Exam 1 Flashcards
atomic number
number of p+
atomic charge calculation
(# of p+) - (# of e-)
mass number =
number of protons + # of neutrons
ionic charge calc
(# of p+) - (# of e-) = +n or -n
matter
anything that has mass and occupies space
protons
positively charged particle with a sizeable mass
neutrons
electrically neutral particle with a mass approximately = to a proton
electrons
negatively-charged particle with a very small mass
solids
molecules densely packed
definite shape
not easily compressible
liquids
molecules are loosely packed
no definite shape (can flow)
not easily compressible
gas
molecules NOT packed
no definite shape
easily compressible
identify elements, compounds, and mixtures
- is the material on the periodic table? > yes? > it is an element
- are the names of of two elements present in the scientific name of the material? > yes? > it is a compound
- is only one substance, layer, or color seen when i look at the material? yes? > the material is a solution
- are two or more substances, layers, or colors seen when i look at the material? yes? > the material is a heterogenous mixture
homogenous mixture
a combination of two or more elements or compounds which appear to be one layer or material
ex) when salt is added to water, the compound hydrogen oxide, the two materials mix with the salt dissolving to make a solution
heterogenous mixture
a combination of two or more elements or compounds which appear without any manipulation to be more than one layer or material
ex) when sand is added to water, the sand settles in one layer on the bottom with the water forming another layer on top
physical change processes
changes state, NOT composition
-odor
-taste
-color
-appearance
-melting point
-boiling point
chemical change process
change in composition
-corrosiveness
-flammability
-acidity
-toxicity
melting:
solid to liquid
freezing
liquid to solid
vaporization
liquid to gas
deposition
gas to solid
condensation
gas to liquid
sublimation
solid to gas
AMU (atomic mass unit)
avg mass of an element based upon the mass of the isotopes
molar mass (g/mol)
mass of a given element divided by the amount of substance
core electrons
innermost e- tightly bound to nucleus that occupy the LOWEST energy level
total e- minus valence e- = core
valence electrons
outermost e- that occupy the HIGHEST energy levels
involved in chemical bonding
= group #
= group # above 12 subtract 10
aufbau principle
e- are placed into orbitals of the lowest available energy
S orbitals are first 2 groups
D orbitals are transition metals
P orbitals are groups 13-18
F orbitals are bottom two periods
pauli exclusion principle
no two e- can be the same and must be spin-paired
s-orbitals hold:
1 orbital; 2 e-
p orbitals hold:
3 orbitals; 6 e-
d orbitals hold:
5 orbitals; 10 e-
f orbitals hold:
7 orbitals; 14 e-
noble gas configuration
normal: 1s22s22p63s23p64s23d104p65s24d105p66s2
noble gas: [Xe]6s2
take the previous noble gas to account for the core e- in the overall electron config
LEO goes GER
loss of e- = oxidation
gain of e- = reduction
anion- = gain e-
cation+ = lose e-
ex) F = 9e-; F- = 10e-
predictable ionic charges
group 1 = 1+
group 2 = 2+
group 3 = 3+ (aluminum)
group 5 = 3-
group 6 = 2-
group 7 = 1-
transition metals:
Chromium = 3+/6+
Manganese = 2+
Iron = 2+/3+
Cobalt = 2+
Nickel = 2+
Platinum = 2+
Copper = +/2+
Silver = +
Gold = +/3+
Zinc = 2+
Cd = 2+
Hg2 = 2+ or Hg2+
periodic trends
atomic size increases: ↙
ionization energy increases: ↗
EN increases: ↗
ionic size: cations < anions
how to identify an element and its isotope
mass #atomic #SYMBOLcharge
empirical formula
simplest whole number ratio of the atoms
ex) CH
molecular formula
exact # of each type of atom found in a compound
ex) C6H6
structural formula
exact # of each type of atom found in a compound; exact manner in which those atoms are bound together
diatomic molecular element
2 atoms; ex) H2
molecular compounds
2 or more nonmentals
nm+nm
ex) H2O
ionic compounds
metal + nm
ex) NaCl
