Aromic Theory And Periodic Table Flashcards

1
Q

A substance that is made of only one kind of atom is

A

An element

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2
Q

Subatomic

A

Smaller than an atom

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3
Q

All atoms of the same element have he same number of

A

Protons

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4
Q

An ion

A

An atom that has gained or lost electrons

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5
Q

An isotope

A

An atom that has a different number of neutrons

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6
Q

The charge of an atom is

A

Neutral

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7
Q

The charge of the nucleus is

A

Positive

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8
Q

How do you find mass number

A

Add protons and neutrons

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9
Q

Atomic mass

A

Average mass for atoms of that element

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10
Q

Units used for mass

A

Atomic mass unit (A.M.U) for atoms

Grams for other things

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11
Q

Units for volume

A

Liters L

Milliliters ML

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12
Q

Experimental variable

A

Thing being tested

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13
Q

Controlled variable

A

Things kept constant and controlled

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14
Q

Depending variable

A

Measured, recorded, counted
Depends on experimental variable
Y axis

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15
Q

Independent variable

A

Known before experiment
Includes experimental
X axis

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16
Q

Control set up

A

Normal
Doesn’t change anything
Used to compare results
New and old soap control is the old soap

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17
Q

If——–

Then——

A

If–prediction—-

Then—expected results—

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18
Q

How many meters in a kilometer

A

1,000

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19
Q

How many centimeters in a meter

A

100

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20
Q

How many mililiters in one meters

A

1,000

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21
Q

How many ML in a liter

A

1,000

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22
Q

How many milligrams in a gram

A

1,000

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23
Q

How many grams In a kilogram

A

1,009

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24
Q

Density formula

A

D = M divided by V

25
How to find proton
Atomic #
26
How to find electron
Neutral atom it's the atomic number | Charge it is the charge number C-14 -1
27
How to find neutrons
Mass #- atomic#
28
Oxidation number
of electrons gained or lost to get full outer energy level. + because adding positive to get rid of the electron
29
Period
Horizontal 1 to 7
30
Columns
Groups, vertical, 1-18
31
Valence electrons
Number of electrons in the outermost shell, the ones that interact
32
Lewis for diagram
- ----15 - -4........3 - -8........7 - ----26
33
Democratus
Named the atom | Big black dot for diagram
34
Lavoisier
Wrote the law of conservation of matter
35
Bohr
Found out that electrons formed different energy levels | Bohr diagram
36
Chadwick
Discovered the neutron
37
Mendeleev
First periodic table
38
Thomson
Discovered the electron | Plum pudding model
39
Rutherford
Solar system model | Discovered proton and nucleus
40
Who used a cathode ray tube to see the path of praticles
Thomson
41
When Thomson discovered negative particles this told him that
There where positive particles somewhere
42
Who was the first person to see the smaller piece of matter was an atom
Democratus
43
What is the most modern theory for the structure of an atom
Wave model
44
Which families are most reactive
Alkali metals and alkaline earth metals are second
45
Where is it easiest to steal electrons
Bottom left corner
46
Metal location/ three l
Left Large radius Low ionization
47
What metals are highly radioactive
Lanthanides and actinides
48
Which family is inert
Nobel gases
49
What metals have different oxidation numbers depending on environment
Transition metals
50
Which non metals are highly reactive
Halogens, for salts
51
How do you find valence electrons an element has using the periodic table
The ones place of the group number
52
How does the periodic table tell how many energy levels an element has
The row number tells the number of energy levels
53
What happens to the atomic radius as you move left to right across a period
Atomic radius decreases as you move across a row because the increasing number of protons increases the electromagnetic force that pulls the electrons close to the nucleus.
54
What happens to atomic radius as you've too to bottom down a group
Atomic radius increases as you move down a group because the increasing number of energy levels increases the distance between the electrons and the nucleus.
55
What happens to the ionization energy as you move left to right across a period
Ionization energy increases as you move across a row because the increasing number of protons increases the electromagnetic force that holds the electrons to the atom, making it more difficult to remove an electron.
56
What happens to the ionization energy as you move top to bottom down a group
Ionization energy decreases as you move down a group because the increasing number of energy levels increases the distance between the electrons and the nucleus, decreasing the force of attraction and making the electrons easier to remove.
57
What is ionization energy
Ionization energy is the amount of energy needed to remove the outermost electron. (ionizing the atom)
58
What is electronegativity
Electronegativity is the amount of attraction that a nucleus has for electrons….how much electromagnetic force of attraction an atom generates