chapters 1&2 Flashcards
1
Q
1 PETAbyte
A
10^15
2
Q
1 TERAbyte
A
10^12
3
Q
1 GIGAbyte
A
10^6
4
Q
1 MEGAbyte
A
10^3
5
Q
1 KILObyte
A
10^3
6
Q
1 DECImeter
A
10^-1
7
Q
1 CENTImeter
A
10^-2
8
Q
1 MILLImeter
A
10^-3
9
Q
1 MICROmeter
A
10^-6
10
Q
1 NANOmeter
A
10^-9
11
Q
1 PICOmeter
A
10^-12
12
Q
1 FEMTOmeter
A
10^-15
13
Q
What to do when uncertain of measurements?
A
Uncertainty of measurement creates uncertainty in time!
14
Q
Significant figures in 4 easy steps:
A
- All nonzero digits and trapped zeroes are significant!
- Zeros that start a number are not significant!
- Zeros that end a number without a decimal are not significant!
- A nonsignificant zero can be made significant with a bar over it!
15
Q
Adding and subtracting significant figures:
A
The answers last digit will be in the same place as the last digit of the least certain measure (least accurate)!
16
Q
Multiplying and dividing significant figures:
A
The number of significant figures in the answer will equal the lowest number of significant figures in any factor! (The one that has the least amount of numbers!)
17
Q
Volume:
A
1L = 1000mL = 1000cm^3
18
Q
Robert Boyle:
A
All matter is made up of either elements or compounds!
19
Q
Element:
A
Any substance that cannot be broken into simpler components by chemical means!
20
Q
Compound:
A
Any substance that can be broken into simpler components by chemical means!
21
Q
John Dalton:
A
- All matter is made up of atoms (elements are composed of atoms!)
2.compounds are composed of atoms of more than one element! - A chemical reaction involves the rearrangement of atoms!
4.All atoms of a given element are identical! - Atoms are indestructible!
22
Q
JJ Thomson:
A
Subatomic particle (smaller than atom!)
Electrons: negatively charged subatomic particles
“Plum-pudding” model of the atom:
* 1. No positively charged particles!*
* 2. Electrons are the only particles= only mass!*
3. Atoms are mostly empty spaced (can’t have negative charges close to each other)!
1 and 2 are incorrect!
23
Q
Ernest Rutherford:
A
Protons:positively charged subatomic particles!
Rutherford’s atomic model:
1. Atoms contain a small, dense positively charged center called the nucleus!
2. The nucleus has almost the entire mass of the atom!
* 3. Electrons are dispersed in the empty space of the atom! *
3 is incorrect!
24
Q
James Chadwick:
A
Neutrons: neutral subatomic particles
25
Atomic number:
(z) The number of protons in an atom of an element
(It is found on the top of an element on the periodic table!)
26
Elements:
*Elements are electrically neutral!*
The same element can have different number of neutrons!
Elements with similar chemical and physical properties are placed in the column "group!"
To facilitate this arrangement, elements are also placed in rows, "period!"
27
Isotopes:
Atoms with the same number of protons, and electrons with different number of neutrons!
28
Mass number (A):
Number of protons + the number of neutrons!
29
Atomic mass unit (amu or u):
One twelfth the mass of carbon - 12 atom, equal to 1.66 X 10^-24
30
Dimitri Mendeleev:
Arranged elements by atomic mass!
31
The periodic law:
When the elements are arranged in increasing mass order, certain properties repeat periodically!
32
Ions:
Reactivity of an atom is related to the charged particles and it forms ions!
33
Cations:
Atoms that lose electrons become positively charged (ca(+)ions)!
Metals form cations!
Metals have the tendency to lose electrons!
For each positive charge, the ion has one less electron than the neutral atom!
Example:
Na atom= 11p+ and 11e- Na+ ion= 11p+ and 10e-
Ca atom= 20p+ and 20e- Ca^2+ ion= 20p+ and 18e-
Cations are named the same as the metal!
Sodium Sodium ion
Calcium Calcium ion
34
Anions:
Atoms that gain electrons become negatively charged!
Nonmetals form anions!
For each negative charge, the ion has one more electron than the neutral atom!
Example:
F atom= 9p+ and 9e- F ion: 9p+ and 10e-
N atom= 7p+ and 7e- N3- ion: 7p+ and 10e-
Anions are named by changing the ending of the name to ide!
Fluorine Fluoride ion
Nitrogen Nitride ion
35
Chemical bonding:
Compounds and molecules are held together by chemical bonds!
36
Ionic bonds:
Electrostatic attraction between positive metal ions and negative nonmetal ions!
Electrons are transferred from cation to anion!
(oppositely charged means they can attract each other!)
Ionic bonds are stronger than covalent bonds because in ionic bonds it is a positive and negative attraction!
37
Covalent bonds:
Electrostatic attraction of the shared electrons to the nuclei of the bonding nonmetal atoms (nonmetal & nonmetal)!
Electrons are always in motion the electrostatic attraction attracts both nonmetals!
38
Nomenclature:
Atoms bond together to make chemical formulas!
