IMF flashcards

VSEPR

valence shell electron pair repulsion

shapes

linear(most common), bent, trigonal, tetrahedral, pyramid, trigonal planar

strongest intermolecular force=

hydrogen

intermolecular forces=

van der wal forces

3 vander wal forces

london dispersion, dipole-dipole, and hydrogen bond

rank low to high 5 different inter and intramolecular forces

london dispersion, dipole-dipole, hydrogen bond, covalent bonding, ionic bonding

highest electronegativity=most polar= stronger

intermolecular forces

electronegativity increases as you go

up and across the table

nonpolar=

london dispersion

hydrogen cannot be the

central atom

carbon is usually the

central atom

the atom with the smallest__ is the central atom

elecronegativity

what type of IMF is PF3

dipole dipole

what type of imf is HF

hydrogen bond

explain how dipole dipole forces cause molecules to be attracted to one another

polar molecules have partially positive and partially negative sides (which correspond to the side of the molecule which is more or less electronegative) because opposite charges attract one another, these molecules stick electrostatically

rank the following compounds from lowest to highest boiling point: calcium carbonate, methane, methanol CH4O, dimethyl ether CH3OCH3)

lowest: methane (non-polar), dimethyl ether (dipole-dipole), methanol (dipole dipole and hydrogen), calcium carbonate (ionic bond)

explain why nonpolar moleules have much lower surface tensions than polar ones

because the molecules aren't attracted to each other as much in polar molecules, these molecules are much less likely to have a high surface tension

bigger molecule, less pull on nucleus, more shielding. Larger molecule means

stronger IMF

rank the following compounds from weakest imf to strongest: H2S, I2, N2, H2O

N2 (I2 is larger therefore stronger LD) I2 (LD), H2S (dipole-dipole), H2O (hydrogen bond)

rank the following from weakest IMF to stongest: H2Se, H2S, H2Po, H2Te

H2Po, H2Te, H2Se, H2S (all dipole dipole, most electronegative=most polar=strongest

predict the shape of H2s

bent

shape of CCL4

tetrahedral

shape of SO2

bent

Shape of Br F

linear

intra

force within molecules (ex. covalent)

inter

force between molecules (ex. van der waals forces)

boiling points low to high

london dispersion, dipole dipole, hydroen bond, ionic bond

hdrogen bonding

FON, stronger than dipole dipole so higher boiling point

London dispersion

present in all molecules, non polar, weakest imf, extremely low boiling point, strength increases with increase in molecular size

what three variables will affect the pressure of a gas

temp, # of molecules, and volume

if a gas is brought to a higher altitude, what happens to the pressure

external pressure decreases

flamin foods lab equation

mass of food times c times delta t= mass of water times c times delta t

groups =

columns

periods=

rows

which side of periodic table is most reactive

ends group 1 and 7

which side of periodic table is least reactive

middle

which trends increase across the periodic table

effective nuclear charge, ionization energy, and electronegativity

which trends decrease across the periodic table

atomic radis, ionic size

proton and neutron location

nucleus

weak to strong and low boiling point to high

london, dipole, hydrogen, covalent, ionic

answer in __ tomorrow

sig figs

what two factors contribute to the trend of ionization energy?

effective nuclear charge, atomic size

H-bonds have high boiling points and___

solubility

dipole-dipole are somewhat

soluble

more difference in electronegativity=

more polar

ionic compound properties

-formula unit (balance of oppositely charged ions)

-metallic combined with nonmetallic

-solid at room temp

-high melting point

-conducts electricity

-dissolves water

covalent bond properties

-low melting points

-solid, liquid, or gas at room temp

-poor electrical and thermal conductivity

-metal and metal sharing electrons

-does not always dissolve in water

-does not easily form electrolytes

octet rule exceptions

hydrogen and helium only need 2 electrons to form stable configurations; Li, Be, and B loose electrons to form He or the? configuration

si unit for mass

kg

y is

dependent

x is

independent

avogadro's hypothesis

given 2 samples of an ideal gas of the same volume, at the same temp and presure, contain the same # of molecules

what is the relationship between temperature change and heat

the greater the temp change, the greater the quantity of heat

what is the relationship between mass and temperature change?

more mass is less mcdelta t

conductors, low electronegativities, low ionization, ductile, give electrons, shiny, malleable, reacts with acids and oxygen, form cations

metals

high electronegativities, non-conductors, insulators, take electrons, dull, brittle, don't react with acids, form cations

nonmetals

periods

same energy levels

gropups

number of valence electrons

order of subshells

spdf

s can hold

2

p can hold

6

d can hold

10

f can hold

14

mass equals

protons plus neutrons

resonance

same bonds different arrangement

single bond

one pair of electrons (2 e)

double bond

two pairs of electrons (4e)

triple bond

three pairs of electrons (6e)

if there are extra electrons in a centrla atom it is

polar

1mL=

1cm^3

kinetic molecular theory

describes all matter as being composed of tiny particles in endless random motion. In a solid,the particles vibrate but are locked into an orderly array. In a liquid, the particles are still touching but are free to move around past one another. IN a gas the particles are moving very rapidly and are widely separated

when energy is transferred to a sample of matter, __ the partiles speed up (temp increases), or they get pulled apart (phase change, but__ both at the same time

either, not

relate energy levels to the distance from the nucleus

the further away from the nucleus, the more energy (higher principle energy level)

given 1s2 2s2 2p6 3s1 describe the meaning of 3; 6; and p

3 is the 3rd principle energy level, there are 6 electrons in the 2 p subshell, p is the sublevel shape of the orbital within the principle energy level type

within a verticle family, the enc is about the

same

the tendency to draw electrons toward it

electronegativity

energy required for an atom to lose or gain an electron

ionization energy

these have more/less number of neutrons that in other atoms of the same type

isotopes

cation is

smaller

anion is

larger

opposite charged particles

attract

similar charged particles

repel