Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry. > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is an atom?

A

The smallest part of an element that can exist.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an element?

A

A substance made up of atoms that all have the same atomic number/number of protons in their nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a compound?

A

2 or more elements chemically bonded together.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a mixture?

A

2 or more elements or compounds not chemically combined together.
e.g. air

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Give 5 chemical formulas for compounds and identify how many elements/atoms they contain.

A

› Carbon Dioxide - CO₂ = 1 carbon atom, 2 oxygen atoms.
› Ammonia - NH₃ = 1 nitrogen atom, 3 hydrogen atoms.
› Water - H₂O = 2 hydrogen atoms, 1 oxygen atom.
› Sodium Chloride - NaCl = 1 sodium atom, 1 chlorine atom.
› Carbon Monoxide - CO = 1 carbon atom, 1 oxygen atom.
› Hydrochloric Acid - HCl = 1 hydrogen atom, 1 chlorine atom.
› Calcium Chloride - CaCl₂ = 1 calcium atom, 2 chlorine atoms.
› Sodium Carbonate - Na₂CO₃ = 2 sodium atoms, 1 carbon atom, 3 oxygen atoms.
› Sulfuric Acid - H₂SO₄ = 2 hydrogen atoms, 1 sodium atom, 4 oxygen atoms.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Practice balancing equations.

A

Practice balancing equation.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How can filtration be used to separate mixtures?

A

To separate insoluble solids from liquids and solutions, also can be used for purification as well.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How can crystallisation be used to separate mixtures?

A
  1. Pour the solution into an evaporating dish and gently heat the solution which will evaporate some of the solvent and the solution will get more concentrated.
  2. When you see crystals start to form, remove the dish from the heat and leave the solution 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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How can simple distillation be used to separate mixtures?

A

Distillation is used to separate mixtures which contain liquids.

  1. Solution is heated and the part of the solution with the lowest boiling point evaporates first.
  2. The vapour is then cooled which then condenses and is collected.
  3. The rest of the solution is left in the flask.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How can chromatography be used to separate mixtures?

A

This is used to separate compounds out of a mixture.

  1. Draw a line with pencil 1-2cm away from the bottom a filter paper.
  2. Add a spot of ink to the line and place sheet in beaker of solvent (make sure ink isn’t touching solvent).
  3. Place a lid on top of the container to stop the solvent evaporating.
  4. The solvent seeps up the water carrying the ink with it.
  5. Different dyes will move up the paper at different rates and when it reaches the top of the paper, take the paper out of the beaker to dry.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the formulae to finding the R𝚏 value?

A

distant travelled by substance / distance traveled by solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What did Rutherford say about the atom?

A

He was the third to speak on atoms saying that the plum pudding was wrong. He thinks that the nucleus is positively charged which is where the mass is concentrated and a ‘cloud’ of negative electrons surround this nucleus so most of the atom is empty space.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What did Neils Bohr say about the atom?

A

He was the last one to speak on atoms making the nucleus model of the atom which suggested that all electrons were contained in shells. The electrons orbit the nucleus in fixed shells and aren’t anywhere in-between as each shell is a fixed distance from the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What did John Dalton say about the atom?

A

He was the first to speak on atoms. At the start of the 19th century, he said that atoms are solid spheres and that the different spheres made up different elements.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What did JJ Thompson say about the atom?

A

He was the second one to speak on atoms in 1897 saying that atoms aren’t solid spheres as his measurements of charge and mass showed that atoms must contain even smaller, negatively charged particles such as electrons which was called the plum pudding model. It shows that the atom is a ball of positive charge with negative electrons embedded on it.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Describe a nucleus.

A

›it’s in the middle of the atom.
› contains protons and neutrons.
› positively charged because of protons.
› mass of atom concentrated in the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Describe an electron.

A

› move around the nucleus in electron shells.
›negatively charged and tiny but cover up a lot of space.
› volume of their orbit determines the size of atom.
›no mass.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is a protons relative mass and relative charge?

A

RELATIVE MASS: 1

RELATIVE CHARGE: +1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is a neutron relative mass and relative charge?

A

RELATIVE MASS: 1

RELATIVE CHARGE: 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is an electron relative mass and relative charge?

A

RELATIVE MASS: very small.

RELATIVE CHARGE: -1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What does the atomic number tell you?

A

The amount of protons (bottom number).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does the mass number tell you?

A

Total number of protons and neutrons (top number).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

How do you find the amount of neutrons?

A

mass number - atomic number.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why do atoms have no overall electrical charge?

A

They have the same number of protons as electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What are isotopes?

A

Atoms which have the same number of protons but a different number of neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is meant by the term relative atomic mass?

A

An average mass number for an element.

[Aᵣ = sum of (isotope abundance x isotope mass number) / total abundance of all isotopes]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

How are elements arranged in the periodic table?

A

In order of atomic number (protons).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

IDENTIFY THE BLOCKS OF THE PERIODIC TABLE SUCH AS GROUP 1, 7,0 TRANSITION METALS AND NON METALS.

A

CHECK ANSWERS AFTER.

29
Q

What are the group 1 metals known as?

A

The alkali metals.

30
Q

What are the group 7 metals known as?

A

Halogens.

31
Q

What are the group 0 metals known as?

A

Noble gases.

32
Q

What is the difference between the modern periodic table and the early periodic table?

A

The modern periodic table is arranged by atomic number but the early periodic table was arranged by atomic mass.

33
Q

What did Dimitri Mendeleev do in the modern periodic table that wasn’t done in the early periodic table?

