"Advanced Chemistry 10 - Summary of Semester #1"

5.0(2)
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/100

flashcard set

Earn XP

Description and Tags

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

101 Terms

1
New cards
Accuracy
The agreement of a particular value with the true value.
2
New cards
Precision
The degree of agreement among several measurements made in the same manner.
3
New cards
Direct Proportion
Two properties that are dividing one by the other and gives a constant value.

\-Straight Line
4
New cards
Inverse Proportion
Two quantities where their product is constant.

\-Curve Line
5
New cards
SI
Le Systeme International d’Unites
6
New cards
Derived Unit
Combinations of SI base units
7
New cards
Quantitative
Numerical information
8
New cards
Qualitative
Non-numerical information
9
New cards
Scientific Notation
Move decimal point so the number fits between 1 and 10.
10
New cards
For electronic devices…
record all digits.
11
New cards
For non-electronic devices..
read all certain digits and one uncertain digit.
12
New cards
Significant Digits
All the digits known with certainty plus one final digit, which is somewhat uncertain or estimated.
13
New cards
Atlantic
Decimal absent (right).
14
New cards
Pacific
Decimal present (left).
15
New cards
When adding or subtracting decimals…
use the fewest number of decimal places.
16
New cards
When multiplying or dividing decimals…
use the least amount of significant digits.
17
New cards
Dimensional Analysis
Skill used to convert units using conversion factors and proving the units.
18
New cards
Denisty
Mass/Volume

\-directly proportional
19
New cards
Thomson
Discovered the electron (cathode ray tube)
20
New cards
Millikan
Measured the charge of the electron (oil-drop experiement).
21
New cards
Rutherford
Gold foil experiement - found details of the atom’s structure - (nucleus was positively charged, atom is mostly space).
22
New cards
Bohr
Proposed a model in which electrons surrouned the positively charged nucleus as the planets surround the sun (planetary model).
23
New cards
Avogadro
Explained the number of particles in a mole (found a relationship between mass and the number of atoms).
24
New cards
Law of Conservation of Mass
Mass is neither created nor destroyed.
25
New cards
Law of Definite Proportions
A given chemical compound always contain its component elements in fixed ration (by weight) and does not depend on its source and method of preparation.
26
New cards
Law of Multiple Proportions
When two elements combine to form one compound, the mass of one element, when combined with a fixed mass of the other element, will always be ratios of whole numbers.
27
New cards
Dalton’s Theory

1. All matter is composed of extremely small particles called atoms.
2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties (not true).
3. Atoms cannot be subdivided, created, or destroyed (not true).
4. Atoms of different elements combine in simple whole number ratios to form chemical compounds.
5. In chemical reactions, atoms are combined, separated, and rearranged.
28
New cards
Nucleus
Center of the atom
29
New cards
Protons
Positive charge
30
New cards
Neutron
Neutral charge
31
New cards
Electron
Negative charge
32
New cards
Atomic Number
Number of protons. Shown on the periodic table.
33
New cards
Mass Number
Protons + Neutrons
34
New cards
Isotopes
Atoms that have the same number of protons and a different number of neutrons.
35
New cards
Molar Mass
Mass of one mole of a pure substance. Units are g/mol. Round to 2 decimal places.
36
New cards
Avogadro’s Number
6\.022x10^23
37
New cards
Electrons have properties of both …
particles and waves.
38
New cards
Wavelength
Distance between two consecutive corresponding points on a wave.
39
New cards
Frequency and energy are …
Directly proportional
40
New cards
Frequency
Number of complete waves that pass a point in 1 second.
41
New cards
Ground state electron
Lowest energy state.
42
New cards
Excited state electron
Highest energy state.
43
New cards
The emission of light is funamentally related to the behavior of the …
electrons.
44
New cards
Heisenberg uncertainty principal
It is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
45
New cards
Schrodinger
The quantum theroy.
46
New cards
DeBrogile
Combined mathematical equations and conluded that ANYTHING with mass and velocity has a corresponding wavelength.
47
New cards
Quantum Numbers
Specify the properties of an atomic orbital and the properties of electrons in an orbital.
48
New cards
Aufbau Principle
Electrons enter the lowest energy level possible
49
New cards
Pauli Exclusion Principle
No two electrons can have the same set of quantum numbers and therefore will have opposite spins.
50
New cards
Hund’s Rule
One electron enters an orbital of equal energy parallel in spin before pairing begins.
51
New cards
Octet Rule
8 electrons in the “s” and “p” sublevels.
52
New cards
Photons
Particles of light. Discovered by Einstein.
53
New cards
Quantum Leap
A huge, often sudden, increase or advance.
54
New cards
When an electron returns to the ground state from excited, it ...
releases the excess energy.
55
New cards
Principal Quantum Number
Describes the size of orbital.
56
New cards
Angular Momentum Quantum Number
Describes the shape of the sublevel.
57
New cards
Magnetic Quantum Number
Describes the orientation about the azes.
58
New cards
Spin Quantum Number
Describes the rotation of an electron.
59
New cards
Mendeleev
Responsible for arranging the periodic table by increasing ATOMIC MASS.
60
New cards
Moseley
Responsible for better arranging the periodic table by increasing ATOMIC NUMBER.
61
New cards
Main group elements
s and p.
62
New cards
Metals
\-Good conductors of heat and electricity

