Chapter 2 - Atoms, Molecules, and Ions Flashcards

1
Q

Who’s studies does Atomic theory come from?

A

Dalton

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2
Q

What are Dalton’s Postulates?

A
  1. all atoms of an element are the same
  2. atoms may move from one substance to another, but they don’t disappear or turn into other elements
  3. compounds form from specific atoms in specific compositions
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3
Q

What does the law of conservation of mass state?

A

in a reaction, there is no change in the mass of atoms
ex: you burn something but mass of atoms stays the same

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4
Q

What does the law of constant composition state?

A

compounds always have the same elements in the same proportion
ex: H2O is always H2O, not HO1, HO3, etc…

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5
Q

What does the law of multiple proportions state?

A

elements combine to form compounds in whole number ratios
ex: you can’t have HO1/2

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6
Q

Summary of Thompson’s Cathode Tube Experiment

A
  1. electrical charge is passed through a gas from + to - plates
  2. as electricity passes, - plate emits a ray that is drawn to + plate
  3. this cathode ray could be deflected by a + or - charge
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7
Q

What conclusion was made from Thompson’s Cathode Tube Experiment?

A

that the rays were negatively charged and consisted of electrons

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8
Q

Summary of Rutherford’s Gold Foil Experiment

A
  1. threw alpha particles at gold foil
  2. hypothesized that if + and - charger were evenly distributed then the collisions would all be the same
  3. but most went straight through, some scattered, some bounced back
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9
Q

What hypothesis was formed from Thompson’s Cathode Tube Experiment?

A

atoms made up of positive and negative particles with charges are distributed evenly - led to the “Plum Pudding Model”

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10
Q

What conclusion was made from Rutherford’s Gold Foil Experiment?

A

that most of an atom is empty space, so there must be an unequal distribution of charge

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11
Q

What is represented by an atom’s Atomic Number “Z”

A

the number of protons in the atom

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12
Q

Characteristics of an Atom

A
  1. (+) charged nucleus (99.9% of the mass)
  2. (-) charged electrons
  3. Are described by their Atomic Number “Z”
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13
Q

Can atoms in a element differ in the number of protons “Z”

A

no

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13
Q

What is represented by an atom’s Mass Number “A”

A

the number of protons and neutrons in the atom

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14
Q

Isotope

A

an atom with a different number of neutrons than protons

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15
Q

How can you find the number of neutrons in an atom

A

By subtracting the Mass Number “A” by the Atomic Number “Z” (A - Z), which is the top number - bottom number in the nuclear symbol

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16
Q

What do Isotopes do if they are unstable

A

they decompose - transpose into another element (radioactivity)

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17
Q

Radiation

A

the energy given off in a decay

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18
Q

Why can’t an atom be weighed

A

because they’re too small and constantly moving

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19
Q

Atomic Mass

A

refers to 12C (carbon 12) as a reference
- 12C is defined as 12 AMU exactly
- other atoms are measured in relation to this

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20
Q

How to find atomic mass of an isotope?

A

Atomic Mass = (mass of isotope 1 x percentage) + (mass of isotope 2 x percentage) + (mass of isotope 3 x percentage)

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21
Q

What are the 3 major divisions of the periodic table?

A

Metals (left), Nonmetals (right), and Metalloids (middle)

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22
Q

Molecules

A

combination of 2 or more atoms
ex: H2O, CO, CH4

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23
Q

Ion

A

an atom that has gained or lost an electron

24
Cation
atom that has lost an electron (+)
25
Anion
atom that has gained an electron (-)
26
Monoatomic Ions
form from single atoms ex: Na+, Ca2+
27
Polyatomic Ions
form from multiple atoms, AKA: charged molecule ex: OH-, PO4 3-
28
Ionic Compounds
- held together by ionic bonds - are not molecules ex: NaCl, CaCl2
29
Transition Metals
- form ions but don't achieve the noble gas state - some exist in more than 1 ionic state (Fe2+ and Fe3+)
30
How are cations named?
by their element monoatomic ex: Fe2+ -> Iron 2 ion polyatomic ex: FeCl2 -> Iron 2 Chloride
31
If polyatomic ions contain oxygen, the one with the less amount of O will end in "...___" and the one with more O will end in "...___"
1. ite 2. ate ex: NO2- -> nitrite NO3- -> nitrate
32
ClO-
hypochlorite
33
ClO2-
chlorite
34
ClO3-
chlorate
35
ClO4-
Perchlorate
36
KCl
Potassium Chloride
37
MgBr2
Magnesium Bromide
38
Na(PO4)2
Sodium Phosphate
39
What indicates that an element can have more than 1 charge
if it is a transition metal ex: Cu, Zn
40
CuCl
Copper (1) Chloride
41
What should you do when naming a compound with an element that can have more than 1 charge (transition metal)
state the charge ex: CuCl -> copper (1) chloride
42
FeBr3
Iron (3) Bromide
43
How to name binary compounds of 2 nonmetals
(prefix) - element - (prefix) - element - ide
44
NO
Nitrogen Oxide
45
N2O
Dinitrogen Oxide
46
N2O3
Dinitrogen Trioxide
47
HCl (g)
Hydrogen Chloride Gas
48
HCl (aq)
Hydrochloric acid
49
NO2-
nitrite
50
NO3-
nitrate
51
SO3 2-
sulfite
52
SO4 2-
sulfate
53
Rule for naming Oxoacids
"...ite" becomes "...ous acid" "...ate" becomes "...ic acid"
54
HNO2
nitrous acid - (NO2- -> nitrite)
55
HNO3
nitric acid (NO3- -> nitrate)
56
HSO3 2-
sulfurous acid (SO3 2- -> sulfite)
57
HSO4 2-
sulfuric acid (SO4 2- -> sulfate)
58