Basic Chemistry
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Transcript of Basic Chemistry
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BASIC CHEMISTRYATOMS, ELEMENTS AND HOW THEY BEHAVE
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IN THIS UNIVERSE…..There is…….
•Matter – anything that has MASS and takes up space.
•Space – what is not matter.
•Which is there more of????
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WHERE DID MATTER COME FROM?Big Bang
• Approx. 13 BYA• Produced enormous amounts of energy!• Energy eventually “chilled” enough to form basic building blocks of matter
• Evidence???• Expanding Universe• Red-shift• Background radiation
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BUILDING AN ATOMAtoms = basic unit of matterMade of…
• Electrons (e-)• small, no mass, negatively charged
• Protons (p+)• Has mass, positively charged
• Neutrons (n0)
• Has mass, no (neutral) charge
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ATOM STRUCTUREProtons and Neutrons are located near the center of the atom and form the NUCLEUS
Electrons orbit around the nucleus in specific electron orbitals/shells.
Why are electrons attracted to the nucleus?
What keeps the electrons from “crashing in?”
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STRUCTURE OF AN ATOM
P+P+
N
N
e-
Nucleus
Orbit
e-
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STRUCTURE OF AN ATOM
PP
N
N
e
e
Nucleus
Orbit
e
eee
e
e
e
e
e
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EACH ORBIT IS A SPECIFIC
DISTANCE FROM THE NUCLEUS.
PP
N
N
e
e
Structure of an Atom
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KEY POINT!!!!Atoms, can have DIFFERENT combinations of electrons, neutrons and protons!These different combinations makes the atoms BEHAVE differently and have different properties.
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INTRODUCING THE ELEMENTS!
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SO WHERE DID ALL THESE DIFFERENT ATOMS COME FROM????
Telling the story of matter….- Big Bang HUGE amount of energy released- Energy “chills” and starts to form basic building blocks
of matter- First atoms form Hydrogen and Helium.- Hydrogen attracted to other hydrogen Big balls of
hydrogen- FUSION REACTION (aka stars) smaller atoms fuse
together to form heavier elements (carbon, nitrogen, phosphorus sulfur).
- SUPER FUSION In supernovas even heavier elements are formed.
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WHERE THIS LEAVES US!
Approx 5 BYA… - some leftover space debris (matter)
from star cycles start to coalesce in different ways
- Hydrogen collected in center starts a fusion reaction => our sun starts fusion
- Circling debris coalesces to form planets, asteroid belt, moons, etc.
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WHAT WE HAVE ON EARTHAtoms can exist in varying forms on earth- Compounds
- Two or more different atoms bonded together- Ex. H20, CH4
- Elements- substances consisting of only one type of
atom. - A single atom is the smallest amount of an
element you can have. - Ex. O2, H2
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ATOMIC THEORIES AND DISCOVERIES
Dalton: Late 19th century- thought the atom was nothing more than a tiny
indivisible sphere
Rutherford: Early 20th century- Nucleus contains protons and neutrons- Number of protons dictates which element it is.- Electrons circle nucleus in orbits.
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ATOMIC THEORIES AND DISCOVERIES (CONT.)
Neils Bohr- Electron orbits
exist at only certain energy levels (distances) from the nucleus.
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BOHR’S VIEW OF THE ATOM
Each orbit holds only a certain number of electrons
Orbit 1 – max 2Orbit 2 – max 8Orbit 3 - max 8
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BOHR’S VIEW OF THE ATOMValence Electrons: - Electrons in the outermost
orbit- Determine how an atom
“behaves” - atoms with not completely full
valences tend to interact (bond) with other atoms.
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BOHR’S VIEW OF THE ATOM
Elements with full “outer shells” do not react- Noble or “Inert” gases- He, Ne, Ar, Kr, Xe, Rn
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FULL VALENCE = NON REACTIVE
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NOT FULL VALENCE = REACTIVE!
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THE PERIODIC TABLE
Key Points for what the periodic table tells us.Atomic number = number of protonsAtomic Mass=“approximate” number of protons + neutronsIf atom has a charge of zero, Electrons = Protons
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HOW TO READ A PERIODIC TABLE
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YOU TRY ITOxygen
Atomic # _______________
Atomic mass ____________
Number of
p+ ____________
n0 ____________
e- ____________
Sulfur
Atomic # _______________Atomic mass ____________
Number ofp+ ____________n0 ____________e- ____________
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IONS
When we say “atoms” we typically mean a neutral charge
- number protons = number electrons
Sometimes and atom can gain or lose electrons!- now has a positive or negative charge =
ION!
