0
Q
Identify Matter vs. Non-matter?
A
- Matter: Anything that has mass and occupies space
- Non-matter: Anything that does not have mass and/or does not occupy space
- Example: Light, heat, air
1
Q
What is Chemistry?
A
-The study of the composition of matter and the changes that matter undergoes
2
Q
List the Steps of the Scientific Method
A
- Make observations
- Proposing 2 hypotheses (one is null)
- Experimentation
- Form a theory or Scientific Law
3
Q
Identify the manipulated, responding, and control variables in an experiment
A
- The manipulated variable in an experiment is the independent variable because it is changed
- The responding variable is the dependent variable because it reacts depending on the independent variable
- The control variables in an experiment are the things that are kept constant during an experiment such as heat, an amount of something, etc.
4
Q
Identify extensive and intensive properties
A
- Extensive: A property that depends on the amount of matter in a substance (mass, volume, height, length)
- Intensive: Do not depend on the amount of matter present (malleability, color, boiling point, melting point/freezing point, density)
5
Q
Compare the properties of solids, liquids, and gases
A
- Solids: Definite shape, definite volume, particles packed tightly together, almost incompressible, expands when heated
- Liquids: No definite shape, particles flow freely, fixed volume, almost incompressible, expands when heated
- Gases: takes shape and volume of container, particles are spread out, easily compressible.
6
Q
Define physical and chemical change
A
- Physical change: some properties of a material change, but the composition of the material does not change
- Chemical change: Any change that results in the formation of a new chemical substance
7
Q
Provide examples of physical and chemical change
A
- Physical: Ice melting to become water, water freezing into ice
- Chemical: mixing sodium and chlorine to made sodium chloride/ salt (NaCl)
8
Q
Explain why a physical change is reversible or irreversible
A
- Irreversible: cannot go back to normal (burned paper cannot be turned back into paper)
- Reversible: cannot go back to normal (ice can be turned back into water)
9
Q
Explain how chemical reactions can be identified
A
- Production of Gas
- Production of precipitate
- Color change
- Transfer of Energy
10
Q
Identify the reactants and products of a chemical change
A
- Reactant: a substance present at the start of the reaction
- Product: A substance produced in the reaction
11
Q
Define the law of conservation of mass
A
-Law of conservation of mass: In any physical change or chemical reaction, mass is conserved
12
Q
Explain how the law of conservation of mass applies to both physical and chemical changes
A
- Physical change: The product before and after the change will weigh the same (has the same mass).
- Chemical change: In a chemical reaction, the mass of the products is always equal to the mass of the reactants.
13
Q
Determine the atomic number and mass of an electron
A
- Compares the relative masses of all elements to carbon-12. #= weighted average of all isotopes of an element. (It’s units are called atomic mass units)
- Atomic #= number of protons
14
Q
Calculate atomic mass of an element from the mass and percent of each isotope
A
-Atomic mass (isotope’s mass x % natural abundance)
15
Q
Explain how electrons move from one energy level to another
A
- For electrons to move from a lower energy level to a higher energy level, they absorb energy while emitting light
- For electrons to move from a higher energy level to a lower energy level, they release energy while emitting light
16
Q
Rutherford’s Atomic model vs. Bohr Model
A
- RAM: Only explained a few simple properties of the atom
- RAM: Could not explain the chemical properties of an element
- RAM: Could not explain why elements heated to higher temps give off colored light
- BM: Showed how energy of an atom changes when absorbing or emitting light
- BM: An electron is only found in specific circular motions, or orbits, around the nucleus
- BM: Explains that when an atom emits light it is moving from one energy level to another
- BM: Each orbit has a different energy level and fixed energy
- Both have something to do with energy
17
Q
Bohr Model vs. Quantum Mechanical Model
A
- BM: Only explained the energy in simple atoms like hydrogen
- QMM: Mathematical equation to describe the behavior of an electron in a hydrogen atom
- QMM: Does not specify the exact path of an electron around the nucleus
- QMM: Orbitals use probability to predict a region of space where an electron is found at any given time
- BM: 2D, QMM: 3D
18
Q
How to write an electron configureation
A
- Ways to show
- Aufbau diagram
- Standard Electron Configuration
- Orbital filling diagram
- Electrons occupy the lower energy levels first (Aufbau principle)
- To be in the same orbital, electrons must have opposite spin (Pauli exclusion principle)
- Ever orbital subshell gets 1 electron before receiving another and have parallel spin ( Hund’s rule)
19
Q
Explain why elements and compounds release different colored light
A
- The orbitals contain different energy levels when they are transferred
- Red= lowest
- Purple= highest
20
Q
Who created the periodic table?
