chem flashcards-all

Question 1

r3.2 cl+br reaction and colour

Answer 1

Cl2(aq)+2Br-(aq) –> 2Cl-(aq) +Br2(aq) and yellow/orange

Question 2

r3.2 cl+i reaction and colour

Answer 2

Cl2+2I- –> 2Cl- +I2 and dark red/brown

Question 3

r3.2 I+br reaction and colour

Answer 3

Br2+I- –> 2Br- + I2

Question 4

r3.2 anything with cl- in it

Answer 4

no rxn

Question 5

r3.2 anything with I2 in it

Answer 5

no rxn

Question 6

r3.2 common oxidation state of oxy

Answer 6

2-

Question 7

r3.2 common oxidation state of hydrogen

Answer 7

1+

Question 8

r3.2 common oxidation state of most halogens

Answer 8

1-

Question 9

r3.2 common oxidation state of alkali metals

Answer 9

1+

Question 10

r3.2 common oxidation state of of alkali earth metals

Answer 10

2+

Question 11

r3.2 common oxidation state of nitrogen

Answer 11

variable

Question 12

s1.1 NAGSAG PMS Castro Bear

Answer 12

nitrates, acetates, group 1 metals, sulfates, ammonium, group 17 non metals. Pb2+, mercury 2+, silver 1+. Calcium, barium.

Question 13

s1.2 what are isotopes /2

Answer 13

atoms of the same element but different number of neutrons/mass number. their physical properties differ.

Question 14

calculating relative atomic mass

Answer 14

=(mass 1RA1)+(mass2RA2)

Question 15

s1.5 how much volume does 1 mole of gas occupy at STP

Answer 15

22.7L

Question 16

s1.5 as volume of a gas goes up what happens to moles (when pressure and temp are constant) and what is the formula

Answer 16

moles increases. v1/n1=v2/n2

Question 17

s1.5 when pressure increases what happens to volume (moles and temp constant) +formula

Answer 17

volume decreases. p1v1=p2v2

Question 18

when volume/pressure up what temperature (moles and pressure constant) +formula

Answer 18

temperature increases. v1/t1=v2/t2

Question 19

s1.5 ideal gas law but with the formula for moles

Answer 19

PV=(mRT)/M

Question 19

s1.5 ideal gas law but with the formula for volume (mass over density)

Answer 19

(Pm)/D=nRT

Question 20

s1.1 what is atomic number

Answer 20

of protons

Question 21

s1.1 what is mass number

Answer 21

of protons+neutrons

Question 22

official definition of an ionic bond

Answer 22

the electrostatic attraction experienced between the electric charges of a cation and anion

Question 23

s2.1 relationship between charge, radii and enthalpy of ionic lattice structures

Answer 23

increased charge=increased enthalpy. increased radii=decreased enthalpy

Question 24

s2.3 relationship between #of delocalized electrons, size of cation, charge of cation and bond strength

Answer 24

more e-=higher strength. smaller radius of cation=higher strength. higher charge=higher strength.

Question 25

s2.2 2 types of covalent bonds and whats happening to e- in each /5

Answer 25

pure (nonpolar) and polar. e- shared equally and e- shared unequally (dipole moment)

Question 26

s2.2 definition of covalent bonding

Answer 26

electrostatic attraction between a shared pair of e- and a positively charged nuclei

Question 27

s2.2 length vs electrostatic attraction (strength) of the bonds

Answer 27

the shorter the bond, the stronger the electrostatic attraction (needing more energy to split apart

Question 28

formal charge

Answer 28

=(number of valence electrons in element while in periodic table) - (non-bonded electrons+ bonded electrons divided by 2)

Question 29

draw out a trigonal pyramidal

Answer 29

AX3E <109.5, polar,

Question 30

name all the kinds of electron domain geometry and draw out

Answer 30

linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral

Question 31

bond angles of all the electron domain geometries

Answer 31

linear 180, trigonal planar 120, tetrahedral 109.5, trigonal bipyramidal 90 and 120, octahedral 90

Question 32

s2.2 5 other common types of molecular shape names and draw them

Answer 32

bent, seesaw, t-shaped, square pyramidal, square planar

Question 33

s2.2 name the axe, molecular shape name, bond angle, polarity, and draw for all tetrahedral electron domains

Answer 33

AX4 +109.5 +NP/P tetrahedral, AX3E + <109.5 +P trigonal pyramidal, AX2E2 +104.5 + P bent