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Honors Chemistry 1st Semester Review
Scientific Method - Observe• Observation – the receiving knowledge or
data through the senses, or from scientific instruments
• Inferences – Assumptions based on observations.
• Example:– Observation: Car won’t start in the morning.– What would you assume (or infer) the problem is?
Scientific Method - ObserveObservations:• 1. Qualitative
– Do you like this powerpoint?• Usually uses the five senses.
• 2. Quantitative– How many words are on this
powerpoint?• Usually can be answered precisely.
Scientific Method - Hypothesis
Hypothesis : a statement that answers a question
(a possible explanation)
Tells what are the independent and dependent variables and how to measure
them.
How do Scientists Communicate? By sharing information.-Poster sessions-Presentations at conferences/meetings-Scientific Journals-Shared Data Bases - Internet
What happens when scientists disagree?Scientific arguments are solved through further observation and experimentation
To reveal data trends, data is placed in graphs
Time (min)
Temp. (˚C)
0 01 02 03 54 105 156 207 258 259 30
10 30
Temperature Change over Time
05
101520253035
0 1 2 3 4 5 6 7 8 9 10
Time (min)
Tem
p (
C)
Finding Volume of Irregularly shaped items
This is called Water Displacement
The Graduated CylinderMeasures Volume
Start by locating the meniscus
Always make your reading at the bottom of the meniscus!!
Finding Density
Density is a ratio between mass and volume.
You need to divide to find the ratio. Density = mass divided by volume
OR D = M/V
Electronic BalanceMeasures Mass
Turn balance on Make sure it reads “0” Place item on balance Obtain mass Turn balance off
SI Unit for mass is the kg
SyllabusWhat is Chemistry?
Chemistry is the study of matter and energy and the interactions between them.
Chlorine – gas will kill you
Sodium – metal reacts violently with oxygenIt is stored in oil.
Sodium + Chlorine= Table Salt which our bodies need
Pure vs. Applied Science• BOTTOM LINE:
• Pure Science is just for the knowledge.
• Applied Science is for someone to make money off of the invention (new technology)
What IS science based on?
•Experimentation
•Observation
Rules for significant figures:
(1) All nonzero digits are significant (1-9):1.234 g has 4 significant figures1.2 g has 2 significant figures
(2) Zeroes between nonzero digits are significant:1002 kg has 4 significant figures3.07 mL has 3 significant figures
(3) Leading zeros (left) of the first nonzero digits are NOT significant; They indicate the position of the decimal point:
0.001°C has only 1 significant figure0.012 g has 2 significant figures
(4) Trailing zeroes (after a decimal point) are significant:
0.0230 mL has 3 significant figures,0.20 g has 2 significant figures.
(5) When a number ends in zeroes that are not to the right of a decimal point, the zeroes are not necessarily significant:
190 miles may be 2 or 3 significant figures50,600 calories may be 3, 4, or 5 sig figures
• The potential ambiguity in the last rule can be avoided by the use of standard exponential, or "scientific," notation.
• What is an "exact number"?
• Some numbers are exact because they are known with complete certainty.
• Most exact numbers are integers: exactly 12 inches are in a foot, there might be exactly 23 students in a class.
• Exact numbers are considered to have an infinite number of significant figures.
• Rules for mathematical operations• In calculations, the general rule is that the accuracy of a calculated
result is limited by the least accurate measurement involved
1) In addition and subtraction, the result is rounded off so that it has the same number of digits as the measurement having the fewest decimal places (counting from left to right). For example,
101 (3 sig figures) + 23.643 (5 sig figures) = 124.643, which should be rounded to 125 (3 sig figures).
302.1 + 54.345 = 356.445,which should be rounded to 356.4 (least shared decimal place)
2) In multiplication and division, the result should be rounded off so as to have the same number of significant figures as in the component with the least number of significant figures. For example,
3.0 (2 sig figures ) × 12.60 (4 sig figures) = 37.8000
which should be rounded to 38 (2 sig figures).
Temperature
Converting between ºC and K
Example
Practice
• ºC = K – 273• K = ºC + 273
• Normal human body temperature is 37 ºC. What is your temperature in K?
• Surgical instruments must be sterilized at 170 ºC. What is this in K?
Physical and Chemical Changes
Physical Changes: Do not alter the identity of a substance
Crushing, tearing, changes of state (solid to liquid to gas)
Chemical Changes: Alter the identity or chemistry of a substance
Burning, cooking, rusting
What is Matter?
Matter is anything that has mass and volume
States of Matter
Liquid has undefined shape but defined
volume
Pure Substances – Element Matter that can not be broken down into
simpler substances under normal lab conditions
Contains only one kind of atom Atom Molecule
Elements (symbols) Na, Au, C Where can you find a list of all the
elements?
Mixtures: Homogeneous Mixture with no visibly different
parts. Sea water - H2O + NaCl Air - N2 + O2 + CO2
Physical and Chemical Changes
Is this a physical or a chemical change? Explain your reasoning.
