Exam Review Flashcards
Electron affinity:
The energy released when an e is added
Ionization energy:
The energy it takes to remove an e
Atomic radius:
Distance from nucleus to outer shell
What Does electron affinity do across a period
Increases bc there r more p+ so it is harder to remove e- (less nuclear attraction)
What does electron affinity do down a family?
Decreases bc shells are further away so e- are easier to remove (less nuclear attraction)
What does ionization energy do across a period?
Increases bc there r more p+ so it is harder to remove e- (less nuclear attraction)
What does Ionization energy do down a period:
Decreases bc shells are further away so e- are easier to remove (less nuclear attraction)
What does atomic radius do across a period:
Decreases across a period bc more p+ as u go across (more nuclear attraction) shells stay same
What does atomic radius do down a family:
Increases bc # of shells increases as u go down the periodic table
Ionic characteristics:
Metalx2, non-metal + metal, total transfer of e-, ⬆️melting/boiling point, solids at room temp, hard/brittle(inorganic compounds), strong bonds, conductive, soluble, electron orbitals r separate
Covalent characteristics:
Non metals, shared e, ⬇️melting/boiling point, liquids+gases at room temp, relatively soft (organic compounds), weak bonds, don’t usually conduct, insoluble, e orbitals overlap
What happens when charge differences occur in ionic compounds:
Electrostatic attraction occurs between ions
What is formed when ions bond together (ionic bonding)
A crystal lattice structure is created with opposite charges
Polar covalent:
When sharing is not exactly equal but is still shared
Electronegativity:
The measure of tendency of an atom to attract a bonding pair of electrons
Electronegativity scale:
0.0 0.5. 1.7. 4
_____________________________
non polar. Polar. Ionic
What happens to electronegativity across a period:
Electronegativity ⬆️ (due to p+ increasing)
What happens to electronegativity down a family:
Electronegativity ⬆️ (due to more energy levels that our outer e-‘s farther from pull of nucleus)
Scaling factor:
scaling factor = MMmolecular
———————-
MMempirical =value
(Multiply value by each number of atoms)
%yield =
%yield= actual
———— x100
Theoretical
%c=
%c= m solute(g) / v solute(ml) x100
how to find ppm, ppb, ppt
Pp(m) = grams x 10^6
———————
Volume (ml)
Ppb= 10^9 Ppt=10^12
M/m and v/v
M/m = mass solute / mass solution V/v = v solute / v solution
Percent composition:
%element= MM element
——————— x100
MM compound
Lab data percent composition:
%element = m element
——————— x100
m compound
Acids produce what when reacted with active metals
Hydrogen gas
Acids produce what when reacted with carbonate compounds
C02
Strong acids occur when
of oxygen exceeds # of hydrogen by 2 or more
Strong bases occurs when
Only made from group 1 or 2 metals (alkali and alkaline earth metals)
Strong acids and bases
Dissociates completely into ions in water
Titration equation:
nbMaVa = naMbVb
Nature of gases characteristics:
- Gases have mass
- Are compressible
- Fill their container
- Exert pressure
- Gases diffuse
- Pressure is dependent on temp
Ideal gas law:
Hypothetical gas:
- molecules occupy negligible space
- have no interactions
- obeys the gas law exactly
High altitude =
Low pressure
Low altitude =
High pressure
Units of STP
1 atm = 14.7 psi = 760 mmHg = 760 torr = 101.3 kPa
Boyle’s law:
The volume of a given mass of gas is inversely proportional to its external pressure
Boyle’s law equation:
P1V1 = P2V2
Charles law:
Temp and volume are directly proportional
Charles law equation:
V1T2 = V2T1
Gay Lussac’s law:
Temp and pressure of a gas are directly related
Gay Lussac’s law equation:
P1T2 = P2T1
Combined gas law:
P1V1T2 = P2V2T1
Temperature:
Measure of avg. KE molecules have (KE ⬆️, temp ⬆️)
Avagadros law:
At same temp & pressure the volume of an ideal has occupies a volume of 22.4 L at STP.
Avagadros law equation:
n1 n2
— = —-
V1. V2
Ideal gas law equation:
PV=nRT
Ideal gas law stp’s:
- 314 kPa
0. 0821 Pa
