Chem Flashcards
Scientific notation: Base Value and logarithm
Significand and exponential
An atomically charged atom
ion- cation+, anion-
Periodic table: periods
horizontal rows
Periodic table: groups
Vertical columns group # = valence electron #
Atomic number
Number of protons, defines atom
Atomic mass
Protons + Neutrons; Average mass of the atoms isotopes
Isotopes determined by
Different number of neutrons
Combination of elements
Compounds; form in whole number ratios ex NaCl 1:1
Chemical equation
Reactants -> products
Equilibrium
State where reactants form products at the same rates that products are forming reactants
Ways to increase reaction rate
Raising temp, increase surface area, increase concentration, catalysts (lower activation energy-enzymes)
Solution parts
Solute- part being dissolved; Solvent- part doing the dissolving
Alloys
Solid solutions of metals to make a new one
Amalgens
A specific type of alloy in which another metal is dissolved in mercury
Emulsion
Mixtures of matter that readily separate such as water and oil
Percent concentration
Expression of concentration as parts per 100 parts; ex: mg/100 mL
Molar concentration
A mole is 6.02 x10^23 molecules of something
Avogadro’s number
6.02 x 10^23
Combustion reaction and products
Self sustaining exothermic chemical reaction;
products: Carbon Dioxide CO2 and water H2O
Single replacement reaction
Involve ionic compounds; consist of a more active metal reacting with an ionic compound containing a less active metal to produce a new compound;
Ex: Cu+2AgBr -> CuBr + 2Ag
Double replacement
Involve two ionic compounds; positive ion from one compound combines with the negative ion of the other compound;
Ex: AgBr + KCu -> AgK + BrCu
Chemical bonding determined by
interplay of the electrons in the outer shell of the atom
Ionic bonding
an electrostatic attraction between two oppositely charged ions or a cation and an anion; Metal + Nonmetal
Covalent Bonding
Formed when two atoms share electrons; strongest chemical bond; nonmetal + nonmetal
Electrons in the bond are shared equally=
Nonpolar
Polar
When the shared electron density of the bond is more concentrated around one atom more than the other
Polarity based on
the difference in electronegativity values of the elements involved
Intermolecular forces
attraction between whole molecules
Hydrogen bonds
attraction for a hydrogen atom by highly electronegative element (F,O,N); strongest intermolecular force
Dipole-Dipole
Dipole created when an electron pair is shared unequally in a covalent bond between two atoms/elements; the molecule will have a positive and negative side which attract
Dispersion Forces (London Forces)
Weakest intermolecular force; electrons within an element concentrate on one side which causes a temporary dipole which attract to another temporary dipole of opposite charge
Oxidation
loss of electron
Reduction
gain of electrons
Reducing agent
element that is oxidized
Oxidizing agent
element that is reduced
Net Charge of a molecule
sum of oxidation numbers
Acids
corrosive to metals, turn litmus paper red ph below 7; hydrogen or proton donors
Bases
Alkaline, denature proteins, slippery, turn litmus paper blue, ph above 7; hydrogen or proton acceptors; have OH group
Radiation
the particles/energy that are emitted from an unstable nucleus
Alpha radiation
emits 2 protons , 2 neutrons, +2 charge, largest emission
Beta radiation
Decomposition of a neutron into positron or Electron- 1 more proton 1 less neutron; Positron-1 less proton, 1 more neutron
Half life
amount of time it takes for half of the unstable isotope to decay; it will decay until it finds a stable nuclear cofiguration
Sugars starches carbs provide
energy for the body, carbs most abundant
Deoxyribose and ribose are used in
the formation of DNA and RNA
Oligo/polysaccharides
3-6 sugars
More than 6 sugars
starch; cellulose and glycogen
Glycolysis
Metabolization of glucose
aerobic: 2 pyruvate, 2 atp
pyruvate further metabolized by krebs cycle (oxidative phosphorylation)
anaerobic (exercise): glucose->lactate
Gluconeogenesis
production of glucose from non-carbohydrate substances-> energy cycle or stored as glycogen
What gives an amino acid its identity
the R group
union if 2 amino acids by a
peptide bond- called a dipeptide
less than 30 amino acids called
polypeptide, larger are proteins
Amino acids in humans
20
Fatty acids consist of
a hydrocarbon chain with an acid group, carboxyl group COOH
Triglyceride
3 fatty acids joined to a glycerol
Phospholipids
2 fatty acids, phosphate group, glycerol; essential components of cell membrane
Fats are used to
protect organs, maintain body temp, keep skin/hair healthy, promote healthy cell function, energy stores
Nucleic acids found in
cytoplasm, mitochondria, nucleus
Backbone of DNA molecule composed of
deoxyribose, pentose, phosphate
2 sugar phosphate chains in DNA
run opposite of each other (Antiparallel)
