Pattern of separation of charge in electronegativity - ️️The greater the difference
between the electronegativities of two bonded atoms, the greater the separation of
charge will be in the bond
What determines the strength and length of a covalent bond - ️️More shared
electron pairs inc...
BMB 401 MSU (FOLEY) Exam 1
Pattern of separation of charge in electronegativity - ✔️✔️The greater the difference
between the electronegativities of two bonded atoms, the greater the separation of
charge will be in the bond
What determines the strength and length of a covalent bond - ✔️✔️More shared
electron pairs increases bond energy and shortens the length between atoms
Importance of Biochemical Reactions - ✔️✔️-Help establish and maintain a stable
optimal internal environment to preserve life
-Maintain Homeostasis
Homeostasis - ✔️✔️A tendency to maintain a balanced or constant internal state
catabolic reactions - ✔️✔️break down large chemicals, oxidative & release energy
anabolic reactions (anabolism) - ✔️✔️build-up larger molecules, reductive, require
energy
How homeostasis regulates the biochemical reactions - ✔️✔️activation and inhibition
phylogenetic tree - ✔️✔️A family tree that shows the evolutionary relationships thought
to exist among groups of organisms
Bacteria - ✔️✔️-lack of membrane-bound organelles
-unicellular
-single circular DNA molecules
Archea - ✔️✔️prokaryotic, live in extreme environments, all live without oxygen and get
energy from inorganic molecules and light. most are unicellular
Bacteria vs Archea - ✔️✔️-Bacteria contains peptidoglycan Archeas doesn't
-Archea doesn't have fatty acids as tails.
Eukarya - ✔️✔️Domain of all organisms whose cells have nuclei; linear chroosomes
The four most common elements in living organisms are - ✔️✔️Oxygen, Carbon,
Hydrogen, Nitrogen
Biochemistry - ✔️✔️chemistry dealing with chemical compounds and processes in
living plants and animals
,Why is HOCN So Common in most Organisms - ✔️✔️They are small and there
electrons are relatively close to their nucleus which allows them to create stable bonds
of optimal strength.
Why small small atoms create stable bonds - ✔️✔️there is less extensive shielding
from internal orbitals and The attractive force between electrons and nucleus is
stronger.
covalent bond - ✔️✔️the inter-atomic linkage that results from the sharing of an
electron pair between two atoms
carbon + 4 hydrogen bonds - ✔️✔️methane
Resonance structures - ✔️✔️-Lewis structures that have the same arrangement of
atoms in a molecule but differ in the distribution of electrons among the atoms.
-Structures with resonance tend to have lower energy states
Electronegativity (Linus Pauling) - ✔️✔️A measure of the ability of an atom in a
chemical compound to attract electrons
Why Hetero nuclear bond energies larger are than homo-nuclear bond energies -
✔️✔️Extra energy arises through ionic character between bonds
ionic bonds - ✔️✔️when a Great electronegative difference cause one atom to gain an
electron and the other to lose an electron. (The charge difference between the atoms is
what causes attraction)
Electron sharing in covalent bonding - ✔️✔️electrons are shared equally
electron sharing in Polar covalent bonding - ✔️✔️electrons un-equally shared in a
covalent bond (partial charges on both atoms)
electron sharing in ionic (non covalent) bonding - ✔️✔️Atoms held together by
electrostatic attraction ( full charge on each atom)
Intra-molecular forces - ✔️✔️Forces that exist within a molecules
Inter-molecular Forces - ✔️✔️forces that exist between molecules. ( attractive or
repulsive)
non-covalent interactions - ✔️✔️-van der waals,
-hydrogen bonds,
, -ionic bonds,
-hydrophobic interactions
Charges in Ionic interactions - ✔️✔️Force of charges are equally distributed in all
directions (linear bonding is not required)
dielectric constant - ✔️✔️a quantity measuring the ability of a substance to store
electrical energy in an electric field
High Dielectric COnstant - ✔️✔️-Solution makes interaction with the ions.
-These interactions dissipate the effect of one charge on another through shielding
Coulomb's Law - ✔️✔️electric force between charged objects depends on the distance
between the objects and the magnitude of the charges.
Coulomb's law equation - ✔️✔️E(orF)=[kq1q2]/[r^2]
-E/-F - ✔️✔️attractive
+E/+F - ✔️✔️repulsive
Dipole-Dipole Interactions - ✔️✔️attractive forces between the positive end of one
polar molecule and the negative end of another polar molecule.
Fixed-Dipole-Dipole Interactions - ✔️✔️Occur between permanent dipoles (hydrogen
bonds)
Bond Angle of Hydrogen Bonds - ✔️✔️Linear bonding increases bonding strength
(Longer than covalent bonds)
Properties that Hydrogen Bonds give water - ✔️✔️-high boiling and freezing points
-Less dense as a solid
-The water molecules are held farther apart when freezing
dipole-induced dipole - ✔️✔️The partial charge on a polar molecule induces a
temporary partial charge on a neighboring nonpolar molecule or atom (relatively weak)
van der Waals forces (London Dispersion) - ✔️✔️Forces of attraction between
instantaneous dipoles
Where do Van der Waals forces occur? - ✔️✔️Most often found in non polar molecules
( can occur in polar molecules as well)
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