Final Exam Review from list Flashcards
L1: what elements are most common in living organisms
HONC
L1: what is an electron, neutron and proton? how do they affect an element
electron- +1 charge, in nucleus, ID element mass
Neutron- no charge, in nucleus, give isotope mass
electron= -1 charge, in cloud, charge bonding
L1: what is mass number and atomic number
mass number is weight, proton and neutrons
atomic number is how it’s IDed how many protons
L1: characteristics of alpha, beta, gamma radiation
alpha: helium nucleus change atomic mass by 4 and atomic # by 2, penetrate top skin layer
beta: nuclear electron, atomic number +1 , sub-cutaneous
gamma: photon- energy wave, no effect on numbers, penetrate deep
L1: Isotopes vs elements
isotopes are different forms of the same element different number of neutrons. Only mass changes
L1: Radioactive Particles include
alpha, beta gamma
L2: Bohr Model - Absorption, Excitation, Relaxation, Fluorescence
absorption-
excitation -
relaxation -
fluorescence -
L2: Quantum Model – Orbitals and how they are organized
orbital: location and wave-like behavior of electrons
shell, subshell, orbital
L2: shell, subshell and orbital
shell: pathway followed by electrons around an atom’s nucleus ex. the 1st, 2nd, 3rd, 4th,etc shell(everything inside)
subshell: pathway in which an electron moves within a shell ex. s,p,d,f
orbital: describe wave-like behavior of an electron. ex. 1,3,5,7
L2: Electron configurations
where electrons go:
SPDF
L2: periodicity - electronegativity and atomic radius trends
electronegativity trend: right top is highest
atomic radius trend: left bottom
L2: valence shell and octet rule
valence shell: outer most shell that contains electrons
octet rule: elements are most stable when they fill their outermost S and P subshell
L2: Lewis dot structure
how many electrons in outer most shell and draw dots either 8 or less
L3: Ions – Anion vs Cation, from which rows in the periodic table?
cation: ion with pos. charge, gave up electron. first 3 rows
anion: ion with neg. charge, took electron last 3-4 rows
L3: Covalent Bonds – Polar vs Non Polar.
How many bonds does H, O, N, C want?
polar: share bonds, one wants it more non-polar: share bonds, both want it the same amount H: wants 2 bonds o: wants 2 bonds N: wants 3 bonds C: wants 4 bonds
L3: Electronegativity (Ionic, Polar, Non-Polar, how does HONC relate to this?
How bad element wants to steal or give away their electrons. Non-polar equal sharing. Polar- unequal sharing. Ionic: take/give up electron. - O>N>C=H +
L3: Single, Double, Triple bond shapes and properties
single: tetrahedral and freely rotate
double: trigonal planar, can’t rotate
triple: linear, can’t rotate
L3: How and why do chemical reactions occur?
when chemical bonds between atoms are being broken or formed
L3: What does equilibrium mean? What is K? What is G?
equal rates forward and backwards, equal energy add reactant =forward, add product = reverse, remove reactant = reverse. remove product = forward K= rate of reaction G = 0 energy used
L4: what bonds are weak bonds
Hydrogen and VDW and Ionic
L4: Ionic when in water what happens to the charge, strength, etc.
Ionic bonds: electron is taken, in water, bond is weak, breaks and h2o surrounds it. still has partial charges
L4: Hydrogen bonds define
h-bonds: partial charges of a neg. and pos. attract
L4: Van Der Walls define and who bonds together
VDW: temporary attraction when long chains are by each other and the electron is close to outside element, the other side is partial neg. and when the electron goes to the other side, they swap positions
nonpolar weak bonds, induced
L5: Why is water so special?
float when solid, H bonding
L5: Cohesion
water w/ water - hydrogen bonds
L5: Adhesion
water w/polar substance- hydrogen bond
L5: what is specific heat
cal = 1 gram raised 1 degree C cal = g x temp change
L5: % solution
= g solute/100 mL solution
L5: What is a mole?
unit of measurement ex. a dozen = 12 eggs
L5: Molar solution
mole solute/ L solution
L6: How to calculate pH
pH = -log [H+]
L6: How to calculate pOH
pOH- = -log [pH-]
L6: pH and pOH together is equal to what number? What equation
pH + pOH- = 14
[H+] x [OH-] = 1 x 10^ -14
L6: Buffer
resists change
HA(weak acid) dissociates H+(proton) and A-(conjugate base)
L7: what is an isomer
same molecular formula, different structure
L7: difference of Structural, Geometric, Enantiomers, Diastereomers isomers
Structural: same molecular formula, different pattern of bonds, atoms connected in different order
Geometric: same molecular formula, same bond pattern, different spatial arrangement around a double bond (cis or trans)
Enantiomer: mirroring the bonds from the two
Diastereomer: mixture of same bond and mirrored bonds
L8: Alkyl structure,
H
I
R-C-R Non-polar
I
HL8: sulfhydryl structure,
R-S-H
L8: hydroxyl structure,
R- O-H
L8: carbonyl structure
.. O
.. II
R-C-R
L8: carboxyl structure,
.. H
.. II
R-C-OH
L8: phosphate structure,
...... O ... .... I R-O-P-OH Acidic, polar ionic ........ I ...... OH
L8: amino structure
… H
… I
R-N-H
L8: Polysaccharide monomer and bond name
monosaccharides and Glycosidic
L8: Protein monomer and bond name
Amino acids and peptide
L8: Nucleic Acid monomer and bond name
nucleotides and phosphodiester
L8: lipids monomer and bond name
fatty acid and glycerol, and ester
L8: condensation is when what happens
when a bond forms and water is a byproduct
L8: hydrolysis is when what happens
water used to break bonds, put back in
L9: Names3 types of Monosaccharides
Fructose
galactose
ribose/deoxyribose
L9: Names/types of Disaccharides
Maltose=glucose + glucose
sucrose=glucose + fructose
lactose=glucose + galactose
L9: define of Oligosaccharides and function
sugars of 3-40 monomers, many different simple sugars,
highly branched
cell recognition/signaling and cell defense
L9: Names/types of Polysaccharides animals/plants
starch(plants), glycogen(animals), cellulose(plants), chitin(insects)
