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Chemistry 1 > Atomic structure and periodic table > Flashcards

Atomic structure and periodic table Flashcards

1
Q

What is a proton?

A

Subatomic particle with a positive charge.

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2
Q

What is an electron?

A

Subatomic particle with a negative charge.

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3
Q

What is a neutron?

A

Subatomic particle with no charge.

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4
Q

What is the nucleus?

A

The massive centre of an atom. It contains the protons and neutrons.

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5
Q

What is an atom?

A

The smallest unit of matter that retains its identity.

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6
Q

What is an element?

A

A pure substance made from one type of atom. It cannot be made into a simpler substance by chemical means

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7
Q

What is a symbol?

A

The abbreviation for an element name. Always starts with a capital letter. (Na for sodium)

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8
Q

What is the atomic number?

A

Tells which element. Equal to the number of protons in an atom. (The top number)

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9
Q

What is the atomic mass?

A

It is equal to the number of protons plus neutrons. (The bottom number)

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10
Q

What is an isotope?

A

An atom of the same element that has a different number of neutrons and therefore a different mass.

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11
Q

What is an ion?

A

An atom that is charged because it has either gained or lost electrons.

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12
Q

What are groups?

A

The columns of the periodic table. It contains elements that are similar and is used to determine valence electrons

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13
Q

What is the periodic table?

A

Organizes all of the elements by increasing atomic number and in groups with similar properties.

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14
Q

What are periods in the periodic table?

A

The rows of the periodic table. Properties change across periods.

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15
Q

What are metals?

A

The largest category of element. Metals are shiny, malleable and conduct electricity

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16
Q

What are non-metals?

A

Located in the upper right of the periodic table. Non-metals are dull, brittle and non-conductor. Many are gases.

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17
Q

What are the alkali metals?

A

Groups 1 elements. They are the most reactive metals

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18
Q

What are the alkaline earth metals?

A

Group 2 elements. Reactive metals next to Group 1

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19
Q

What are the halogens?

A

Group 7 elements. Most reactive non-metals.

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20
Q

What are the Noble gases?

A

Also called inert gases. Unreactive.

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21
Q

What is reactivity?

A

How easily and quickly an element combines with another element

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22
Q

What is a compound?

A

Two or more different elements chemically combined

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23
Q

What are organic compounds?

A

Present in living or once living things. Contain both carbon and hydrogen.

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24
Q

What are inorganic compounds?

A

Not organic. Do not contain both carbon and hydrogen

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25
Define element
A substance made from one type of atom
26
Define mixture
A substance made from different elements/compounds not chemically combined/bonded
27
How are elements arranged in the modern periodic table in terms of protons?
In order of atomic number
28
What do groups?
The number of electrons in the outer energy level of an atom
29
What do periods show?
The number of energy levels in an atom
30
Why are elements placed in the same group in the periodic table?
They have similar chemical properties
31
Why is the periodic table called the periodic table?
Similar properties occur regularly
32
What are similarities between elements in the same group?
They have the same number of electrons in their outer energy level and similar chemical properties
33
Explain the development of the periodic table
- before discovering protons, neutrons and electrons, scientists tried to arrange the elements by putting them in order of their atomic weights. john newlands - noticed octaves/dobreiner - noticed triads) - the early periodic tables were incomplete and some elements were in the wrong groups if atomic weight was strictly followed - mendeleev then left gaps for elements he thought were undiscovered and in some places changed the order based on atomic weights. also arranged elements in rows and columns - knowledge about isotopes explained why atomic weight wasn't always correct
34
What is the difference between non-metals and metals in terms of chemical properties?
Metals react to form positive ions, non-metals react to form negative ions
35
What is the difference between non-metals and metals in terms of physical properties?
- Metals are conductive, non-metals are insulators - metals have high melting/boiling points, non-metals have low melting/boiling points - metals have high density, non-metals have low density - metals are shiny/hard/solid, non-metals are dull/brittle - metals are malleable, non-metals are not malleable (able to be moulded into different shapes)
36
Why are noble gases unreactive?
Their full outer energy level of electrons is full. this means they have a very stable electron configuration so they are inert (unreactive).
37
How many electrons in the outer energy level of a noble gas?
8 (they are full)
38
What happens to the boiling points of the noble gases as you go down the group?
It increases
39
Why do they boiling points of noble gases increase as you go down the group?
The intermolecular forces between the atoms become stronger
40
What gas is used in food packets and why?
Argon because it is unreactive and prevents food from degrading
41
What happens to density in noble gases as you go down the group?
It increases
42
What are group 1 elements called?
Alkali metals
43
What kind of compound is formed by group 1 elements when they react with non-metals? what charge does this compound have?
An ionic compound is formed (metal ion) with a positive charge (+1)
44
When group 1 metals react with water, what is formed?
A metal hydroxide is formed and hydrogen gas is given off
45
When group 1 metals react with oxygen, what is formed?
Metal oxides
46
What kind of solution is formed when group 1 metal hydroxides are dissolved in water?
An alkaline solution
47
When group 1 metals react with chlorine, what is formed?
A chlorine
48
Describe what reactions between alkali metals and oxygen/water are like
VIgorous
49
Write a BALANCED symbol equation for the reaction between sodium and oxygen
4Na + O2 -> 2Na2O
50
What happens to reactivity as you go down group 1?
It increases
51
Why does reactivity increase as you go down group 1?
The atom gets bigger and therefore the outer electron is further and more shielded from the positive nucleus. so, the outer electron experiences less attraction and is lost more easily.
52
What do halogens look like (fluorine to iodine)?
Fluorine - yellow Chlorine - pale green Bromine - orange/brown Iodine - purple
53
What state is fluorine at room temperature?
Gas
54
What state is chlorine at room temperature?
Gas
55
What state is bromine at room temperature?
Liquid
56
What state is iodine at room temperature?
Solid
57
What happens to the colour of halogens as you go down?
It gets darker
58
What is produced when halogens react with metals? what is the charge of a halide ion this happens?
Ionic salts, negative (-1)
59
What happens to melting/boiling and relative molecular mass as you go down group 7?
It increases
60
What happens to reactivity as you go down group 7?
It decreases
61
How many electrons in the outer energy level of a group 7 element?
7
62
Why does reactivity decrease as you go down group 7?
As the atom gets bigger, the outer energy level is further and more shielded from the positive nucleus. therefore the incoming electron experiences less attraction so is gained less easily.
63
What is the rule for displacement of halogens in group 7?
More reactive halogens can displace less reactive halogens
64
Will chlorine displace bromine from a solution of potassium bromide?
Yes
65
Where are transition metals?
Between groups 2 and 3
66
What charge do the ions transition metals form have?
Different (Both +1 and -1)
67
What can transition metals be used as?
Catalysts to speed up chemical reactions
68
Are transition metals good conductors of heat and electricity? are they malleable?
Yes, Yes
69
All noble gases have 8 electrons in their outer energy level but which is an exception?
Helium (it has 2 in its outer energy level)
70
Why is chlorine used in water?
It kills bacteria as halogens are toxic

Chemistry 1 (9 decks)

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