Basic chemistry
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Transcript of Basic chemistry
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Basic chemistry
•Atoms to Organisms
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Section 1 Vocabulary:9 words
1. atom ( Proton, neutron, electron),
2. element,
3. isotope,
4. compound,
5. covalent bond,
6. molecule,
7. ion,
8. ionic bond,
9. Vander Waals forces.
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WHAT IS MATTER?
Anything that has
mass and volume!
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ATOMS AND ELEMENTS
1. ATOMS: make up elements, they are the smallest part of an element that still has all of the properties of the element.
2. ELEMENT: a substance that can not be broken into simpler substances.
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Model of an Atom
• Moving charged particles
• Protons +• Neutrons 0• Electrons –
• Most of the volume is empty space!
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ELECTRONS ARE IMPORTANT!
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• Electron spend their time in areas around the nucleus.
• Each area or orbital hold a certain number of electrons.
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• The first orbital for electrons holds 2
• The next level holds 8
• The electrons are in pairs!!!
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• They fill the open spaces one at a time
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BONDING• This leaves one electron with out a partner
• This electron will be more stable with another
electron in the orbital with it. The atom is likely to
bond with an atom that has one extra electron.
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ATOMIC NUMBERis
the number of protons in an atom
# protons
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• ELECTRONS ARE LIGHT!
• PROTONS ARE HEAVY
• NEUTRONS ARE HEAVY
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SO………
The mass of an atom is made up of the protons
and neutrons!
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ATOMIC MASS• The number of protons plus the number of
neutrons in an atom. • How many neutrons?• Subtract the atomic number from the mass
number!
19 atomic number
Example: K symbol Potassium name 39.098 Atomic mass
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19 atomic number= # P = # E
K symbol Potassium name
39.098 Atomic mass= P + N
Protons = 19 Electrons =19 Neutrons =20
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# NEUTRONS
39
- 19
20 NEUTRONS
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How many electrons?
• The number of electrons is equal to the number of protons unless the atom has a charge!
• 10 p+ = 10 e - neutral
• 10 p + 9 e - positive 1 charge +1
• 10 p + 11 e - negative 1 charge -1
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3. isotopes
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WHAT IS DIFFERENT ABOUT ISOTOPES?
THE NUMBER
OFNEUTRONS
OR ATOMIC MASS
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4. COMPOUNDS
• A SUBSTANCE THAT CONTAINS 2 OR MORE ELEMENTS CHEMICALLY COMBINED.
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5. Covalent Bonds
• Sharing of electrons to make both atoms have a complete set of orbitals
ME too!
I could use one more electron
I just need 2
more and I will be perfect!
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6. molecule,
• When 2 or more atoms are combined with chemical bonds a molecule is formed.
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7. ion,
• An atom that gains or loses an electron and therefore has a charge.
+ -
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8. Ionic Bonds• ELECTRIC ATTRACTION!!!!!
+
-• NEGATIVE TO POSITIVE!
• IONS HAVE A CHARGE-
• AN EXTRA ELECTRON (-)
• MISSING ELECTRON (+)
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Ionic- donation!!!
One spare.-1 charge
Needs one
+ 1 charge
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Sodium chloride
• An example of an ionically bonded molecule
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Let’s share!!!!!!!!
Now we all are happy!!!
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• 9. Vander Waals forces. When molecules come close together and positive and negative regions are attracted the forces of those attractions are called van der Waals forces.
• Notes: the strength depends on the size and shape of the molecules. They are not as strong as covalent and ionic bonds.
• They are important to biological processes!
• Water is an example of a substance with van der Waals forces!
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Water
Hydrogen bond
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Surface Tension
• Water to Water bonds
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cohesion• Water to water
• Adhesion: water to something else
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meniscus
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Capillary Action
• Water “pulls” itself up a tube by its adhesion to the sides of the tube
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pH• A measure of hydrogen ion concentration
• Scale 1- 14
• 1-6 acid
• 7 neutral
• 8-14 base
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pH paper
• Measure by a color change
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pH activity
• Make a data chart of the items to be tested
• Test the pH and record the number
item pH