New substances formwhen there is a chemical change.
ATOMIC THEORIES J.J. Thomson 1897 Experiment - discovered electrons
Atom is made up of charged matter
ATOMIC THEORIES Ernest Rutherford: 1910 – Planetary Model Atom is mostly empty space Found the nucleus (a small dense region of positively
charged particles).
If the nucleus were the size of a marble, Then the atom would be the size of Cardinal’s stadium Theorized about the neutron – not proven until 1932
RUTHERFORD – GOLD FOIL EXPERIMENT DISCOVERED THE NUCLEUS
ATOMIC THEORIES John Dalton – 1808
Atomic Theory:1. Elements are made up of tiny particles called atoms.2. Atoms of one element are identical.3. Atoms of other elements are different from each other.4. Atoms can combine to form compounds.5 Atoms are not created, nor destroyed, but can change they way they are grouped together.
Periodic Table Trends The most important difference
between Mendeleev's table and today’s table:
the modern table is organized by increasing atomic number, not increasing atomic weight.
Why was the table changed? Discovery of isotopes and ions.
PERIODIC TABLEAtomic Number = Number of Protons
Hydrogen – 1 proton = #1 Helium – 2 protons = #2 Gold – 79 protons = #79
Rules: All elements on the period table are neutral.
Therefore, #of protons = #of electrons What about neutrons – we’re coming to that
later
Periodic Table Trends Groups – Columns
Elements within a group share several common properties.
Groups have the same outer electron arrangement.
Like families, the share the same characteristics
Periodic Table Trends Metals Most of the elements are metals. You see metals every day. Aluminum
foil, gold, silver. If someone asks you whether an element is a metal, metalloid, or non-metal and you don't know the answer, guess that it's a metal.
Properties of Metals lustrous (shiny) malleable (can be hammered) good conductors of heat and electricity
Periodic Table Trends Group 18: Noble Gases Helium and neon are examples of noble
gases. These elements are used to make
lighted signs, refrigerants, and lasers. The noble gases are not reactive.
He Never Argued with Superman Xenon’s a Nurse.
Periodic Table Trends Group 17: Halogens (Examples of halogens are
chlorine and iodine.) You find these elements in
bleaches, disinfectants, and salts. highly reactive.
What does this mean and why do we care?
Properties of atoms correlate with the number and energy of electrons
Atoms like to have full outer shells
Valence electrons have the most energy (this is where all the action occurs)
This will help us predict what reactions may occur when we start mixing elements together
Note periodicity of charges
Main Group Elements & Their Ions
Periodic Table – Long Form
PERIODIC TABLE Atomic # = # of Protons Symbol
Atomic Mass
PERIODIC TABLEIsotopes: elements with a different number of neutrons.
Elements have to have the same number of protons to be the same element.
ATOMIC THEORIES Mass Number
ProtonsNeutrons
NOT Electrons(too small to want to count)
PERIODIC TABLE Atomic mass
Review: What does one proton weigh? 1 atomic mass unit (amu) What does one neutron weigh? 1 amu What does one electron weigh? So small we will consider it to be zero
PERIODIC TABLE Atomic # = # of Protons Symbol
What is this?
PERIODIC TABLE Why the weird number?
We know that Lithium has 3 protons 3 amu We assume it has 3 neutrons 3 amu We assume the electrons are zero mass. So we total 6 amu. Where is the 0.941
coming from? Isotopes 6.941 is the average of all the naturally
occurring isotopes of lithium.
ELECTRON CONFIGURATION
Li-, Mg 2- Cu2+, F+
Note periodicity of charges
Main Group Elements & Their Ions
PERIODIC TABLEIsotopes: elements with a different number of neutrons.
How do we write isotopes? 14C
Alka
liAl
kalin
e Ea
rth
Transition Metals
Chal
coge
nsHa
loge
nsNo
ble
Gase
s
Periodic Table Trends Nonmetals upper right side of the periodic
table (Yellow) The halogens, the noble
gases, and the rest. Poor conductors of heat and
electricity. Solid nonmetals are brittle and
lack metallic luster.
Hund’s Rule: electrons will not share an orbit until needed
White Board PracticeLewis Symbols or Lewis Dot Diagrams• We place the electrons on four sides of a
square around the element symbol.
Practice:O Na Ca Ba
Ne H I Cs
• Check with your partner
Shorthand If it is in a row past a noble gas,
we can use that for a shortcut.
Short-hand Notation[Ne] 3s1
[Ar] 4s2, 3d1
[He] 2s2, 2p5
Energy NotesEnergy – Capacity to do work or produce
heat
– Capacity to move or change matter
Types of Energy• Stored
– Energy of position (water wheel, book on shelf)– Chemical energy (gas, food, batteries)
• Motion– Mechanical energy (moving parts of
machines)– Sound: vibration of molecules
• Radiant (EMR)Thermal energy (Sun’s heat)
Light
Potential
Kinetic
ENERGY• Energy can be converted from one form to another.
