ch 2 chemistry- properties & the transformations (chemical reactions) of all forms of matter...
TRANSCRIPT
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Ch 2
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Chemistry- properties & the transformations (chemical reactions) of all forms of matter
Matter is ….anything that takes up space or has mass.
Matter is made of elements.
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How are atoms studied?
• Atoms smallest unit of matter “indivisible
• Atoms too small in size to study easily
• Size of Earth : soda can = soda can : atom
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Who studied the atom?
• Studied by many scientists for centuries– Democritus (400 BC) – phrase “atomos”– Rutherford (1911) – nucleus (gold foil expt)– Moseley (1913) – X-rays to find atomic #– *Bohr (1913) – planetary model of the atom– *Schrödinger (1923) – electron cloud
model
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What is the structure of an atom?
Bohr Model
“Planetary Model”
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Structure• Nucleus – center of atom
– Protons and Neutrons
1. Proton–positive (+) charge–relative mass 1–Determines atomic number
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2. Neutron• no (0) charge• relative mass 1• Determines isotope
–Isotopes are two of the same element with different masses (and diff # of neutrons)
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3. Electron– negative (-) charge
– relative mass of 0 (zero)
– Determines ion
– Found outside the nucleus• Bohr model – electrons are in specific
energy levels
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Electron shells
• determine how atom behaves when encounters other atoms
• Valence shell- outer shell
• Placed according to rules• 1st shell holds up to 2 electrons• Each shell after can hold up to 8• Most stable octet rule- 8 in valence shell
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Structure of Atoms
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Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons
C would like to N would like toO would like to
Gain 4 electronsGain 3 electronsGain 2 electrons
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Element-
• Pure substance, one type of atom
• Represented with symbol(s)
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Atomic number equals the number of ____________ ________________.Atomic mass equals the number of ______________ + .
Atomic NumberSymbolNameAtomic Mass
protons
protons neutrons
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How are P, N, e- related?
• # protons = atomic number
• # electrons = # protons in a neutral atom
• # protons + # neutrons = atomic mass
• # neutrons=atomic mass -atomic number
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Electron Dot Structures
Symbols of atoms with dots to represent the valence-shell electrons
1 2 13 14 15 16 17 18
H He:
Li Be B C N O : F :Ne :
Na Mg Al Si P S :Cl :Ar :
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Compound- substance formed when two or more elements combine
Molecule- smallest particle of a compound
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IONIC BOND- giving and taking of electrons- forms ions- charged particles
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Covalent Bond
• Sharing of electrons
Non-polar covalent bond – equal sharing of electrons
Polar covalent bond – unequal sharing of electrons ex. water
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Bonding
Covalent bonding
Polar covalent bond
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Hydrogen Bond
• Weak chemical attraction between polar molecules (water molecules)
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Water – Chapter 2.3
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Properties of Water
• Transparent• Universal solvent• Cohesion and adhesion• High heat capacity• High boiling point• Evaporative Cooling• Less Dense as ice/solid
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1. Transparent
• Light passes through (reach aquatic plants)
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Solute – substance dissolved in a solvent forms solution
Solvent – fluid that dissolves solutes
ex. Substances dissolved in blood
2. Solvent of Life- many compounds dissolve in water
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- Cohesion- Water molecules stick together due to H bonds- Adhesion- Stick to other molecules
3. Cohesion and Adhesion
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capillary action- water pulled to top of trees (adhesion)
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4. High Heat Capacity
- Takes a lot of energy to raise the temp of water because h bonds
- helps maintain body temp
Water is cooling!Do I look
cool?
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5. High Boiling Point
• A lot of energy needed to pull apart water molecules, rare when boiling occurs in nature
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6. Evaporative Cooling• The cooling of a
surface occurs when liquid evaporates
– Moderating earth’s climate
– Preventing overheating
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Molecules spread apart as temp goes down
- or all aquatic animals would die in winter
7. Less Dense as solid
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So can you name all of the properties of water?
