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Chemistry > Atomic Structure and Periodic Table > Flashcards

Atomic Structure and Periodic Table Flashcards

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1
Q

The radius of an atom

A

0.1 nanometres (1 x 10^-10)

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2
Q

Radius of a nucleus

A

1 x 10^-14

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3
Q

Protons relative mass

A

1

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4
Q

Protons relative charge

A

+1

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5
Q

Neutrons relative mass

A

1

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6
Q

Neutrons relative charge

A

0

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7
Q

Electrons relative mass

A

Very small

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8
Q

Electrons relative charge

A

-1

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9
Q

Do atoms have any overall charge

A

No they are neutral (unlike ions), becasue they have the same amount of protons and electrons.

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10
Q

Atomic Number (bottom)

A

Tells you the number of protons

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11
Q

Mass Number (top)

A

Tells you the number of protons and neutrons

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12
Q

Definition of Isotopes

A

Different forms of the same element, which have the same number of protons, but a different number of neutrons.

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13
Q

Relative atomic mass

A

Is an average mass taking into account the different masses and abundances (amounts) of all the isotopes that make up one element.

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14
Q

Relative atomic mass =

A

sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes

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15
Q

A compound formed from a metal and a non-metal consists of

A

ions (ionic bonding, metal loses electrons to get positive ions and non-metal gains electrons to get negative ions, opposites attract.)

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16
Q

Ionic Bonded compounds

A

Sodium chloride, magnesium oxide, calcium oxide

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17
Q

A compound formed from non-metals consists of

A

molecules (covalent bonding, sharing electrons)

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18
Q

Covalent Bonded compounds

A

hydrogen chloride gas, carbon monoxide, and water.

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19
Q

Balancing Equations

A

Can’t change the little numbers so have to add a big number in front, everything needs the same number of atoms on both sides.

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20
Q

Ways to separate mixtures

A

Crystallisation, Simple Distillation, Fractional Distillation, Filtration, and Chromatography.

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21
Q

Chromatography steps

A
  1. Draw a line at the bottom of the filter paper in pencil
  2. Add a spot of ink to the line and place the sheet in a beaker of solvent (water), make sure the ink isn’t touching the water
  3. Place a lid on the container to stop the solvent from evaporating
  4. As the ink moves up the paper the dyes will separate out
  5. If any of the dyes in the ink are insoluble they will stay on the baseline
  6. Remove the paper once the solvent has nearly reached the top of the paper, and leave to dry
  7. The end results should be a pattern of spots called a chromatogram.
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22
Q

Filtration Steps

A
  1. Filtration can be used when the product is an insoluble solid that needs to be separated from a liquid.
  2. Put filter paper in a funnel that is placed in a beaker or conical flask.
  3. pour the mixture into the funnel
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23
Q

Evaporation

A
  1. Pour the solution into an evaporating dish
  2. Slowly heat the solution. The solvent will evaporate and the solution will get more concentrated. Eventually, crystals will start to form.
  3. Keep heating the evaporating dish until all you have left are dry crystals.

Equipment: Bunsen Burner, Evaporating dish, tripod.

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24
Q

Crystallisation Steps

A
  1. Pour the solution into an evaporative dish and gently heat the solution. Some of the solvent will evaporate making the solution more concentrated.
  2. Once some solvent has evaporated, or once you start to see crystals form (the point of crystallisation), remove the dish from the heat and leave it to cool.
  3. The salt should start to form crystals as it becomes insoluble in the cold, highly concentrated solution.
  4. Filter the crystals out of the solution, and leave them in a warm place to dry. You could use a drying oven or a desiccator.
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25
Q

How to separate Rock Salt (salt and sand)

A
  1. Grind the mixture to make sure the salt crystals are small so they can dissolve easily.
  2. Dissolve the mixture in water, the sand will not dissolve. Heating will help the salt dissolve faster.
  3. Filter the mixture to separate the sand from the salt water.
  4. Evaporate the water from the salt so that it forms dry crystals.
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26
Q

Simple Distillation Steps

A
  1. Simple distillation is used for separating a liquid from a solution.
  2. The solution is heated. The part of the solution that has the lowest boiling point evaporates first.
  3. The vapour is then cooled, condenses (turns back into a liquid) and is collected.
  4. The rest of the solution is left behind in the flask.

Equipment: Conicle flask with bung, thermometer, condenser, a beaker.

Can only be used to separate things with very different boiling points, if the temperature goes higher than the point of the substance with the higher boiling point, they will mix again.

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27
Q

Fractional Distillation Steps

A

Can separate mixtures of liquids even if they have similar boiling points.

  1. Put the mixture in a flask and stick a fractionating column on top and a thermometer on top of that. Then you heat it.
  2. The different liquids will all have different boiling points, so they will evaporate at different temperatures.
  3. The liquid with the lowest boiling point evaporates first. When the temperature on the thermometer matches the boiling point of this liquid, it will reach the top of the column.
  4. Liquids with higher boiling points might also start to evaporate. But the column is cooler towards the top. So they will only get part of the way up before condensing and running back down towards the flask.
  5. When the first liquid has been collected, you raise the temperature until the next one reaches the top.

Equipment: Flask, Fractioning column, thermometer, condenser, test tubes.

28
Q

John Dalton

A

The first description of the atom was in the 19th century. Solid spheres and different spheres made up the different elements.