Chemical formulas have predictable naming patterns!
Focus primarily on ionic bonded compounds!
Generally ions forms to have number of electrons = to their closest noble gas (not the for transition metals)!
Example 1:
Potassium= 19p+ and 19 e- closest noble gas: argon (18e-)
Example 2:
Potassium ion= 19p+ and 18e- k^+1
39
Ionic compounds:
Compounds have no net charge!
Number of electrons lost by cations = number of electrons gained by anions!
Symbol of cation number of cations symbol of anion number of anions!
Example:
Cation= Na^+1 Anion= S^-2
2nd cation= Na^+1
Naming: Metal name+ anion name (-ide suffix)!:
Sodium sulfide
40
Writing ionic compound formulas:
1. Write the symbol and charge for each metal and anion!
2. Generate a number of ions to equal out the charges!
3. Reduce to smallest whole number ratio!
4. Assign it a name!
41
Complications: Cation charges:
Some cations have multiple Jons they can form!
Use the formula to get the name or use the name to get the formula!
Example:
Iron (fe) can form Fe^+2 (ferrous) or Fe^+3 (ferric)
42
Multivalent cations:
1.Determine the charge of the anion!
S (group 6A = 2 charge)
2. Calculate the total negative charge!
(-2)x(3)=-6
3. Determine total positive charge needed!
+6
4. Divide total charge by number of cations!
+6/2 Fe cations= +3 charge per cation
5. Name the compound!
Iron (III) sulfide
43
Complications: Polyatomic ions:
Some ions have multiple atoms in them, but only 1 charge!
Polyatomic ions!
-ate ions
Chlorate= CIO-3
-ate ion + 1O——-> same charge, per-prefix (per means add oxygen!)
Perchlorate= CIO-4
-ate ion -1O——> same charge, -ite suffix (ate to ite just means subtract 1oxygen!)
Chlorite= CIO-2
-ate ion -2O——> same charge, hypo-prefix,!
ite suffix
Hypochlorite= ClO-
44
Polyatomic ions:
1. Identity the ions!
Iron(IIl)= Fe+3
Nitrate= polyatomic ion= ( NO3)-1
2. Equal the charges!
Fe+3 (NO3)-1
(NO3)-1
(NO3)-1
(Add parenthesis to emphasize that need you that ion!)
3. Reduce!
Fe(NO3)3!
45
Acids:
A compound that loses H+ in solution!
Always shown as dissolved in water (aq)
*Anion in acid ends in-ide!*
Hydro-root ic- acid. HBr(g)= hydrogen bromide (root:brom) (suffix:ide)
HBr(aq)= hydrobromic acid (root:brom)
*Anion in did ends in-ate!*
Root-ic-acid. HNO3(g)= hydrogen nitrate (root:nitr) (suffix:ate)
HNO3(aq)= nitric acid (root:nitr)
*Anion in acid ends in-ite!*
Root-ous-acid. H2Co2(g)= hydrogen carbonite (root:carbon) (suffix:ite)
H2Co2(aq)= carbonous acid
46
NH4 (+1charge):
Ammonium ion!
47
Hg2 (+2 charge):
Mercury (I) ion!
48
CN (-1 charge):
Cyanide ion!
49
CH3CO2 (-1 charge) or C2H3O2 (-1 charge):
Acetate ion!
50
CO3 (-2 charge):
Carbonate ion!
51
HCO3 (-1 charge):
Bicarbonate ion or hydrogen carbonate ion!
52
C2O4 (-2 charge):
Oxalate ion!
53
NO2 (-1 charge):
Nitrite ion!
54
NO3 (-1 charge):
Nitrate ion!
55
PO4 (+3 charge):
Phosphate ion!
56
HPO4 (-2 charge):
Hydrogen phosphate ion!
57
H2PO4 (-1 charge):
Dihydrogen phosphate ion!
58
OH (-1 charge):
Hydroxide ion!
59
SO3 (-2 charge):
Sulfite ion!
60
SO4 (-2 charge):
Sulfate ion!
61
HSO4 (-1 charge):
Hydrogen sulfate ion or bisulfate ion!
62
CIO (-1 charge):
Hypochlorite ion!
63
CIO2 (-1 charge):
Chlorite ion!
64
CIO3 (-1 charge):
Chlorate ion!
65
CIO4 (-1 charge):
Perchlorate ion!
66
BrO (-1 charge):
Hypobromite ion!
67
BrO2 (-1 charge):
Bromite ion!
68
BrO3 (-1 charge):
Bromate ion!
69
BrO4 (-1 charge):
Perbromate ion!
70
IO (-1 charge):
Hypoiodite ion!
71
IO2 (-1 charge):
Iodite ion!
72
IO3 (-1 charge):
Iodate ion!
73
IO4 (-1 charge):
Periodate ion!
74
CrO4 (-2 charge):
Chromate ion!
75
Cr2O7 (-2 charge):
Dichromate ion!
76
MnO4 (-1 charge):
Permanganate ion!
77
O2 (-2 charge):
Peroxide ion!
78
SCN (-1 charge):
Thiocyanate ion!
