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CHEMISTRY TOPIC 1 GENERAL > ATOMIC STRUCTURE & THE PERIODIC TABLE > Flashcards

ATOMIC STRUCTURE & THE PERIODIC TABLE Flashcards

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1
Q

What is the relative mass, charge and position is the atom of a proton?

A

1, +1, nucleus

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2
Q

What is the relative mass, charge and position is the atom of a neutron?

A

1, 0, nucleus

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3
Q

What is the relative mass, charge and position is the atom of an electron?

A

1/1840, -1, energy level/orbitals

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4
Q

Atomic number = ?

A

Number of protons (=number of electrons)

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5
Q

Mass number = ?

A

Number of protons + number of neutrons

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6
Q

What is an isotope?

A

Atoms of the same element with a different amount of neutrons (different masses).

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7
Q

What is the relative atomic mass of an atom?

A

The weighted mean mass of an atom of the element compared to 1/12 the mass of an atom of carbon-12, which has a mass of 12

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8
Q

What is the relative isotopic mass?

A

The mass of an atom of an isotope of the element compared to 1/12 the mass of an atom of carbon-12, which has a mass of 12.

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9
Q

What does a mass spectrometer do?

A

Measures the masses of atoms and molecules.

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10
Q

How does a mass spectrometer measure the masses of atoms and molecules?

A

-Produces positive ions that are deflected by a magnetic field. According to the mass-to-charge ratio.

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11
Q

What is the molecular ion peak?

A

The peak with the highest m/z ratio in the mass spectrum.

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12
Q

What is a quantum shell?

A

A quantum shell defines the energy level of an electron.

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13
Q

What is the electronic configuration of an atom?

A

It shows the number of electrons in each sub-level in each energy level of the atom.

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14
Q

What is Hund’s rule?

A

It states that electrons will occupy the orbitals singly before pairing takes place.

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15
Q

What is the Pauli exclusion theory?

A

It states that two electrons cannot occupy the same orbital unless they have opposite spins.

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16
Q

How is electron spin usually shown?

A

By an up or down arrow.

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17
Q

What is an orbital?

A

A region within an atom that can hold up to two electrons with opposite spins

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18
Q

How many electrons can an s sub-shell hold?

A

2

19
Q

How many electrons can a p sub-shell hold?

A

6

20
Q

How many electrons can a d sub-shell hold?

A

10

21
Q

How many electrons can an f sub-shell hold?

A

14

22
Q

What is the first ionisation energy?

A

The energy required to remove an electron from each atom in one mole of atoms in the gaseous state.

23
Q

What is the second ionisation energy?

A

The energy required to remove an electron from each singly charged positive ion in one mole of positive ions in the gaseous state.

24
Q

We can represent the first ionisation energy of an element, A, by the equation…

A

A(g) → A⁺(g) + e⁻

25
Q

We can represent the second ionisation energy of an element, A, by the equation…

A

A⁺(g) → A²⁺(g) + e⁻

26
Q

Ionisation energy (IE) = …

A

energy of electron when removed - energy of electron when in the orbital.

27
Q

The vertical columns in the Periodic Table are called…

A

groups.

28
Q

The horizontal columns in the Periodic Table are called…

A

periods.

29
Q

The periodic table is divided into…

A

blocks.

30
Q

The s-blocks consists of…

A

elements in group 1 and 2.

31
Q

The p-block consists of…

A

elements in group 3-8.

32
Q

The d-block consists of…

A

elements scandium to zinc, one in which the d subshell is being filled.

33
Q

The factors that affect the energy of an electron has are…

A
  • The orbital the electron exists in
  • The nuclear charge of the atom(number of protons)
  • The repulsion(shielding) experienced by the electron from the other electrons.
34
Q

What is the general trend in ionisation energy across a period?

A
  • The nuclear charge increases as the number of protons increases. This, on its own, would lead to an increase in attraction between the nucleus and the electron, and therefore a decrease in the energy of the outermost electron, and an increase in the first ionisation energy.
  • To counteract this, 1 electron is added to the same quantum shell on each occasion and this increases the electron-electron repulsion within the quantum shell. This, one its own, would cause an increase in energy of the outermost electron, and would lead to a decrease in the first ionisation energy.
  • However, the increase in nuclear charge is more significant than the repulsion. So there is a general increase.
35
Q

What is the trend in ionisation energy down a group?

A
  • As you descend, the nuclear charge increases as the number of protons increases. This increases the attraction between the nucleus and the electron, and therefore a decrease in energy of the outer electron. This in turn would increase the ionisation energy.
  • However, one new quantum shell is added on each occasion. This increases the energy of the outermost electron, as the 3rd quantum shell has a higher energy value than the 2nd and more shielding is experienced.
  • On this occasion, the extra shell and more shielding is more significant than the nuclear charge, so the ionisation energy decreases.
36
Q

What groups doesn’t have a trend in ionisation energy?

A

3.

37
Q

What is the anomaly in group 4?

A

Lead is the anomaly because the first ionisation energy that is higher than that of tin, the element above.

38
Q

What is periodicity?

A

A regular repeating pattern of atomic, physical and chemical properties with increasing atomic number.

39
Q

What is atomic radii?

A

A measure of the size of its atoms. It is the distance from the centre of the nucleus to the boundary of the electron cloud.

40
Q

How do you find the atomic radius?

A

Since an atom has a well-defined boundary, we can find the atomic radius by determining the distance between the two nuclei and dividing it by two.

41
Q

Which is a larger radius covalent radius or van der Waals?

A

van der Waals.

42
Q

What does a van der Waals and covalent radius look like?

A

Atoms are just touching whereas with covalent radius they are closer.

43
Q

What is the trend in the radius across each period?

A

The radius decreases. This is because as the number of protons in the nucleus increases, so does the nuclear charge. This results in an increase in the attractive force between the nucleus and the outer electrons. This increase in attractive force offsets the increase in repulsion as the number of the electrons in the outer shell increases.

CHEMISTRY TOPIC 1 GENERAL (1 decks)

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