Chemistry Flashcards
(116 cards)
1
Q
Chemistry
A
study of matter (what matter is made of)
2
Q
The things that make up stuff
A
the entities that comprise matter
3
Q
Entities (biggest to smallest)
A
atoms (protons, electrons, neutrons), molecules, electrons
4
Q
John Dalton
A
English schoolteacher- billiard ball (sphere) model
5
Q
The Dalton Model
A
billiard ball/sphere- atom is indivisible
6
Q
J.J Thomson
A
raisin bun model or plum pudding
7
Q
Plum Pudding Model
A
electrons embedded into a positive fluid
8
Q
Cathode ray tube
A
light cannot bend by itself it needs a charge (magnetic or electric)
- showed that the mass is 2000 times smaller than a hydrogen item
9
Q
You can calculate what with strong magnets in a circle
A
charge and mass of particles
10
Q
Ernest Rutherford
A
the gold foil experiment
11
Q
The Gold Foil Experiment
A
expected the beam of particles to go right through the gold foil but instead some went different ways
12
Q
Gold Foil Experiment proved that…
A
there was a small massive centre to the atom (nucleus) that caused them to deflect
13
Q
Nuclear Model
A
Rutherford- small positive, densely packed nucleus (over 99% of the mass in the nucleus)
Planetary
14
Q
Niels Bohr
A
Bohr Model found by the bright line spectra
15
Q
Bohr Model
A
nucleus and electrons orbiting (excited state)
16
Q
Excited State
A
add electricity and the electron jumps to the higher shell from the atom absorbing energy
17
Q
Bright Line Spectra
A
when the electrons in the excited state drop back down a certain colour is emitted based on the energy level
18
Q
Wave Mechanical Model
A
Erwin Schrodinger
19
Q
Number of electrons in each shell
A
2, 8, 18, 32, 32, 18, 2
20
Q
Bohr Model outer things
A
shells or orbits or energy levels
21
Q
Wave Mechanical Model outer things
A
orbitals (Bohr orbits)
22
Q
Periods
A
2 elements, 8, 8, 18, 18, 32, 32
18 groups
23
Q
Alkali metals are
A
Extremely reactive- 1
24
Q
Alkali metals
A
Li, Na, K, Rb, Cs
25
Alkali earth metals are
Quite reactive- 2
26
Alkali earth metals
Be, Mg, Ca, Sr, Ba, Ra
27
Transition metals
3-12
28
Halogens are
extremely reactive- 17
29
Halogens
F, Cl, Br, I
30
Noble gases are
stable- 18
31
Noble gases
He, Ne, Ar, Kr, Xe, Rn
32
An entity is stable when...
the valence shell is full
33
IUPAC
International Union of Pure and Applied Chemistry
34
Molecular
two non-metals
35
Common molecular compounds
Sucrose- C12H22O11(s), glucose- C6H12O6(s), water- H2O(l), ammonia- NH3(g), ozone- O3(g), methanol- CH3OH(l), ethanol- C2H5OH(l)
36
Naming molecular compounds
use the prefixes
37
Prefixes
1. Mono-
2. Di-
3. Tri-
4. Tetra-
5. Penta-
6. Hexa-
7. Hepta-
8. Octa-
9. Ennea-
10. Deca-
38
Ionic
one non-metal one metal (solids)
39
Types of Ionic Compounds
Binary, Multivalent, Polyatomic
40
Sucrose
C12H22O11 (s)
41
Glucose
C6H12O6 (s)
42
Ammonia
NH3 (g)
43
Ozone
O3 (g)
44
Methanol
CH3OH (l)
45
Ethanol
C2H5OH (l)
46
Binary (naming)
two elements
| - MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT
47
Multivalent (naming)
- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT AND THEN WHICH EVER OF THE TWO CHARGES YOU USED WILL BE THE ROMAN NUMERICAL
48
Polyatomic (naming)
- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT (using polyatomic ions)
49
Acids (5 indicators that can be seen)
- pH below 7 (lemon like 5 battery acid like 1)
- turns litmus paper red
- sour
- react with active metals (Mg, Zn, etc.)
- conduct electricity
50
Acid Indicator (cannot be seen)
- hydrogen (H)
- COOH will always be an acid
- all acids will be (aq)
51
Base (5 indicators that can be seen)
- pH above 7 (7 is neutral)
- turns litmus paper blue
- bitter
- feel slippery
- conduct electricity (electrolytes)
52
Base Indicator (cannot be seen)
- hydroxide (OH)
53
Aqueous means...
dissolved in water
54
Will mixing an acid and a base change the conductivity?
- no
| - it will produce water and electrolytes
55
Every difference of one pH unit is an acidic difference of....
- 10
| - ex. pH 8 to 4 is 10000 times more acidic
56
Isotopes
- Potassium is made of 19 protons and 19 neutrons
- some isotopes would have 21 neutrons some would have 20
- the .1 changes the amount
57
Atomic Number
- tells you how many PROTONS and ELECTRONS
58
Mass Number
- tells you the total number of protons and NEUTRONS added
59
Atomic mass minus atomic number...
- tells you the number of NEUTRONS
60
Why is water the universal solvent?
- it is a polar substance (O is negative and H and H are positive)
61
For acids ate goes to...
| ide goes to....
- ic
| - hydro _______ ic
62
If an ion is dissolved it is an ____________.
electrolyte
63
Element
cannot be broken down into any other substance (one atom)
64
Periods are
horizontal (7 of them)
65
Groups are
vertical (18 of them)
66
Do electrons farther away from the nucleus have more energy than those closer?
yes
67
Valence electrons
electrons in the OUTER energy level
68
Valence number
the number of electrons an element can gain or lose to combine with other elements
69
Ion
an atom where the number of electrons is not equal to the protons (has a net electric charge due to the loss or gain of electrons)
70
Precipitate
sometimes when ionic solutions are mixed they form a precipitate (a solid with low solubility that forms a solution)
71
When acids and bases are mixed... (neutralization)
when acids and bases react together both their acidic and basic properties disappear (process of neutralization)
72
Neutralization
acids and bases mixing and producing water and salt
73
Why do ionic solids have high melting points while molecular solids have low melting points?
- ionic solids have stronger attractive electrostatic (higher the attraction, higher melting point) (positive and negative attract strongly)
74
Electrolyte
a solution that conduct electricity (ionic compounds) (ions are able to flow and move)
75
Octect Rule
every atom wants to have 8 valance electrons in the outer most shell
76
Ionic Bonding
when elements bond to become stable (bonds between non-metals and metals)
77
Acid in Batteries
sulfuric acid
78
Acid in Vinegar
acitic acid
79
the most common multivalent is...
the top one on the chart
80
Electrons are the same number as
protons
81
Protons are the same number as
electrons
82
bottle of hydrochloric acid means what hazard symbol
corrosive
83
ionic are (conductor, melting point, solubility)
good conductor, high melting point, soluble
84
neutralize stomach acid with...
NaHCO3
85
photosynthesis formula
6CO2(g) + 6H2O ----- 6O2(g) + C6H12O6 (exothermic)
86
law of conservation of mass
mass of reactants and products must be the same
87
reactants
left side of equation
88
products
right side of equation
89
endothermic
energy going in (takes in energy)
90
exothermic
energy going out (lets out energy)
91
cellular respiration formula
C6H12O6(aq) + 6O2 --------- 6CO2(g) + 6H2O(l) + energy
| endothermic
92
anaerobic respiration
(bread, pizza dough)
- yeast is the enzyme (catalyst) digesting the sugar to produce gas to make the chemical reaction occur (not part of the reaction)
C6H12O6(s) -------
2CO2(g) + 2C2H5OH(l)
93
airbags
energy + 2NaN3(s) ------- 2Na(s) + 3N2(g) (exothermic)
94
sodium azide
used in airbags NaN3(s) (decomposes into its elements)
95
Rusting
Fe(s) + O2(g) ------- Fe2O3(s)
96
BBQ
C3H8(g) + 5O2(g) -------- 3CO2(g) + 4H2O(g)
| combustion of propane
97
diatomic
elements need (H2, Br2, etc.) in chart
98
ionic compounds are (s, l, g, aq)
solid
99
Acids are always (s, l, g, aq)
aqueous
100
Formation
a + b = ab
101
Decomposition
ab = a + b
102
combustion
CxHy + O2(g) = CO2 + H2O
103
single replacement
ab + c = ac + b or bc + a
104
double replacement
(displacement or neutralization) ab + cd + cb + ad
105
hydrogen w a match
pops
106
match ____ in CO2
goes out
107
match _____ in O2
gets bigger
108
Moles
used to count atoms, particles, molecules
109
Avogadro's number (1 mol)
6.02 x 10 to the 23
110
1 mole is defined as
12g of pure carbon -12
111
n=m/M
```
chemical amount (mol) = mass (g) / molar mass (g/mol)
- mass is is amount (g), chemical amount is moles, molar mass is in periodic table
```
112
how to find atoms or molecules
multiply the moles by 6.02 x 10 to the 23
113
How to read 2Na(s) + 2H2O(l) ------- H2(g) + 2NaOH(aq)
“2 moles of sodium react with 2 moles of water to produce 1 mole of hydrogen and 2 moles of sodium hydroxide”
114
How to find # of particles
n x N (moles times Avogadro's number)
115
when writing equations do you put the positive or negative element first?
Positive
116
round to...
the same number of digits as the question gives you