A

He left gaps to make sure elements with similar properties stayed in the same groups

34
Q

What ions do metals and non-metals form when they react?

A

› metals form positive ions.

› non-metals form negative ions.

35
Q

What are 3 differences between non-metals and metals?

A

› metals have metallic bonding which causes them to have similar basic physical properties - non-metals don’t have metallic bonding.
› metals are strong (hard to break) but can be bent or hammered into different shapes (malleable) - non-metals are brittle.
› metals are great at conducting electricity and heat - non-metals don’t generally conduct electricity.
› metals have high boiling and melting points - non-metals aren’t always solids at room temperature and often have a lower density.

36
Q

Why are the elements in group 0 (noble gases) unreactive?

A

They have full outer shells of electrons.

37
Q

How does the boiling point of noble gases increase?

A

As the relative atomic mass increases.

38
Q

Describe the reaction of the alkali metals with oxygen.

A

Forms (metal) oxide as the metal reacts with oxygen in the air to form a dull metal oxide layer:
› lithium reacts to form lithium oxide (Li₂O).
› sodium reacts to form a mixture of sodium oxide (Na₂O) and sodium peroxide (Na₂O₂).
›potassium reacts form a mixture of potassium peroxide (K₂O₂) and potassium superoxide (KO₂).

39
Q

Describe the reaction of the alkali metals with chlorine.

A

Group 1 metals react vigorously when heated in chlorine gas to form white metal chloride salts.
› 2Na(𝗌) + Cl₂(𝗴) → 2NaCl(𝗌)
↳ sodium + chlorine → sodium chloride.

40
Q

Describe the reaction of the alkali metals with water.

A

They react vigorously to produce hydrogen gas and (metal) hydroxides which are salts that dissolve in water to produce alkaline solutions.
› 2Na(𝗌) + 2H₂O(𝙡) → 2NaOH(𝖺𝚚) + H₂(𝗴)
↳ sodium + water → sodium hydroxide + hydrogen.

41
Q

What are the 3 trends in reactivity going down group 1?

A

› increasing reactivity - outer electron is more easily lost as the attraction between the nucleus and electron decreases.
›lower melting and boiling points.
›higher relative atomic mass.

42
Q

What are the 3 trends in reactivity going down group 7?

A

› become less reactive - harder to gain extra electron as outer shell’s further from nucleus.
› higher melting and boiling points.
› higher relative molecular masses.

43
Q

When does a displacement reaction occur?

A

Between a more reactive halogen and the salt of a less reactive one.

44
Q

How many elements are there?

A

About 100.

45
Q

What are the 5 ways to separate mixtures?

A 
›filtration.
› simple distillation.
› chromatography.
› crystallisation.
› fractional distillation.
46
Q

What is the independent variable?

A

The variable for which variables are changes.

47
Q

What is the dependant variable?

A

The variable for which the value are measured.

48
Q

What is the control variable?

A

The ones which must be kept the same.

49
Q

What are accurate measurements?

A

Close to the true value.

50
Q

What do valid experiments do?

A

Answer the question being asked.

51
Q

What are precise measurements?

A

Ones where there is little spread about the mean value.

52
Q

When is a measurement repeatable?

A

If the experiment is carried out by the same person using the same method and obtains the same results.

53
Q

What is meant by the term reproducible?

A

When the small experiment is carried out by a different person/group and you get the same results.

54
Q

What is the radius of an atom approximately?

A

≈ 0.1 nm

[≈ 1 x 10⁻¹⁰m]

55
Q

What is the radius of a nucleus approximately?

A

≈ 1 x 10⁻¹⁴ m

56
Q

What is a molecule?

A

Particle containing two or more non-metal atoms bonded covalently.

[molecules can be elements (if they only have one type of atom) or compounds]

57
Q

What is the use of a chemical formula?

A

Shows the proportion of atoms of each element in a compound.

58
Q

How do you find the group number of an element?

A

The number of electrons in the outer shell.

59
Q

How do you find the period number of an element?

A

The number of shells with electrons in.

60
Q

Describe how metals react to form outer shells?

A

> it gets a full outer shell by losing electrons.
more reactive when it loses electrons more easily.
more reactive towards the bottom left of the periodic table.

61
Q

Describe how non-metals react to form outer shells?

A

> it gets a full outer shell by gaining or sharing electrons.
more reactive when they gain electrons more easily.
more reactive towards the top right of the periodic table.

62
Q

What are the properties of group 1 metals?

A

> much more reactive.
less dense and softer.
lower melting points.

63
Q

What are the properties of group 0?

A

> electronic structure is stable so they are unreactive.
colourless monatomic gases at room temperature.
as you go down group 0, the boiling point increases.

64
Q

What happens when group 7/halogens react with fluorine?

A

It produces yellow gas.

65
Q

What happens when group 7/halogens react with chlorine?

A

It produces dense green gas.

66
Q

What happens when group 7/halogens react with bromine?

A

It creates volatile red-brown liquid.

67
Q

What happens when group 7/halogens react with iodine?

A

It produces dark grey solid or purple vapour.

68
Q

What ways can group 7 elements react to fill their outer shell in two ways?

A

> sharing electrons.
↳ halogens form the covalent bonds with other non-metals to form molecular compounds.
gaining an electron.
↳ halogens form ionics compounds when they react with metals.
↳ as they gain one electron, they form 1- ions
called halides.

69
Q

What happens to the chemical properties of each substance in the mixture?

A

They are unchanged.

chemistry. (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions