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matter
anything that occupies space and has mass
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element
a substance that cant be broken down to other substances by ordinary chemical means
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compound
a substance consisting of two or more different elements in a fix ratio
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trace element
elements that are essential to humans
ex. iron (fe) needed by all forms of life
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4 elements found in the human body
oxygen, carbon, hydrogen, nitrogen
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goiter
an iodine deficiency in the diet that causes the thyroid gland to grow to an abnormal size.
*caused when u dont ingest enough idodine
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atom
smallest unit of measure that still retains the properties of an element
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3 subatomic particles found in an atom
proton, electron, nuetron
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electron
a subatomic particle with a single negative charge
(-)
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proton
a subatomic particle with a single positive electrical charge (+)
*found inside the nucleus, central core
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nuetrons
electrically nuetral has no charge
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atomic number
- the number of protons
- (top number)
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mass number
sum of the # of protons and neutrons in its nucleus
(big, bottom number)
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isotope
one element that has the same number of protons and behave identically in chemical reactions but have different number of neutrons
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how to get # of neutrons
atomic mass - atomic # = # of neutrons
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structure of an atom
- 1st shell - 2 e- (max)
- 2nd shell - 8 e- (max)
- 3rd and above - up to 18 e-
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ionic bonding
- electrons get transfered
- metal to a nonmetal
- forms ions
- ex. salt
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ions
an element with a charge
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covalent bonding
- electrons get shared
- nonmetal with a nonmetal
- ex. methane gas
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polar covalent
forms when 2 atoms share their e- unequally ex. h2o creates a slightly positive side and negative side
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nonpolar covalent
forms when 2 atoms share their e- equally ex. methane or hydrogen gas
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hydrogen bonds
- the attraction with a Hydrogen atom w/ a positive charge and another atom with a negative charge
- the polarity of water allows for hydrogen bonding
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properties of water
- universal solvent
- expands
- high specific heat
- cohesian
- adhesion
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universal solvent
- water is the universal solvent
- ions and polar molecules dissolve easily in water
- when solute dissolves, water molecules cluster around its ions or molecules and keep them seperated
- water transports molecules dissolved in it .
ex. blood, a water based solution, transports molecules of nutrients and wastes in organisms
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expands
water expands when it freezes
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why does ice float in water
because its frozen and the colder it gets the less dense it gets
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high specific heat
it takes alot of energy to change waters temp (due to h bonds breaking and reforming)
- important because A large body of water can absorb and store a huge amount of heat from the sun in the daytime and during summer while warming up only a few degrees. And at night and during winter, the gradually cooling water can warm the air
- The high specific heat of water also tends to stabilize ocean temperatures, creating a favorable environment for marine life.
THus because of its high specific heat, the water that covers most of Earth keeps temperature fluctuations on land and in water within limits that permit life.
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cohesian
- water sticking to itself
- attraction between molecules of substance
- produces surface tension in a measure of the force neccesary to stretch or break the surface of a liquid
- ex. wax paper
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adhesion
- water sticking to other substances
- attraction between a molecules of different substance
- ex. water on paper or glass
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mixture
- 2 or more elements/compunds physically combines
- (salt & pepper )
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types of mixtures
- solution
- solute
- solvent
- suspension
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solution
components are evenly distributed
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solute
substance that is dissolved
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solvent
substance in which the solute is dissolved
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koolaid (what kind of mixture ) sss
solution
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koolaid mix (what kind of mixture ) sss
solute
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water (what kind of mixture ) sss
solvent
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suspension
mixture of water with dissolved material
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hydrophilic substances
- water loving
- polar
- hydrogen bond with water
- ex glucose (sugar)
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hydrophobic
- water fearing
- nonpolar
- repelled by water (no hydrogen bonds can form)
- ex. oil
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the ph scale
- tells us how acidic or basic a substance is
- 0-14
- 0 to 6 = acidic
- 7= neutral
- 8 to 14 = basic
- scale measures h+ concentration of fluid
- (the more h+ the more acidic)
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acids
ex . stomach acids, urine, hydrchloric acid, coffee, soda
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bases
ex. intestinal fluid, blood, magnesium hydroxide, bleach, salt water
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buffers
weak acids or bases that can react with strong acids or bases to prevent sudden changes in PH. this is done by donating or accepting a h+ ion to or from the solution
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carbonnic acid
- bicarbonate buffer system
- when blood ph rises the carbonic acid dissasosiates to from bisarbonate and h+
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