A
- Mendeleev
- Based on increasing atomic mass
21
Q
Identify a substance as a metal, metalloid, or nonmetal
A
- Metal: shiny, malleable, good conductor of electricity, ductile, mostly solid at room temp
- Non-Metal: dull, brittle, poor conductor
- Metalloid: depending on conditions can act like metal or nonmetal, poor conductor
22
Q
Determine the number of valence electrons in an element
A
- Look at its group number
- The number of electrons on the outside energy level of an element
23
Q
Alkali Metals
A
-Most Reactive Metals (Group 1 A)
24
Alkaline Metals
- Relatively soft
- Harder than alkali metals
- Group 2a
25
Halogens
-A nonmetal in group 7A
26
Nobles Gases
-An element group in 8a of periodic table
27
Transition metals
-One of the group B metals
28
Inner Transition Metals
-An element in the lanthanide or actinide series
29
Percent Error Formula and Error Formula
- Iexperimental value - true valueI
| - IerrorI/accepted value x 100%
30
Si Base Units
- Distance: Meters
- Temperature: Kelvin
- Density: Kilograms
- Volume: Liters
- Time: seconds
31
Converting temperature from Kelvin to Celsius and vice versa
- Kelvin= Celsius + 273
| - Celsius= Kelvin -273
32
What is the lowest possible temp on the kelvin scale?
-Absolute 0
33
Tera
-10^12 times larger (T)
34
giga
-10^9 times larger (G)
35
Mega
-10^6 times larger (M)
36
Kilo
10^3 times larger (k)
37
Hecto
10^2 times larger (h)
38
Deka
-10^1 times larger (da)
39
Deci
-10^-1 times smaller (d)
40
centi
-10^-2 times smaller (c)
41
milli
-10^-3 times smaller (m)
42
Micro
-10^-6 times smaller (upside-down h)
43
Nano
-10^-9 times smaller (n)
44
Pico
-10^-12 times smaller (p)
45
Mass, Volume, and Density formulas
- Density= Mass/ volume
- Mass= Density x Volume
- Volume= Mass/ density
46
Rules for Addition, Subtraction, Multiplication, and Division of Sigfigs
Multiplication and Division: Count # of sigfigs in each #, round to that many sigifgs
Addition and Subtraction: Answer rounded to the number with the least number of decimal places
47
What is an atom?
- The smallest particle of an element that retains its identity in a chemical reaction
- Mad up of subatomic particles (protons, neutrons, electrons)
48
What makes the atoms of each element unique?
-It's atomic number, aka how many protons it has
49
Explain why Daltons Atomic Theory is true or flase
- True: All matter consists of tiny particles
- False: Atoms are indestructible and indivisible
- False: Elements are characterized by the mass of their atoms (atoms nuclear charge)
- True: When elements react, their atoms combine in whole-number ratios
50
Similarities and Differences between isotopes of the same element
- Similar: # of electrons, # of protons, react the same in chemical reactions
- Different: # of neutrons
51
Plumb Pudding Model
- created by Thompson
- Positively charged atom with negative particles scattered throughout
- No movement
- No nucleus
- No orbitals
52
Rutherford's Atomic Model
- Discovered through the gold foil experiment
- Positively charged nucleus
- Electrons orbit nucleus
- Movement!
53
Mass number
Protons + Neutrons
54
Number of Neutrons
atomic # - mass Numbers
Chemistry
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