Exam 3 Vocab Flashcards
atomic number
mass number
atomic mass
atomic number- # p
mass number- #n + #p
atomic mass- average mass
properties of metals
- conductive
- malleable
- usually solid
properties of non-metals
- nonconductive
- solid, liquid, gas
properties of metalloids
- semi-conductive
- generally solid
What is the Bohr model?
- electrons orbit around the nucleus and only fixed quantized distances
- elections can only live in orbitals levels
- gaps get smaller as n gets bigger
- electrons as low as they can be is ground state
Relate emission and absorption of photons with energy levels
gains potential energy (absorption/atom excited)
Loses PE (emission/ atom relax)
Relate size with the periodic table
- go down PT, elements get bigger
- go left PT, nucleus has great pull, making element smaller
Chemical change vs physical
Chemical: alter the nature of the particles, rearrange atoms
Physical: alter physical substance
Define:
Pure element:
Pure compound:
Homogenous mixture:
Heterogenous mixture:
Pure element: single element
Pure compound: single chemical formula
Homogenous mixture:
- solution: White gold salt water,
- suspension: milk, blood
Heterogenous mixture: not fully mixed
What is hydroxide and sulfate formulas?
OH-
SO4 2-
What are ionic bonds?
Full stealing of electron between metal and non-metal
What are covalent bonds?
sharing of electrons
How do you name compounds?
Ionic:
1. metal first
2. replace anion with -ide
Covalent:
1. least EN first
2. more EN gets -ide
3. greek prefix (1-mono; 2-di; 3- tri; 4- trenta; 5-penta; 6-hexa)
What are 4 types of IM forces?
Strongest to weakest
- Ion-Dipole: polar molecule with ionic compound
- Hydrogen bonding: X-H … X
(X = O,N,F)
- Dipole-dipole: 2 polar molecule
- London Dispersion: any attraction between 2 molecules (bigger with size)
What are metallic bonds?
Metals share electrons, but the sharing extends over the whole metal
- Why they a malleable and conduct electricity
How does intermolecular forces affect boiling point?
Stronger the force, higher boiling point
Solute vs. solvent (components of a solution)
solvent: what we have more of in solution
solute: minor component
soluble vs. insoluble
How it relates to I.M.Fs and phases
soluble: solute dissolves easily
Insoluble: only dissolves small amount
IMF: determined by competition between IMFs
Phases:
- solubility with solids increases with high temp
- solubility with gases increases with low temp
Definition of saturation
Max solubility of a solution has been reached
How do soaps function?
Has a polar ionic head that is hydrophilic and a non-polar tail which is hydrophobic (hydrocarbon chain that dissolves oil)
What is a mole?
1 mole of an element has same mass in grams as 1 atom in amu
6.022 x 10^23
How can the rate of a reaction be altered?
Temp, pressure, more substance (concentration), catalyst
What is activation energy?
minimum energy required to have a reaction
What is equilibrium? Product-favored vs. reactant-favored?
Relationship to Gibbs free energy?
Chemical equilibrium: when rates are balanced
Product-favored: More products (neg free energy)
Reactant-favored: more products (pos. free energy)
What is Gibbs Free Energy?
Total change in energy in a reaction
Exergonic vs. Endergonic
High in what?
Exergonic: releases energy; high products
Endergonic: gains energy; high reactants
Acid-base reactions are…
acid- donates an H+
base- accepts an H+
What are strong vs weak acids and bases?
reactant or product favored?
Strong acids and bases will react 100% (product-favored equilibrium)
Weak: not 100%, may be either product or reactant-favored
PH scale
1-6 Acidic
7 Neutral
8-14 Basic
Compare acid-base reactions and hydronium and hydroxide
basic: OH- > H3O+
acidic: OH- < H3O+
NH3 and OH- are what?
strong bases
CH3CO2H is what?
acetic acid (vinegar) - strong
