introduction to chemistry chapter 11. student learning objectives distinguish between physical &...
TRANSCRIPT
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Introductionto
Chemistry
Chapter 11
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Student Learning Objectives
• Distinguish between physical & chemical properties
• Classify, compare, name, & identify
chemical quantities
• Recall properties of solubility
• Apply trends in the periodic table.
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What is chemistry?
Chemistry is the study of microscopic properties.
Chemical properties
“Invisible”
How and why atoms combine into molecules
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What are some physical and chemical properties?
Physical Properties(Macroscopic)
• Density• Phase
• Appearance• Size
Chemical Properties(Microscopic)
• Atomic make-up• Structure• Reactivity
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Practice
1) How many different medicines exist for pain relief?
2) Is surface tension a microscopic or macroscopic property of matter?
3) What does the image show?
Is it an example of a physical
or chemical property?
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More Practice
4) Name the macroscopic properties of water.
5) Name the microscopic properties of water.
6) How do carbon dioxide (CO2) and water (H2O) compare and contrast?
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Some ChemicalChange Indicators
The primary difference between a physical change and a chemical change is that a chemical change produces a new substance.
Color change
Production of a Gas
Temperature Change
Light
Sound
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How are elements, molecules, compounds& mixtures defined?
Question: What are the origins of the elements?
Element all of one type of atom
Molecule atoms in a chemical bond
Chemical bond attraction between atoms
Molecular Formula relative numbers of atoms in bond
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A compound contains two or more types of atoms.
Type Number of Atoms
Diatomic 2Triatomic 3Polyatomic 4+
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Practice
1) Which is not a compound?
2) How many atoms are contained in each?
3) Classify as diatomic, triatomic, or polyatomic.
H2O CaF2 NH3 O2
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Classifying Mixtures
A substance that is pure has only one type of element, or molecule, present.
CopperSalt
A mixture contains two or more distinct types of substances (atoms/molecules).
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Homogeneous Mixture
Same uniform appearance and composition throughout
Solution
(same phase)
Heterogeneous Mixture
Consists of visibly different substances and/or phases
Suspension
(particles settle)
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Practice: Classify Each Substance
7-up
Aluminum
Homogenized milk
Raw milk
Oil and water
Carbon monoxide
Distilled water
Air
Tap water
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How can mixtures be separated?
Water may cross a semi-permeable
membrane. (Osmosis)
Osmosis: from less to more concentrated
Reverse osmosis: from more to less concentrated
Filtration separate liquids and solids
Distilation separate gasses, liquids, solids
Desalination combines distillation and reverse osmosis
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Question
Why are distillation and desalination typically not used to obtain fresh water from salt water?
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What is solubility?
Solubility is a measure of how much solute will dissolve in a solvent to produce a stable solution.
Water & Sugar
Solvent (larger amount) Does the dissolving
Solute (smaller amount) Dissolves
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Oil & Water
Liquids may be miscible or immiscible.
(mix or not mix)
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Solubility is variable.
• Bond Strength• Bond Types• Temperature• Pressure• Molecular attractions
Solubility has a limit, based on each individual substance and physical conditions.
Concentrated
Dilute
Saturated
Concentration = Grams Liter
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Practice1) If you cannot dissolve anymore sugar in your coffee,
your coffee is?
2) What is the concentration when 5 grams of sugar is added to ½ a liter of water?
3) If you have 30 mL of 25% HCl solution, how many grams of HCL are in the solution?
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What are the basic trends in the periodic table?
The periodic table is periodic!
Most of the elements in the periodic table are metals.
ShinyOpaque
Good Conductors
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Trends
• Chemical reactivity decreases L R
• Radius decreases along a period L R
• Ionization energy increases along a period L R
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Practice
1) Which metals are liquid under normal atmospheric conditions?
2) Which of the following would be most reactive?
a. O b. He c. Al d. Cl
3) Which of the would have the smallest radius?
a. Al b. Cl
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Atomic Periods (rows) are periodic.
Atomic Groups (columns) have similar trends.
1 amu = 1.661 x 10-24 grams
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Group Name AttributesIA Alkali Metals Highly ReactiveIIA Alkali Earth Metals
Middle Transition Metals High Melting PointIIIA Metalloids Metals/ Non-metalsVIA Ore Forming ElementsVIIA Halogen Gases Salt Forming ElementsVIIIA Noble Gases Non-Reactive
Emerald is a variety of beryl, a mineral that contains the
alkaline earth metal beryllium.
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Lanthanides (58-71): found in geologic zones
Actinides (90-103): most are synthesized in labs
A Uranium Rock
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Practice
1) In which group are the precious metals?
2) List all attributes of Bromine (Br) that can be determined using the periodic table.
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What does the shell model indicate?
No two electrons can have the exact same energy state. (Pauli Exclusion Principle)
Electrons are arranged in particular orbitalsEach electron has its own set of quantum numbers (n,l,ml, ms)
which determine the energy state of the electron
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Atomic period indicates the number of main energy shells available in the ground state.
Shell Maximum e-
Allowedn = 1 2n = 2 8n = 3 8n = 4 18n = 5 18n = 6 32n = 7 32
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Practice
Draw the electron configuration for each atom. (Assume atoms in ground state)
1. N 2. Kr 3. Mg 4. O
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Electrons attempt to have configurations that match those in group VIIIA. (Octet Rule)
Valence electrons are what make the physical and chemical properties of the atoms in a group similar.
8 − Group Number = Number Unpaired e–
Valence Electrons
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More unpaired electrons = more reactive
Unpaired valence electrons are used to form chemical bonds
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What are some rules for naming compounds?
Compounds
Metal is named first and then the Non-metal
NaCl = Sodium Chloride HF = Hydrogen Fluoride
Prefixes
CO2 = Carbon Dioxide
1. Mono2. Di3. Tri4. Tetra5. Penta6. Hexa7. Hept8. Oct
“Left” then “Right + ide”
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Polyatomic Ions
Polyatomic Ions are molecules made up of two or more atoms that are considered an ionic group, that have charge.
1. Name the cation (+ ion) first
2. Name the anion (- ion) second + ate
CaCO3 Calcium Carbonate
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PracticeWhat is the chemical name?
Does it have a common name?
1. O2 5. SF6
2. H2O 6. CH4
3. KBr 7. NH3
4. O3 8. PCl5
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Practice with Polyatomic Ions
What is the chemical name?
Does it have a common name?
1. AlPO4 4. Fe(NO3)2
2. Cu2SO4 5. NaHCO3
3. KClO3 6. NaH2PO4