chem flashcards-all
r3.2 cl+br reaction and colour
Cl2(aq)+2Br-(aq) –> 2Cl-(aq) +Br2(aq) and yellow/orange
r3.2 cl+i reaction and colour
Cl2+2I- –> 2Cl- +I2 and dark red/brown
r3.2 I+br reaction and colour
Br2+I- –> 2Br- + I2
r3.2 anything with cl- in it
no rxn
r3.2 anything with I2 in it
no rxn
r3.2 common oxidation state of oxy
2-
r3.2 common oxidation state of hydrogen
1+
r3.2 common oxidation state of most halogens
1-
r3.2 common oxidation state of alkali metals
1+
r3.2 common oxidation state of of alkali earth metals
2+
r3.2 common oxidation state of nitrogen
variable
s1.1 NAGSAG PMS Castro Bear
nitrates, acetates, group 1 metals, sulfates, ammonium, group 17 non metals. Pb2+, mercury 2+, silver 1+. Calcium, barium.
s1.2 what are isotopes /2
atoms of the same element but different number of neutrons/mass number. their physical properties differ.
calculating relative atomic mass
=(mass 1RA1)+(mass2RA2)
s1.5 how much volume does 1 mole of gas occupy at STP
22.7L
s1.5 as volume of a gas goes up what happens to moles (when pressure and temp are constant) and what is the formula
moles increases. v1/n1=v2/n2
s1.5 when pressure increases what happens to volume (moles and temp constant) +formula
volume decreases. p1v1=p2v2
when volume/pressure up what temperature (moles and pressure constant) +formula
temperature increases. v1/t1=v2/t2
s1.5 ideal gas law but with the formula for moles
PV=(mRT)/M
s1.5 ideal gas law but with the formula for volume (mass over density)
(Pm)/D=nRT
s1.1 what is atomic number
of protons
s1.1 what is mass number
of protons+neutrons
official definition of an ionic bond
the electrostatic attraction experienced between the electric charges of a cation and anion
s2.1 relationship between charge, radii and enthalpy of ionic lattice structures
increased charge=increased enthalpy. increased radii=decreased enthalpy
s2.3 relationship between #of delocalized electrons, size of cation, charge of cation and bond strength
more e-=higher strength. smaller radius of cation=higher strength. higher charge=higher strength.
s2.2 2 types of covalent bonds and whats happening to e- in each /5
pure (nonpolar) and polar. e- shared equally and e- shared unequally (dipole moment)
s2.2 definition of covalent bonding
electrostatic attraction between a shared pair of e- and a positively charged nuclei
s2.2 length vs electrostatic attraction (strength) of the bonds
the shorter the bond, the stronger the electrostatic attraction (needing more energy to split apart
formal charge
=(number of valence electrons in element while in periodic table) - (non-bonded electrons+ bonded electrons divided by 2)
draw out a trigonal pyramidal
AX3E <109.5, polar,
name all the kinds of electron domain geometry and draw out
linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral
bond angles of all the electron domain geometries
linear 180, trigonal planar 120, tetrahedral 109.5, trigonal bipyramidal 90 and 120, octahedral 90
s2.2 5 other common types of molecular shape names and draw them
bent, seesaw, t-shaped, square pyramidal, square planar
s2.2 name the axe, molecular shape name, bond angle, polarity, and draw for all tetrahedral electron domains
AX4 +109.5 +NP/P tetrahedral, AX3E + <109.5 +P trigonal pyramidal, AX2E2 +104.5 + P bent