TransparentAdhesion
Cohesion
capillary action
high surface tension
holds heat to regulate temperature (High heat capacity)High Boiling PointEvaporative Cooling
less dense as a solid than a liquid
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Restate Questions
• Pg 30 1-3
• And pg 33 1 and 2
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Acids and BasesAcids and BasesAcids and BasesAcids and Bases
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Acids
Taste Sour
pH less than 7
Corrode metals (produce H gas with some metals)
Neutralize bases
Turns blue litmus paper red “Blue to Red A-CID”
Turn bromthymol blue to yellow
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Bases
• Taste bitter, chalky• pH greater 7• Turn litmus paper blue• Turn bromthymol blue to blue “basic blue”• Slippery to touch• Neutralize acids• Many soaps, antacids
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Acids and BasesStrength compared using pH scale
Ranges from 0 – 14
Acid – donates H+ to the solutionRanges from pH 0-6.9
Base – removes H+ from the solution by donating OH-
Ranges from pH 7.1 – 14
Distilled water is pH 7.0 or neutral. Why?
H2O H+ + OH-
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Chapter 2 Chemical Principles
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Chapter 2 Chemical Principles
Acids and Bases
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Neutralization- reaction b/n acids and bases
• Remaining ions from acid and base combine to form a salt
• Salt- any substance formed along w/water in a neutralization reaction.
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• come up with 7 questions that would be good on the test over chapter 2.
• High Order thinking
• At most four multiple choice
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Cells and Nutrition
• nutrients- chemicals that organisms use for energy
development, growth, and tissue repair
• Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus and Sulfur made up 98% mass of living organisms (CHNOPS)
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A. Carbohydrates (sugars and starches)
1. Simple Sugars- monosaccharide- made of one sugar molecule. ex glucose
2. Complex Sugars- disaccharide, ex Sucrose (table sugar) made of two simple sugars. glucose and
fructose3. Starches- polysaccharide (poly= many) made up of long chains of simple sugar molecules combined together
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B. Lipids
• when body has excess carbs converts to fats.
- fats store energy more efficiently than carbs
- make up part of the plasma membrane
- include oils, waxes, steroids, and other water insoluble organic compounds
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C. Protein
• composed of long chains of amino acids• 20 different types of amino acids in humans
Two functions 1. Build types of tissue - and repair of cell
a. ex cartilage tendons made of collagen
b. hair and nails made of a different protein called keratin
c. proteins in the cell membrane
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2. Regulate rate which chemical reactions take place by acting as enzymes
-made in ribosomes-amino acids connected to make specific proteins.
-blueprint stored in DNA
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D. Nucleic Acids
• - Two types of nucleic acids DNA and RNA
•
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1. DNA- Deoxyribonucleic acid- double strand of nucleotides (double helix)
- Long chain of nucleotides (3 parts)a) sugar (deoxyribose= DNA) b) phosphate groupc) base - one of four
1. adenine (A)2. thymine (T) 3. cytosine (C)4. guanine (G)
- A pairs with T- G pairs with C
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2. RNA Ribonucleic acida) sugar (ribose)b) phosphate groupc) base
1. adenine (A)2. uracil (U)3. cytosine (C)4. guanine (G)
- A pairs with U- G still pairs with
C
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Homework
• PG 33 # 3
• Pg 37 1,3,4,5
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2.4 Energy and Chemical Reactions
• Organisms need Energy for Life Processes (stored, power metabolism, build cell structures)
• Energy- ability to do work
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Examples- Light- radiant energy in waves- Heat- molecular motion of matter ex. Rubbing hands
- Chemical- stored because of chem makeup
- electrical energy- electrons through a conductor
- mechanical energy- moving objects perform work ex. Sound, pedals turning bike
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energy can be stored or released by chemical
reactions- chem bonds broken and new
formeda) Reactants =starting materials in chem reaction
b) Products = newly formed substances
Reactants------> ProductsNaCl---> Na+ + Cl-
- activation energy - energy needed to start a reaction
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•metabolism- all chemical reaction occur in a organism
- get most energy from food
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Enzymes (protein)- increase speed of chemical
reactions- most proteins- act as catalysts- reduce
activation energy - Helps maintain homeostasis- allows body to breakdown CO2
quickly- only bind to certain substrates***Temperature and pH affect
enzyme activity *
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Homework Restate
• PG 42 1-3
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