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Chemistry 11 Chapter 1 > All > Flashcards

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1
Q

Explain Thomson’s model of the atom.

A

Thomson’s model or the “plum pudding” model consisted of a positively charged sphere, with negatively charged particles (later called electrons) embedded in it.

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2
Q

Explain Rutherford’s model of the atom.

A

Rutherford’s model or the planetary model had planet-like electrons orbiting a positively charged nucleus. The nucleus contained most of the mass of the atom.

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3
Q

Explain Rutherford’s gold foil experiment.

A

He directed highly energetic, positively charged alpha particles at very thin gold foil. He traced the paths of the alpha particles after they collided with the gold foil. After math calculations, he showed that the only configuration that could explain the path of the alpha particles was the idea that all the positive charge and nearly all mass is located in the centre.

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4
Q

Explain Bohr’s model of the atom

A

Bohr’s model was very similar to Rutherford’s except that he found that electrons can have only specific amounts of energy. These energy levels are called electron shells.

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5
Q

What was the limitation to Bohr’s model?

A

The limitation was that as the electron goes around the nucleus, it would lose energy and eventually collapse into the nucleus, but we can see that items simply don’t collapse into each other. It is somehow able to sustain its energy .

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6
Q

What was Chadwick’s contribution to the atomic model?

A

His contribution was the discovery of neutrons (neutrally charged particles). He bombarded beryllium atoms with alpha particles and found that the atom is mostly empty space with a tiny dense central nucleus. He found that the mass of 1 neutron = mass of 1 proton

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7
Q

What is the Quantum model of the atom.

A

Introduction of sub levels called orbitals which are found only in Quantum Theory.

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8
Q

How many electrons can each orbital accommodate, why and what is this principle called?

A

Each orbital can accommodate 2 electrons because they can only spin 2 ways. Clockwise and counter clockwise. This principle is called Pauli’s exclusion principle.

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9
Q

What did Schrödinger add to the atomic model?

A

He showed that electrons do not travel in precise orbits but instead exist in defined regions of space. Electrons in each energy level are confined to specific regions of space, represented by electron clouds. Usually called the electron cloud model.

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10
Q

What are isotopes?

A

Atoms that have the same number of protons but different numbers of neutrons. Ex. A hydrogen atom can have 0, 1, or 2 neutrons

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11
Q

What are radioisotopes?

A

Isotopes with unstable nuclei that decay into different often stable, isotopes. A stable isotope will have a correct balance between protons and neutrons which this stabilizes the nucleus.

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12
Q

What is the periodic law?

A

When elements are arranged by atomic number, their chemical and physical properties recur periodically

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13
Q

Name some properties of alkali metals

A
  • highly reactive

- Group 1 elements

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14
Q

Name some properties of alkaline earth metals

A
  • are reactive but less so than alkaline earth metals

- Group 2 elements

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15
Q

What are some properties of transition metals?

A
  • Very hard metals
  • High melting point
  • Because of complex electron config, they can form a wide variety of compounds with other elements
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16
Q

What are some properties of other metals?

A
  • not as reactive as group 1 and 2 elements

- Common and useful

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17
Q

What are some properties of metalloids?

A
  • have properties between those of metals and non-metals
  • shiny solids
  • poor conductors of the electric current
  • brittle
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18
Q

What are some properties of other non-metals?

A
  • non-metals that are not halogens or noble gases
  • Not as reactive as halogens or as unreactive as noble gases
  • common elements in tissues of living organisms
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19
Q

What are some properties of halogens?

A

-reactive non-metals

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20
Q

What are some properties of noble gases?

A
  • extremely unreactive

- do not undergo any naturally occurring reactions

21
Q

What are some properties of lanthanoids?

A
  • rare earth elements

- used in advanced batteries for hybrid cars

22
Q

What are some properties of actinoids?

A
  • Have no stable isotopes, so they are all radioisotopes

- elements beyond uranium cannot occur naturally

23
Q

Compare reactivity between metals and non-metals

A

Metals become more reactive as you go DOWN a group and go LEFT a period

Non-metals become more reactive UP a group and RIGHT a period

24
Q

Compare melting and boiling points between metals and non-metals?

A

For metals, boiling point decreases down a group

For non-metals, boiling point increases down a group

25
Q

What is the periodic trend of atomic radius?

A

The periodic trend of atomic radius is that the radius gets smaller ACROSS a period and LARGER down a group

26
Q

Define atomic radius

A

The distance from the centre of an atom to the boundary within which the electrons spend 90% of their time

27
Q

What is the trend for ionizing energy?

