion?

A

2+ = Zn(2+)

51
Q

What is the charge of a silver ion?

A

1+ = Ag(+)

52
Q

What ions does copper form?

A

Copper (I) = Cu(+)
Copper (II) = Cu(2+)

53
Q

What ions does iron form?

A

Iron (II) = Fe(2+)
Iron (III) = Fe(3+)

54
Q

What is a binary compound? How do you name them?

A

A binary compound contains two elements.
1. To name a binary compound, use the name of the element that change the ending of the second element’s name to -ide.
2. For ionic compounds, the metal ion always comes first.

55
Q

What are polyatomic ions?

A

Sometimes, an ion may contain atoms of more than one element bonded together. These ions are called polyatomic ions.

56
Q

What is the empirical formula?

A

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

57
Q

How do you calculate the empirical formula?

A
  1. Divide the amount of each element by its molar mass.
  2. Divide the answers by the smallest value obtained.
  3. If there is a decimal, divide by a suitable number to make it into a whole number.
58
Q

What are the four state symbols?

A

(g) - gas
(l) - liquid
(s) - solid
(aq) - dissolved in water (aqueous)

Chemistry Module 2 (4 decks)

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