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ISOTOPESSometimes an atom of the SAME element can gain or lose neutrons
- does it change the charge?- does it change how it behaves?
Isotopes = atoms with the same number of protons and electrons but different neutrons
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COMPOUNDSTwo or more atoms bonded together in a set proportion. Ie. CH4, H20, C6H12O6
MOLECULESSingle unit of a compoundContains more than one atom,
BUT can be the same type of atom (O2, N2)
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COMPOUNDSTwo or more different atoms bonded together.Type of bond depends on the number of valence electrons of the atoms involved.
• Ionic•Covalent
Bonding Animations
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TYPES OF BONDSIonic: one atom gives electrons to another, creates opposite charges
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TYPES OF BONDSCovalent: atoms share electrons to get full valences
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BONDING – DEPENDS ON VALENCE E-’S
Atoms will form bonds to get full valencesRemember:
1st level holds 2 electrons2nd level holds 8 electrons3rd level holds 8 electrons
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ATOMS WORKING TOGETHER TO GET FULL VALENCES!Examples: Predict how/what type of bondNa (1Ve) bonds with Cl (7Ve’s)C (4Ve) bonds with 4H (1 Ve each)O (6 Ve) bonds with 2H (1 Ve each)
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TYPES OF BONDS
Which do you think is stronger?•Ionic: two atoms attracted by opposite charges?
OR•Covalent: two atoms holding on to same electrons
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MIXTURES VS. COMPOUNDSCompounds have different properties than any of the elements that make it up
Example:4 H2 (gas) + 2 O2 (gas) 4 H20 (liquid)
•Parts are Chemically bound•Definite proportions required
• Ex. H20 means there are always two hydrogen atoms per one oxygen atom
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CHEMICAL FORMULAS
A chemical formula tells us three things:•What elements are involved•How many atoms of each you have•How many molecules you have
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CHEMICAL FORMULAS
•Ex: 3C6H12O6
•This means there are 3 molecules of (C6H12O6) which is glucose
•1 molecule of (C6H12O6) contains 6 Carbon atoms, 12 Hydrogen atoms and 6 Oxygen atoms
•So how many H’s total are represented in the formula at the top?
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MIXTURES VS. COMPOUNDSMixtures have ingredients that do not chemically bind to one another
•Mixture has same properties as ingredients
•No definite proportions needed•Can easily be separated•Types: solution, suspension, colloid
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TYPES OF MIXTURESSolution – Homogeneous mixture
•equal composition throughout•2 or more substances; solvent and solute •Solute is individual ions or molecules•Solvent is what the solute is dissolved in.•Ex: Saltwater, sugarwater
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TYPES OF MIXTURES
Suspension – heterogeneous•looks uniform when shaken or stirred;
•Separates upon sitting (no agitation)
•Ex. Blood, salad dressing
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TYPES OF MIXTURES
Colloid – •Mixture of very tiny particles of dispersed in another substance;
•Suspended but do not settle out •Ex. Mayonnaise, fog, milk
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THE MOST IMPORTANT INORGANIC MOLECULE OF LIFEWATER!
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PROPERTIES OF WATER- Nearly all of life’s chemical reactions
happen in water.- Water is a pretty special molecule due to
some unique characteristics of the molecule
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WATER- POLAR COVALENT MOLECULE•Share electrons but not equally
• slight (-) charge in the O• slight (+) charge in the H’s of water
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HYDROGEN BONDING: WHAT’S HAPPENING?
Bio H
Because of the dipole (partial charges) created by the polar covalent bond H2O molecules are weakly attracted to one another
This attraction is called a H-bond
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PROPERTIES OF WATER
Polarity of Water movie
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PROPERTIES OF WATER
Cohesion•Water molecules stick to other water molecules
•Creates a high surfacetension
•Belly flop anyone?
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Adhesion•Water molecules stick to other substances with partial charge
•Capillary action!
Properties of Water
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PROPERTIES OF WATER Universal Solvent
Polarity of water allows it to interact with neighboring polar or ionic molecules
Dissolves or suspends many substances
What will not dissolve in water?
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PROPERTIES OF WATER
Universal Solvent – making salt water
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PROPERTIES OF WATEREXAMPLE NaCl + H2O Na+ + Cl- + H2O
oxygen attracts sodium hydrogen attracts chloride sodium & chloride separate as ionic
bonds are broken Is this a solution, suspension or
colloid?
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Water has a high specific heat•Specific heat is the amount of energy needed to raise 1 gram of water 1 degree.
•Water absorbs a lot of energy before its temp goes up
•Keeps earth’s temperature stable!
Properties of Water
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CONCEPT OF PH – SEE PH SCALE AND WORKSHEET