\-Malleable

\-Ductible

\-High tensile strength

\-Have luster
63
New cards
Nonmetals
\-Poor conductors of heat and electricity

\-Tend to brittle

\-Gases at room temperature
64
New cards
Ion
Particle with a charge.
65
New cards
Cation
Positive ion

\-Formed when electrons are lost.
66
New cards
Anion
Negative ion

\-Formed when electrons are gained.
67
New cards
Periodic Law
The physical and chemical properties of the elements are periodic functions of their atomic numbers.
68
New cards
Atomic Radius
One-half distance between two identical nuclei that are bonded. Increases going left and down.
69
New cards
Ionization Energy
The energy needed to remove the most loosely bound electron in an atom. Increases going right and up.
70
New cards
Electronegativity
The ability of an atom in a chemical compound to attract (gain) electrons. Increases going right and up.
71
New cards
Metalloids
\-Have properties of both metals and nonmetals.

\-More brittle than metals, less brittle than most nonmettalic solids.

\-Are semiconductors of electricity.
72
New cards
Chemical Bond
A mutual electrical attraction between the nuclei and valence electrons of different atoms that bind them together.
73
New cards
Ionic Bond
Transfer of electrons.

\-Metal and nonmetal
74
New cards
Covalent Bond
Sharing of electrons.

\-nonmetal and nonmetal
75
New cards
Bond energy and bond length are …
inversely proportional
76
New cards
Intermolecular Forces
Forces of attraction between molecules.
77
New cards
Dipole-Dipole
The negative region of one molecule is attracted to the positive region of another molecule.
78
New cards
Hydrogen Bonding
A hydrogen atom that is boned to a highly electro-negative atom is attracted to an unshared pair of electrons of another highly electronegative atom on another molecule.
79
New cards
London Dispersion Forces
Intermolecular attractions resulting from the constant motion of electrons and the creation of instant dipoles.
80
New cards
Intramolecular Forces
Forces of attraction within atoms.
81
New cards
Molecule
The smallest part of a covalently bonded substance within the properties of that substance.
82
New cards
VSEPR Theory
(Valence shell electron pair repulsion). States that bonded atoms and unshared electron pairs orient themselves as far apart from each other as possible.
83
New cards
Polar Covalent
Bond in which bonded atoms have an unequal attraction for the shared electrons.
84
New cards
Non-polar Covalent
Bond in which bonding electrons are shared equally by bonded atoms.
85
New cards
Lone Pairs
Electrons NOT involved in a chemical bond.
86
New cards
Percent Composition
The number of grams in one mole of a compound. A statement of the relative mass of each element contributes to the mass of the compound as a whole.
87
New cards
Empirical Formula
Formula that shows the whole-number ratio of elements in a compound.
88
New cards
Molecular Formula
The true numebr of atoms of each element in the formula compound.
89
New cards
Writing Binary Ionic Compounds

1. Write the symbol and charge of the cation first.
2. Write the symbol and charge of the anion last.
3. If the value are opposite and equal, use NO SUBSCRIPTS!
4. If the values of the charges are different, Criss-Cross Method!
5. Never bring down a 1 it is understood.
6. The formula must be in the simplest ratio.
90
New cards
Naming Binary Ionic Compounds

1. Write the cation name (metal) first.
2. Write the anion root name second.
3. Add “ide” to the end of the nonmetal element.
4. Use a Roman # for transition metals and Group IV cations. Except for Ag +1, Zn +2, Cd +2.
91
New cards
Writing Binary Covalent Compounds

1. Write the least electronegative element first and most electronegative element last.
2. The prefix before the names of the elements tell the number of atoms for each element and the subscript use.
3. DO NOT USE CHARGES!!!!!!!
4. DO NOT CRISS-CROSS!
92
New cards
Naming Binary Covalent Compounds

1. __Do not__ use prefix on the first element if only __one__ atom is present.
2. If __more than one atom__ of the first element is present, use a prefix with it.
3. __ALWAYS__ use a prefix before the second element’s name!
4. Add “ide” to the ending of the second element.
93
New cards
Naming Binary Acids
Hydro-nonmetal-ic.
94
New cards
Naming Ternary Acids
\-DON’T use the prefix hydro-

\-Use the stem of the polyatomic and change the ending to…


1. -ate changes to -ic
2. -ite changes to -ous
95
New cards
Synthesis
A + X→AX
96
New cards
Decomposition
AX→A + X
97
New cards
Single Replacement
A + BX → AX + B
98
New cards
Double Replacement
AX + BY → AY + BX
99
New cards
Combustion
Hydrocarbon + O2 → CO2 + H2O
100
New cards
Diatomic Elements
F2, Cl2, Br2, I2, O2, N2, H2