A

The trend is that the ionizing energy INCREASES across the period and DECREASES down a group

28
Q

Define ionizing energy.

A

The amount of energy required to remove the outermost electron from an atom

29
Q

What is the trend for electron affinity?

A

The trend is that electron affinity INCREASES across the period and DECREASES down the group

30
Q

Define electron affinity

A

The energy absorbed or released when an electron is added to a neutral atom

31
Q

What is the trend in electron negativity?

A

The trend is that electron negativity INCREASES across a period and DECREASES down a group.

32
Q

Define electron negativity.

A

The indicator of the relative ability of an atom to attract shared electrons

33
Q

What is the trend in melting and boiling points?

A

Melting point decreases down the group

34
Q

What is the trend in hardness across the periodic table?

A

The trend is that hardness decreases down the group.

Hardness is mainly for metals

35
Q

Why does the trend of atomic radius occur across a period?

A

Atomic radius DECREASES across a period. This is because the number of positives charges increases, meaning the attractive force on each electron becomes stronger. The stronger the force, the closer the electrons are drawn to the nucleus, thus making the atom smaller

36
Q

Why does the trend of atomic radius occur down a group?

A

Atomic radius DECREASES across a period and INCREASES down a group. This is because as you go down the group, the number of occupied electron shells increases. The filled inner shells shield the outer electrons from the positive charge of the nucleus. Because of this shielding, the effective nuclear charge appears smaller than the actual charge in the nucleus. Making the atom appear bigger.

37
Q

Define effective nuclear charge

A

The apparent nuclear charge, as experienced by the outermost electrons of an atom, as a result of the shielding by the inner-shell electrons

38
Q

Why does the trend of ionization energy occur across a period?

A

Ionization energy INCREASES across a period and DECREASES down a group. This is because as you move across a period, the number of protons ,and electrons in the valance she’ll increases. The more filled the shell, the more stable it is. The more stable the outer shell is, the more energy is needed to remove an electron

39
Q

Why does the trend of ionization energy occur down a group?

A

Ionization energy INCREASES across a period and DECREASES down a group. This is because as you move down a group, the number of electron shells in an atom increases, meaning the outer shell is further away from the positive nucleus. The further away an outer shell is from the nucleus, the weaker the attraction so it requires less energy to remove an electron.

40
Q

Explain Dalton’s model of the atom.

A

Dalton’s model or the billiard ball model, of the atom was a solid sphere. Atoms of different elements differed from one another by sizes and colors.

  • All matter is composed of tiny, indivisible particles called atoms
  • Atoms of an element have similar properties
41
Q

Why does the trend for electron affinity occur across the period?

A

Electron affinity INCREASES across the period and DECREASES down the period. This happens because across the period, the number of protons increases causing a greater attraction for electrons

42
Q

Define electron affinity

A

The energy released or absorbed when an electron is added to a neutral atom

43
Q

Why does the trend for electron affinity occur for down a period?

A

Electron affinity INCREASES across a period and DECREASES down a group. This happens because as you go down the group, there are more filled electron shells. The more shells there are, the further the valance electrons are from the nucleus. The inner electrons block the positive charge from the nucleus there causing the electron affinity to decrease.

44
Q

Define electro negativity

A

The indicator of the relative ability of an atom to attract shared electrons

45
Q

Why does the trend for electron negativity occur across a period?

A

Electron Negativity INCREASES across a period and DECREASES down a group. This is because electrons are attracted by the positive protons in the nucleus and as you go across a period, the nucleus contains more protons. Therefore when there are more protons, you need more power to attract electrons

46
Q

Why does the trend for electron negativity for occur down a group?

A

Electron negativity INCREASES across a period and DECREASES down a group. This happens because as you go down a group, there are more electron shells being added and the valance electrons are further away from the nucleus and therefore does not have as strong of a pull.

47
Q

Why is the second ionization energy higher than the first ionization energy?

A

This is because it requires more energy to remove an electron from a positively charged ion than from a neutral atom.

48
Q

What are some differences between Bohr’s model and Quantum’s model?

A

Electrons:
According to Bohr they are particles with a negative charge, but quantum states that it is a cloud or smear of negative charge

Energy Level:
According to Bohr a circular path or orbit on which the electron travels around the nucleus, but quantum states that it is a distance from the nucleus within which is found an electron of a given energy

Orbital:
According to Bohr’s model there are no orbitals but quantum states that a specific shaped region of space (s,p,d,f) within which there is over 90% chance of finding an electron within an energy level holding 2 electrons

Chemistry 11 Chapter 1 (1 decks)

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