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Unit 1 Chemistry > The periodic table > Flashcards

The periodic table Flashcards

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1
Q

What is the kinetic theory of matter?

A

It states that:
Particles move faster with increasing temperature
Solids —-> particles vibrate in a fixed position
Liquid —-> particles are further apart and move more
Gas —-> particles are distinct from each other and move randomly

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2
Q

What is the atomic theory?

A

The atomic theory States that all matter in the universe is made up of little particles called ATOMS.

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3
Q

What did John Dalton propose?

A

All matter is composed of tiny particles called atoms
Atoms are indivisible (can’t be broken down further)
Atoms combine in whole number ratios

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4
Q

What did J.J. Thomson discover?

A

He discovered the electron and therefore particles were not indivisible
He proposed that atoms were positively charges spheres and negative charged particles called electrons embedded in the sphere

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5
Q

What did Ernest Rutherford propose?

A

The nuclear model of the atom
Consisted of mostly empty space with a dense nucleus that had positively charges protons
Orbiting around this were electron.

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6
Q

What was the flaw in Rutherford’s model?

A

That the orbiting electrons would lose energy and spiral into the nucleus

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7
Q

What did Niels Bohr propose?

A

That electrons orbit the nucleus in fixed energy levels and only electrons having a specific energy level could be in the energy level
Also electrons can jump to different energy levels by gaining or losing packets of energy

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8
Q

Who discovered the neutron?

A

Sir James Chadwick discovered that the nucleus contained a particle called neutrons as well as protons
Also that neutrons carried a neutral charge

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9
Q

What are the subatomic particles, where they are found and their relative charges?

A

Proton —-> found in the nucleus and a positive charge
Neutron —-> found in the dense nucleus and a neutral charge
Electron —-> found moving very rapidly around the nucleus in specific energy levels. Negative charge

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10
Q

What is an element?

A

An element is the purest form of substance containing only atoms of the same structure

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11
Q

What is the nuclei symbol?

A

A - mass number E - element symbol

Z - atomic number

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12
Q

What are isotopes?

A

Are atoms of the same element containing the same amount of protons but a different number of neutrons.

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13
Q

Explain Bohr’s energy levels?

A

Bohr proposed that electrons revolve around a nucleus in energy levels. Electrons can be given energy and thus they will move to a higher energy level or orbit. It has moved to excited state. When the electron gives off its energy it gives off the energy in the form of light

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14
Q

What is the emission spectra?

A

It is the separate lines of colour that correspond to an atoms energy levels if it’s electrons. Each line corresponds to one exact amount of energy being emitted

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15
Q

What is an electron shell?

A

A shell is a definite energy level that electrons move around in orbits

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16
Q

What is the equation of determining the max number of electrons in a shell?

A

2n^2

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17
Q

How many elements are there?

A

111 identified

93 found in nature

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18
Q

What is a compound?

A

Is any substance that can be broken down into its raw elements and are made by reacting elements together

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19
Q

What is a mixture?

A

A mixture is substance that is formed when to or more pure substances are combined without them reacting chemically

20
Q

What is a group and what does it correspond to?

A

A group is the vertical columns of the periodic table and corresponds to the number of valence electrons

21
Q

What is a period and what does it correspond to?

A

A period is the horizontal rows in the periodic table and corresponds to the number of electrons shells

22
Q

What are valence electrons?

A

Is the number of outer shell electrons

23
Q

What is group 1?

A

Alkali metals

24
Q

What is group 2?

A

Alkali earth metals, found in the earths crust

25
Q

What is group 17?

A

The halogens and are highly reactive

26
Q

What is group 18?

A

The inert gases or noble gases and are unreactive due to a full valence shell

27
Q 
Across a period what happens to 
Metallic character 
Atomic size
Reactivity
Electronegativity
A

Metallic character —> decreases across a period
Atomic size —> generally decreases as increasing electrons in outer shells causes them to come closer to the nucleus
Reactivity —> lowest in middle and high at ends except group 18
Electronegativity —> increases across a period

28
Q 
Down a group what happens to 
Metallic character 
Atomic size
Reactivity
Electronegativity
A

Metallic character —> increases down a group
Atomic size —>increases as more shells are added
Reactivity —>increases down a group
Electronegativity —> decreases as outer electrons are shielded from nucleus

29
Q

What is sublimation?

A

Sublimation is the process of a solid converting into a gas and vice versa without the substance turning into a liquid.

30
Q

Who discovered isotopes?

A

Frederick Soddy as he noticed whilst observing radioactive decay of thorium that two atoms of same element have different masses

31
Q

What is a mass spectrometer?

A

It is a machine that would make comparisons of the relative mass of atoms
Heavier atoms —> harder to deflect and travel in a wider curve.

32
Q

What does the mass spectrometer tell us?

A

The number of isotopes of any given element
The relative isotopic mass of each isotope
Percentage abundance of each isotope

33
Q

What colours appear on the hydrogen visible spectrum?

A

Red, Green, blue and violet.

34
Q

What did Bohr propose?

A

That electrons move around the nucleus in fixed paths called orbits each orbit corresponds to a specific energy level and electrons could jump to different orbits if they gain a specific amount of energy.

35
Q

What is the difference between ground state and excited state?

A

Ground state is when all electrons of an atom are in their designated energy level or shell/orbital whereas when electrons are in an excited state some electrons have jumped to higher energy levels or orbits

36
Q

What is the jump made by an electron called when it goes into excited state?

A

A quantum jump

37
Q

What did Schrödinger suggest about the arrangement of electrons within an atom?

A

He developed the quantum mechanical model where electrons are arranged in shells, sub shells and orbitals.

38
Q

What did Schrödinger say about the movement of electrons?

A

Electrons don’t move in a definite path however electrons of a specific energy level may be found in a region of space around a nucleus called an orbital.

39
Q

List the sub shells and their maximum amount of electrons?

A

S-2
P-6
D-10
F-14

40
Q

What is a sub shell?

A

Within a shell there are several different energy levels within the full shell and these are called sub shells

41
Q

Why do chromium and copper have different configurations than the usual pattern?

A

The arrangements gives chromium a half filled d shell and copper a full d shell. This is due to a full shell being more stable than a half filled shell and also a half filled shell is more stable than a partially filled shell

42
Q

Why did Mendeleev leave gaps in his version of the periodic table?

A

As many elements were sill undiscovered and Mendeleev proposed that the gaps in his table were elements that we’re going to be discovered in the future

43
Q

Explain Pauli exclusion principle

A

Orbitals can either contain 0, 1 or 2 electrons at any given time

44
Q

Why do you put one electron into each orbital before you add the second electron?

A

As the atom is a 3 dimensional shape it is more stable to have one electron in each orbital on each axis before the second one is added

45
Q

The purpose of the beam of high energy electrons used in the mass spectrometer is to..

A

Ionise atoms

46
Q

What do spectral lines suggest about the arrangement of electrons?

A

Suggest that electrons orbit around the nucleus in fixed energy levels with the higher energy level the further away from the nucleus

Unit 1 Chemistry (4 decks)

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