Review of Basic Chemistry Chapter 2. What is Biochemistry? Biochemistry – the study of the...
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Review of Basic Chemistry Chapter 2. What is Biochemistry? Biochemistry – the study of the chemical substances and vital process occurring in living organisms
What is Biochemistry? Biochemistry the study of the chemical
substances and vital process occurring in living organisms.
Biochemistry allows us to understand how the body works. Ex. Your
body breaks down food and makes ATP for energy through
chemistry.
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Essential Elements Most organisms are made of: 1. Hydrogen (H)
2. Oxygen (O) 3. Nitrogen (N) 4. Carbon (C)
Slide 4
Vocabulary Element - substance composed of one type of atom
only. Ex. Na Atom smallest part of an element that possesses all
the properties of the element. Proton particle in the nucleus with
a positive charge of +1. Neutron a non-charged particle found in
the nucleus.
Slide 5
Vocabulary Electron negatively charged particle -1. Weighs only
a fraction of the proton and neutron. Isotope - atoms with the same
number of protons and electrons, but different numbers of
neutrons.
Slide 6
Organic and Inorganic Chemistry Organic contains carbon.
Exceptions CO 2 and CO Inorganic do not contain carbon
Slide 7
Defining Characteristics of Matter Matter is anything that
occupies space, has mass and possesses the property of inertia.
Inertia a body remains in the same state of motion until an outside
force acts upon it.
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Forms of Matter Solid, liquid, gas The form of a substance is
determined by the potential energy of the molecules. The more
energy, the quicker the molecules move. There is more energy in a
liquid than in a solid.
Slide 10
Electrons Electrons are found outside of the nucleus in
orbitals. Chemical reactions involve sharing or exchanging
electrons. Valence Electrons electrons found in the outermost
energy level
Slide 11
Carbon The first orbital can hold 2 electrons. The next can
hold up to 8. Because carbons atomic number is 6, it has 6 protons
and 6 electrons.
Slide 12
Stability Elements are stable when the outer electron level is
full or has 8 electrons.
Slide 13
Energy When bonds form, energy is stored in that bond. When
bonds break, energy is released. 2 hydrogen atoms bonded together
need 104 kcal/mole to break.
Molecules and Compounds Molecule two or more atoms of the same
type chemically combined. Ex. O 2 Compound two or more different
atoms chemically combined. Ex. HCl
Slide 16
Covalent and Ionic Covalent bonds share electrons. Ex. O 2
Ionic bonds formed by transferring electrons. Ex. NaCl (sodium
chloride)
Slide 17
Electronegativity Oxygen has a stronger pull on electrons
because it is more electronegative. Oxygen has an electronegativity
of 3.5. Hydrogens affinity is only 2.1
Slide 18
Salt Salt is sodium chloride or NaCl. Sodium chloride is formed
when sodium donates an electron to chlorine. This is an ionic
bond.
Slide 19
Importance of Water Covalent bonds hold a water molecule
together through 2 pairs of shared electrons. Bohr model of
water
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Importance of Water Polar means that the electrons are not
evenly shared between the atoms. Oxygen is partially negative
because it has a greater pull on the electrons than hydrogen.
Oxygen is slightly negative, hydrogen is slightly positive.
Slide 23
Slide 24
Importance of Water Since the oxygen atoms are slightly
negative and the hydrogen atoms are slightly positive, there is an
electrostatic attraction between the positive and negative ends of
two molecules. This results in a hydrogen bond holding two water
molecules together.
Slide 25
Importance of Water Water has the ability to dissolve other
molecules due to the fact that water is a polar molecule. It
surrounds negative atoms with the positive hydrogen ends and
positive atoms with the oxygen ends. This is why it is called the
universal solvent.
Slide 26
Importance of Water Properties of water: 1. Ice floats (water
expands as it freezes) 2. High heat of vaporization (a lot of
energy to go from liquid to gas) 3. High specific heat (a lot of
energy is required to raise the temp.) 4. Universal solvent 5.
Hydrophobic effect (water pushes non-polar molecules together)
Water will not interact with non-polar molecules
Slide 27
Acids and Bases Acid molecules that split apart in water and
release hydrogen ions (H+) Base molecules that split apart in water
and release hydroxide ions (OH-)
Slide 28
Acids and Bases Buffer substance that helps keep body solutions
at the proper pH level releasing H+ or OH-. Bicarbonate and
Carbonic acid are the most common buffers in the human body.
Buffers maintain homeostasis.