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Chemistry 🧪 > 1. Atomic Structure > Flashcards

1. Atomic Structure Flashcards

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1
Q

How do you create a new compounds word when reacting a metal/hydrogen and non metal (NONE BEING OXYGEN)

A

Combine the words and add the suffix -ide.

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2
Q

How do you create a new compounds word when reacting a metal/hydrogen and non metal (ONE BEING OXYGEN)

A

Combine the words and add the suffix -ate.

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3
Q

What is filtration for?

A

Separating an insoluble solid from a liquid.

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4
Q

What is crystallisation for?

A

Separating the product from the solvent.

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5
Q

What is chromatography for?

A

Separating different substances dissolved in a liquid.

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6
Q

What is simple distillation for?

A

Separating a solvent from a solution

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7
Q

What is fractional distillation for?

A

Separating a mixture of substances according to their different boiling points.

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8
Q

What is a solvent?

A

The substance in which a solute is dissolved in.

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9
Q

What is a solute?

A

A substance that is being dissolved.

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10
Q

What is a solution?

A

A mixture of a solute and solvent.

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11
Q

What does soluble mean?

A

A substance that CAN be dissolved in a solvent.

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12
Q

What does insoluble mean?

A

A substance that CANNOT be dissolved in a solvent.

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13
Q

What process should you use to separate a solid from a solid?

A

Dissolve, filtration and crystalisation

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14
Q

What process should you use to separate an insoluble solid and liquid?

A

Filtration

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15
Q

What process should you use to separate a soluble solid and liquid?

A

Crystallisation

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16
Q

What process should you use to separate a liquid and a liquid?

A

Distillation

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17
Q

What process should you use to separate multiple soluble solids and a liquid?

A

Chromatography

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18
Q

How did the alpha particle experiment work?

A
  1. Ernest Rutherford did it to disprove the Plum Pudding Model by JJ Thomson
  2. Theoretically alpha particles pass straight through the thin gold foil
  3. Most passed straight through but some were deflected more than 90 degrees. As smaller percentage were reflected back
  4. This proved that the atom is mostly empty space and the reflections proved that there was a positively charged central dense mass (nucleus)
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19
Q

What is the charge and mass of a proton?

A

+1 and 1

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20
Q

What is the charge and mass of an electron?

A

-1 and 1/2000

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21
Q

What is the charge and mass of a neutron?

A

0 and 1

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22
Q

What does the atomic number represent?

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A

The number of protons (it is the smaller number)

23
Q

What does the relative atomic mass represent?

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A

The number of protons and neutrons (the larger number)

24
Q

How do you find out the number of electrons in an element?

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A

Look at the atomic number, it is the same IF the element has no charge.

25
What is an isotope?
Atoms of the same element which have a different number of neutrons but they have the same number f protons and electrons. Therefore they have the same atomic number but a different relative atomic mass.
26
How do you calculate the relative atomic mass of an element?
(Isotope 1 abundance x Isotope 1 mass) + (Isotope 2 abundance x Isotope 2 mass) ALL divided by 100
27
How many electrons can be in each shell?
2 in the first shell 8 in the second shell 8 in the third shell 18 in the fourth shell
28
What are some facts about John Dalton?
- he was the first scientist in the discovery of the atom in 1808 - he made the solid spheres model - it described that an element is made up from atoms of identical size and mass
29
What are some facts about JJ Thomson?
- he was the second scientist in the discovery of the atom in 1897 - he created the plum pudding model - it described that an atom is a big area of positive charge with tiny electrons dotted through it
30
What are some facts about Ernest Rutherford?
- he was the third scientist in the development of the atom in 1911 - he created Rutherford’s atomic model - he carried out an experiment using gold foil and alpha particles to discover that atoms are mostly empty space with a small centre called the nucleus - later in 1920, Rutherford came up with the idea that there must be a third particle in the atom that has no charge
31
What are some facts about Niels Bohr?
- he was the fourth scientist in the discovery of the atom in 1913 - he created the Bohr model - it described that electrons are grouped together in layers/ shells at particular energy levels
32
What are some facts about James Chadwick?
- he was the fifth scientist in the discovery of the atom in 1932 - he created the current model of the atom - he discovered the neutron and realised that an unusual radiation was a neutral, sub-atomic particle
33
Why did Mendeleev leave gaps in his version of the periodic table?
To place elements not known at the time later.
34
What are some properties of metals?
They are: - good conductors of electricity - good conductors of heat - shiny - having different levels of reactivity - ductile - malleable - strong - having a high density - sonorous
35
What does malleable mean?
Something can be hammered into different shapes
36
What does ductile mean?
Something that can be pulled into wires.
37
What is an ion?
A charged atom
38
What does sonorous mean?
Something is capable of making a ringing noise
39
What are some facts about the electron structure of metals?
- they tend to have 3 electrons or less in their outer shell - in chemical reactions involving metals, these electrons are given to another atom - when this happens, the atom is called an ion - the negative electrons are lost - inside the nucleus, the number of protons stays the same so there will be more positive charges than negative - metals form positive ions
40
What are alkali metals?
Metals in group 1 of the periodic table which react with water to form strongly alkaline hydroxides.
41
What is density?
A measurement of mass per unit volume. It is how tightly packed a substance’s particles are in a particular space.
42
What are alkali metal hydroxides?
Soluble compounds formed when alkali metals react with water. They form colourless solutions.
43
What increases down group 1?
- size of atoms (atomic radius) - mass of the atoms - softness of the metal (due to the weakness of metallic bonds) - generally density
44
What decreases down group 1?
- the melting point - the boiling point
45
What happens to lithium in water?
It floats, moves rapidly across the surface of the water, disappears once reacted and fizzes.
46
What happens to sodium in water?
It floats, moves very rapidly across the surface of the water, forms a disappearing ball shape and fizzes vigorously.
47
What happens to potassium in water?
It floats, moves the most rapidly across the surface of the water, fizzes and ignites and burns with a lilac flame.
48
What are 6 examples of transition metals?
- chromium (Cr) - manganese (Mn) - iron (Fe) - cobalt (Co) - nickel (Ni) - copper (Cu)
49
What are the properties of transition metals in comparison to group 1elements?
- strong, dense and hard - much higher melting and boiling points - often used as catalysts - transition metals react slowly or not at all - the compounds formed from transition metals are usually coloured
50
What happens when group 1 metals react with each other?
Usually white compounds are formed.
51
What are some facts about group 7 elements?
- they are called the halogens - they are all found in pairs of atoms (they are diatomic) - they form molecules with two atoms in them - this structure gives them a full outer shell by sharing electrons - the halogens need to gain one more electron to have a full outer shell, forming a negative ion
52
What increases down group 7?
Melting and boiling points (as atoms get bigger)
53
What decreases down group 7?
Reactivity
54
What happens as electrons get closer to the nucleus?
The electrons become more reactive and held tighter to the nucleus.

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