Ap chem do not forget

List the 4 imfs

ldfs dipole to dipole hydrogen bonding and ion dipole bonding

More polarizable” refers to which IMF?

ldfs

1. 6Name 2 properties that decrease as IMF’s increase.

vapor pressure volatility

1. 7Which type of solid has the lowest melting/boiling points?

molecular soids

1. 8Which type of solid will not conduct electricity until it is a liquid or aqueous?

ionic soilds

1. 9a) Give 2 examples of a covalent network solid.

diamond and quartz

9b) Which type of solid has the highest melting/boiling points?

covalent network

1. 10What type of solid always conducts electricity?

metalic

1. 11When a molecular solid melts or boils, which bonds break?

iintermolecular forces

1. 12 What type of alloy is made when the radii of the atoms are different/similar in size?

different size interstial similar size substitional

1. 13a) What type of change separates a compound into elements?

chemical

13b)  What type of change separates a mixture into its components?

physical

1. 14 Filtering separates mixtures based on differences in what property?

particle size

1. 15 Distillation separates mixtures based on differences in what property?

boiling point

1. 16 Chromatography separates mixtures based on differences what property?

polarity

1. 17a) In paper chromatography, if water is used as the “mobile phase”, what kind of substance will move moves up the farthest:  something polar or something nonpolar?

polar

17b) In paper chromatography, if a nonpolar substance is used as the “mobile phase”, which component of a mixture will move moves up the farthest:  something polar or something nonpolar?

nonpolar

1. 18 What type of change conserves mass: chemical, physical, both or neither?

both

1. 19 Why are all gas mixtures homogeneous?

They are in a constant rapid moving motion

1. 20 Why are gasses compressible?

they are seperated by vast areas of empty space

1. 21 What causes gas pressure?

the collision with the walls

1. 22 P and V are inversely or directly related?

inversley related

1. 23 T and V are inversely or directly related?

directly

1. 24 T and P are inversely or directly related?

directly

1. 25 In the formula PV=nRT , what are the units for P, V, n, and T  

atm L moles kelvin

1. 26 One mole of an ideal gas = _______ Liters at STP.

22.4

1. 27 Gas pressure and # of moles are inversely or directly related? corrections

directtly

1. 28a) dRT/P equals what quantity?       

molar mass

28b) The “d” in dRT/P has what metric units?  

grams per liter

1. 29 The more molar mass a gas has, the faster or slower it moves?

the more molar mass the slower it moves

1. 30 Average Kinetic Energy is another term for _____________.

temp

1. 31 What 2 pressures add together when calculating the total pressure of a gas collected by water displacement?

vapor presure of water and presure of dry gas

1. 32a) Real gases behave most like an ideal gas at what conditions of temperature and pressure? 

high temp low pressure

32b) What gases deviate from ideal behavior the most/the least: small polar, large polar, small nonpolar, large nonpolar?

large polar devites the most while small nonpolar deviates the least

1. .What type of bond forms between hydrogen and chlorine: polar covalent, nonpolar covalent., ionic, metallic or h-bond?

polar covalent

1. a) Ionic bonds are formed between what types of elements?

metal and non metal

b) .When forming an ionic bond, which element gains/loses electrons?

metal loses non metal gains

1. .As the electronegativity difference between 2 atoms increases, what happens to the polarity of the bond? 

polarity increaces

1. .Name the 7 diatomic elements.  

N,H,F,O,I,C,Br

1. What is the formula for calculating % yield?What is the formula for calculating % error?

Actual yield/theoretical yield x 100 experimental - actual/actual x 100

1. What is a limiting reactant?

a reactant that is completely consumed first in a chemical reaction

1. What is the total # of covalent bonds carbon has to make when drawing a Lewis (e- dot) structure?

4

1. a) .Are asymmetrical/symmetrical molecules polar or nonpolar?

asymetrical is polar

1. .How many sigma and pi bonds are there in a triple bond?

1 sigman 2 pi

1. a) .What term do we use for the energy to break the ionic bond in a compound? 

lactice energy

b) What 2 properties affect the lattice energy?

ionic charges and ionic radii

c) Which ionic compound would have the most lattice energy? large/small ion charges; large/small ion radii

larger charges smaller radii

1. .When drawing a Lewis (electron dot) Structure, after connecting the atoms with single bonds, if you notice that you have too few remaining electrons to give every atom an octet, that’s an indication that you are going to have to do what?

form double or triple bonds

1. a) Which piece of glassware is the most precise: beaker, burette, or graduated cylinder? 

b). Which piece of glassware is the least precise: graduated cylinder, beaker, or burette?

d) Which piece of glassware only has one line on it so it can only be used to measure one specific volume?

1. What is the equation for calculating the density of a substance?

1. The % composition by mass of which substance does not change: heterogeneous mixture, homogeneous,  mixture or compound?

1. a). When an electron is in a higher/lower energy level, is it closer or farther away from the nucleus? a). When an electron is in a higher/lower energy level, is it closer or farther away from the nucleus? 

b) When an electron is in a higher/lower energy level does it have more or less Coulombic attraction to the nucleus? 

c) When an electron is in a higher/lower energy level, is it easier to remove or harder to remove?

d) When an electron is in a higher/lower energy level, does it have a higher or lower 1st ionization energy?

1. a) Moving across a row (L to R) on the periodic table, does Z_eff increase, decrease, or stay the same?

Moving across a row (L to R) on the periodic table, are the valence electrons more or less attracted to the nucleus

c)  Moving across a row (L to R) on the periodic table, does the atomic radius increase or decrease?

d) Moving across a row (L to R) on the periodic table, does the ionization energy increases or decrease?

e) Why do atoms get smaller moving across a row (L to R) on the periodic table?

1. a). When reading a PES graph, what does the height of a peak represent?