29
Q

J J Thomson

A

He found out that Atoms aren’t solid spheres in 1897. His measurements of charge and mass showed that an atom must contain even smaller, negatively charged particles, electrons. Now called the plum pudding model.

30
Q

Ernest Rutherford

A

1909 conducted alpha particle scattering experiments. Fired positively charged alpha particles at a thin sheet of gold. Most of the atoms passed through the sheet but some deflected more than expected, meaning the plum pudding model couldn’t be right. As the atoms should have all passed through or been slightly deflected at most.

He called the new model the nuclear model, in this, there is a tiny positive nucleus, a cloud of negative electrons surrounding the nucleus, so most of the atom is empty space. The closer the atoms were fired to the nucleus the larger the deflection, if fired into an empty space the atoms would pass through.

31
Q

Niels Bohr

A

Realized that a cloud of electrons would cause the atom to collapse as they would attract to the nucleus. Bohr suggested that the electrons are contained in shells and rotate around the nucleus and all have an equal distance from each other.

32
Q

James Chadwick

A

20 years after scientists accepted that atoms have nuclei, James Chadwick provided evidence for neutral particles in the nucleus. These became known as neutrons.

33
Q

How was the periodic table arranged in the 1800s

A

Atomic weight

34
Q

Dmitri Mendeleev (changed the periodic table)

A

Put the elements mainly in order of atomic weight but switched it if the properties meant it should be changed. This is shown in Te and I, Iodine actually has a smaller atomic weight but is placed after Tellurium as it has similar properties to elements in that group. He left gaps in the table for undiscovered elements, the known elements helped to place the new elements as they had similar characteristics.

35
Q

Where are the metals in the periodic table

A

metals - left non-metals - right

36
Q

Does group 1 react more vigorously as you go down the group?

A

Yes

37
Q

Does group 7 react more vigorously as you go down the group?

A

No, the reactivity decreases

38
Q

Metal’s physical properties

A
  1. Strong (hard to break), but can be bent and shaped (malleable).
  2. Good at conducting heat and electricity
  3. High boiling and melting points
39
Q

Non-metal physical properties

A
  1. More dull looking
  2. brittle
  3. aren’t always solids at room temp
  4. don’t generally conduct electricity
  5. often have a lower density
40
Q

Are group 1 elements very reactive

A

Yes, they only have 1 electron in their outer shell making them very reactive

41
Q

Alkali metal physical properties

A
  1. Soft
  2. Low density
42
Q

What are the elements in Group 1

A

Lithium, Sodium, Potassium, Rubidium, Caesium, Francium

43
Q

Does reactivity in group 1 increase as you go down the group?

A

Yes, as you go down the group the outer shell gets further away from the nucleus, making it easier to loose.

44
Q

Do Alkali metals have high melting and boiling points?

A

No

45
Q

How do group 1 elements react with water?

A

Vigorously to produce hydrogen gas and metal hydroxides, to produce alkaline solutions. The energy given by the reacting increases as you go down the group.

46
Q

How do group 1 elements react with chlorine?

A

Vigorously when heated in chlorine gas to form white metal chloride salts.

47
Q

How do group 1 elements react with oxygen?

A

They react to create a metal oxide.

Lithium reacts to form lithium oxide.

Sodium forms a mix of sodium oxide and sodium peroxide.

Potassium forms a mix of potassium peroxide and potassium superoxide.

48
Q

What are group 7 elements known as?

A

Halogens

49
Q

Are halogens all non-metals?

A

Yes, with colored vapors

50
Q

Florine properties

A

Very reactive, poisonous yellow gas

51
Q

Chlorine properties

A

Fairly reactive, poisonous dense green gas.

52
Q

Bromine properties

A

Dense, poisonous, red-brown volatile liquid.

53
Q

Iodine properties

A

Dark grey crystalline solid or a purple vapor.

54
Q

What happens as you go down group 7?

A
  1. Become less reactive, harder to gain an extra electron as its further away from the nucleus.
  2. Higher melting and boiling points
  3. Have higher relative atomic masses.
55
Q

What happens when halogens bond with metals?

A

They form Halides with 1- ions, from ionic bonding. (F-, Cl-, Br-, I-)

56
Q

Will more reactive halogens displace less reactive ones?

A

Yes, chlorine can displace bromine and iodine from an aqueous solution of its salts.

57
Q

What group are noble gases?

A

Group 0

58
Q

What elements are in noble gases?

A

Helium, Neon, Argon, Krypton, Xenon, Radon

59
Q

Why don’t noble gases react much?

A

They all have full outer shells so don’t need to gain or give an electron to be stable.

60
Q

What are monatomic gases?

A

Single atoms not bonded to each other. (Group 0)

61
Q

Properties of Noble Gases

A
  1. Boiling points increase as you go down the group, along with relative atomic mass.
62
Q

Why does the boiling point of noble gases increase as you go down the group?

A

Increase in the number of electrons in each atom leading to greater intermolecular forces to overcome.

63
Q

What is the order of the noble gases?

A

Helium, neon, argon, krypton, xenon, radon

64
Q

Neon is a gas at 25c. predict the state of helium at this temp?

A

25c. Helium is lower in the order of noble gases so must also be at 25 degrees.

65
Q

Radon and krypton have bp of -62 and -153. Predict the boiling point of xenon.

A

-108. Xenon is between radon and krypton in the order so we can estimate that it would be halfway between their boiling points.

(-153) + (-62) = -215
-215 / 2 = -107.5 = 108c

Chemistry (10 decks)

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