Download Chapter 1 Chemistry: the study of the composition of matter and the

Chapter 1
Chemistry: the study of the composition of matter and the changes it
undergoes (what stuff is made of, and how it reacts)
Chapter 3
Quantitative vs. Qualitative
Pure chemistry: studying chemistry just for the sake of knowing
-Quantitative = QUANTITY = NUMBERS (It is 39 degrees
Organic Chemistry: study of substances containing CARBON
Inorganic Chemistry: study of substances the DO NOT contain carbon
Analytical Chemistry: the study of the composition of substances
Physical Chemistry: study of theories and experiments that describe the
BEHAVIOR of chemicals
Celsius)
-Qualitative = QUALITY = NO NUMBERS (it is hot)
Scientific Notation
-Move the decimal behind the first non-zero digit
-Count the number of ‘jumps’
Biochemistry: study of the chemistry of living organisms
-Jump right? Negative exponent
Scientific Method: a logical approach to the solution of scientific problems
-Jump left? Positive exponent
Steps: Observe, form a hypothesis, experiment, repeat
Accuracy/Precision/Error
Hypothesis: proposed explanation for what is observed
-Accuracy: How close your values are to the ‘true value’
Theory: a broad and extensively tested explanation as to why experiments
give certain results (almost certainly true)
Scientific law: describes a natural phenomenon without explaining the why
-Precision: How close your measurements are to each other.
-Error: ‘How wrong were you?’ … This is the difference between
your value and the accepted value (difference means SUBTRACT)
Chapter 2
-Percent Error: Error/accepted value x 100
Matter: anything that has mass and takes up space
Significant figures
Mass: amount of matter an object contains
KNOW THE RULES!
Substance: matter that has a definite and uniform composition
1.
Physical Property: a quality of an object that can be observed without
changing the substances composition (color, weight, boiling point)
Physical Changes: a change that alters a material without changing its
composition (ex. Water is still water, even when frozen)
2.
3.
4.
Mixture: physical blend of two or more substances
5.
Heterogeneous: not uniform (salad)
6.
Homogeneous: uniform (salt water) also called SOLUTIONS
Phase: any part pf a system with uniform composition and properties
Elements: simplest forms of matter that cannot be separated by chemical
means
Compound: substances that can be separated into simpler substances by
chemical means
Chemical Reaction: when one or more substances change into new
substances
Reactants: the starting substances (the ones that REACT)
Products: the substances formed (or the ones that are PRODUCED)
Chemical property: the ability of a substance to undergo a chemical reaction
and to form new substances
Chemical change: always results in a change of composition of the substance
(burning)
Law of Conservation of Mass: in any physical change or chemical reaction,
mass is neither created or destroyed; it is conserved
7.
Every non-zero digit is significant= 1,234 has 4 significant
figures
Zeros between non-zero digits are significant = 1001 has 4
significant figures
Leftmost zeros before a nonzero digit are NOT significant =
0.000012 has 2 significant figures
Zeros at the end of a number AND to the right of a decimal
point ARE significant 100.23 has 5 significant figures
Zeros at the end with no decimal point are NOT significant =
1,000,000 has 1 significant figure
When adding/subtracting, line up decimal point and round
your answer to the least number of DECIMAL places in the
problem = 2.14 + 2.1 = 4.2 (The answer has 1 decimal place
because that is the lowest number of decimal places)
When Multiplying/dividing, round your answer to the least
number of significant figures
SI system of Measurement
Length = meter
Volume = cubic meter
Mass = Kilogram
Temperature = kelvin
Time = second
Convert!!!
mega (M) 1,000,000 times larger than the unit
kilo (k) 1,000 times larger than the unit
deci (d) 1/10 the size of the unit
cent (c) 1/100 the size of the unit
milli (m) 1/1000 the size of the unit
Atomic Mass Unit (amu): unit for atomic mass
micro ( ) 1/1,000,000 the size of the unit.
Periodic Table
Mendeleev: Arranged by atomic mass
Density
Mosely: arranged by atomic number
Density= relationship between and objects mass and volume
Periods: horizontal rows
Density = mass/volume
Groups/Families: Vertical columns
Temperature
Periodic law: when the elements are arranged by increasing atomic number,
there is a pattern to their properties
Temperature shows us the heat transfer
Group 1A; Alkali Metals
Feels cold to you? Heat going to that object
Group 2A: Alkaline Earth Metals
Feels hot to you? Heat going from object to you
Group 7A: Halogens
Temperature scales
Group 8: Noble Gases
Celsius = based on freezing point and boiling point of water
Metals to the left, nonmetals to the right, metalloids on the zigzag line
Kelvin = based on ABSOLUTE ZERO
Know how to find the # of protons, neutrons, electrons
K = Degrees Celsius + 273
Degrees Celsius = K – 273
What type of questions will you see?
1.
2.
3.
4.
5.
6.
Conversion questions. For example, how many grams in
27.4 kilograms?
Significant figures
a.
Count them, round to a specific significant figure,
add/subtract/multiply/divide
Write in scientific notation
Is it accurate? Precise? What is the percent error?
Be able to solve for the missing value in a density problem
Temperature conversion: kelvin-Celsius and reverse
Chapter 5
Democritus: reasoned that all things were made up of ATOMS
Dalton: developed the ATOMIC THEORY
1.
2.
3.
4.
All elements are made up of atoms
Atoms of the same element are identical
Atoms can be combined with other atoms
Chemical reactions occur when atoms are separated or
combined
J.J. Thompson: ELECTRON
Millikan: charge and mass of the electron
Goldstein: PROTON
Chadwick: NEUTRON
Rutherford: Most of an atom is empty space
Atomic Number: number of protons in the nucleus of an atom (also electrons)
Mass Number: the total number of protons and neutrons in an atom
Neutrons = mass number – atomic number
Isotopes: Atoms with the same number of protons, but different numbers of
neutrons