• Law of Conservation of Energy:
• energy is not created nor destroyed, but can CHANGE from one form to another.
• 3 examples of Chemical Energy.
ROYGBIV – backwards – R least energy
Wednesday – October 24• Rube Goldberg Poster –
Presentations
How do atoms release energy?Energy In Energy Out
Heat and TemperatureExothermi
c
Endothermic
• System that releases energy into its surroundings
• Release energy because a change has occurred
• Combustion reactions
• System that takes energy in as heat from the surroundings
• Needs energy from outside source in order for a change to occur
• Changing water to steam Or melting ice
How do we measure energy?
SI Unit: Joule (J)
1 Calorie = amount of energy required to raise 1g of water by 1°C
1000cal = 1 kilocalorie = 1Cal = food Calories
Conversion Factor1 calorie = 4.184 Joules
Calculating Energy
Specific Heat Capacity or Specific Heat:The amount of energy required to change the temperature of 1 g of substance by 1̊CUnits are: J (Joule) g ̊C Centrigrade NOT Calories
It takes different amounts of energy to heat different substances.
Phase Diagram - Overview
Phase Change diagram
sublimationdeposition
ExothermicEndothermic What definition are we missing?
Q= mCT• Example
4
• Practice 4
• What is the specific heat of lead if a 30.0 g piece of lead undergoes a 250ºC change while absorbing 229.5 calories?
• 0.0306 cal/gºC = sigfigs? • 3.06x10-2 cal/gºC• What is the specific heat of
an unknown substance if the addition of 950 J of heat energy caused a 20 gram sample to warm from 18ºC to 42ºC?
1.97 cal/gºC = sigfigs? 2.0 cal/gºC
Writing Formulas for Ionic Compounds• Crisscros
s Method
• Example
• Write the element symbols for the cation and anion, with the cation on the left and the anion on the right.
• Write each ion’s charge as a superscript.
• Crisscross the two charges moving them downward diagonally from one superscript to the other subscript.
Naming Binary Ionic CompoundsName Formula
Example:Calcium ChlorideCa +2 and Cl -1
CaCl2
1. Identify the ions involved2. List the cation first and
then the anion3. Determine that charge of
each ion involved4. Balance the charges so
the compound is neutral.
Naming Binary Covalent Compounds
Prefixes 1= mono (can be omitted – assumed)2= di3 = tri4 = tetra5 = penta6 = hexa7 = hepta8 = octa9 = nona10 = deca
Naming Binary Covalent Compounds
PracticeName Formula
What is the formula for the following compounds?
1. Write the chemical formula of the first element listed.
2. Write the prefix number as a subscript.
3. Write the chemical formula of the second element listed.
4. Write the prefix number as a subscript.
a. Pentachlorine dioxideb. Carbon monoxidec. Tribromine hexasulfide
Naming Binary Covalent Compounds
PracticeFormulaName
What is the name of the following compounds?
1. Write the number of the first element as a prefix, add the name of chemical.
2. Write the number of the second element as a prefix, add the name of chemical and end in –ide.
a. P4C8
b. F9I6
c. SN3
• Solids are usually soft• low melting points• low boiling points• Properties arise because molecules are
not strongly held together• Usually found with nonmetals
Properties of Covalent Bonds
• Ionic bonds are very strong (separating ions requires lots of energy)
• High melting points, boiling points• Crystals are hard and brittle• Electrical insulators when solid, electrical
conductors when molten or dissolved in water• Between a metal and a non-metal
Properties of Ionic Bonds
Why do atoms form bonds?Octet Rule
Lewis Dot Diagrams
Atoms tend to gain, lose, or share electrons in order to acquire a full set of valence electrons.
• Used to illustrate valence electrons
• Used to illustrate how electrons rearrange during chemical reactions (when bonds are formed or broken)
Review: Ions • What are Ions?• Ions are formed by adding or subtracting electrons
from a neutral atom or molecule.
Cation: positive charge Anion: negative charge (remove electrons) Na+ (add electrons) Cl-
Naming Binary Covalent Compounds
PracticeFormulaName
What is the name of the following compounds?
1. Write the number of the first element as a prefix, add the name of chemical.
2. Write the number of the second element as a prefix, add the name of chemical and end in –ide.
a. P4C8
b. F9I6
c. SN3
ORGANIC • In Chemistry, Organic means it has a carbon atom in it.
• Question: can there be an organic ion? NO – carbon does not form ions.• Can there be organic covalent bonds? YES – all carbon bonds will be covalent and therefore they will be organic.
Carbonated Drinks
• Carbonate: special group of polyatomic ion• CO3
2-
• What kind of Ion does • It need to balance?• 2+ like what family?• Alkaline Earth Metals• How many Carbon molecules? 1