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General Chemistry
General Chemistry
66
Chemistry
Undergraduate 1
04/28/2014

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Cards

Term
what particle in the atom defines the element?
Definition
the proton
Term
what does atom mean in greek?
Definition
uncuttable - the most fundamental part, now we know it can be cut
Term
what is the relationship between the atomic # and the # of protons?
Definition
They are the same
Term
what is the mass of 1 neutron or 1 proton?
Definition
1 amu or 1.67 * 10-27 kg
Term
most of the things we look at are not solid but more empty space. Why is this so?
Definition
because most of the mass of an atom is in the nucleus. The nucleus volume is 1/10,000th of the atom volume
Term

what is a period on the periodic table?

 

what is the difference between periods?

Definition

a row

 

they have different energy levels 

 

 

Term

which electrons are highest energy and which are in the outermost energy shell?

 

4s or 3d?

 

which would be the valence electrons?

Definition

4s is the outer most of the two

 

3d electrons have the highest energy

 

the 4s are the valence electrons

 

Term
in the periodic table when you are writing electron configurations and you run into the d and f section, how do you calculate the energy level?
Definition

d = period -1

 

f = period - 2

 

there are d levels of 3,4,5, and 6

and f levels of 4 and 5

Term
why do all of the transition or d groups have 2 electrons in their outermost shell?
Definition

because they s orbitals are farther out than the d's but they are filled first

 

chromium and copper are 2 exceptions

 

Term

each period is a shell and within each shell you have different s,p,d,f orbitals or subshells.

 

How many valence electrons does Sn have?

Definition
4
Term

how many electrons do atoms want to have in their outermost shell? why?

 

not orbital but shell

Definition

8

 

experiments have proven we're not sure why

 

atoms are not very reactive when they have 8 in their outermost shell

Term
what is the first group in the periodic table called?
Definition

alkali metals, except hydrogen, they are highly reactive especially with halogens

 

they are not often found in elemental form because they are so reactive, same with halogens

Term
What do scientists mean when they talk about how metallic something is?
Definition
how much they want to give away electrons
Term
what are group or column 8 elements in the periodic table called?
Definition
noble gases, they have 8 in their outermost shell. they are happy
Term
what are group or column 2 called?
Definition
alkaline earth metals,
Term

What is the best conductor?

 

What makes a good conductor?

Definition

Silver Ag is the best

 

having available electrons makes a good conductor

 

flow of electrons is electricity

 

 

Term
around group 3-4 why do elements get more metallic or want to give up their electrons as you move down in periods?
Definition
because they get large, bulky, and farther away from the nucleus so they can give up their outer electrons easier whereas carbon they are close to the nucleus and don't want to give them up
Term
what are group or column 7 called?
Definition

halogens, they are very reactive and want to gain 1 electron

 

halogens lamps come from this

Term

what is ionization energy?

 

how does it trend?

Definition

the energy it takes to remove an electron, or the energy to make something into a cation

 

low to high is up and to the right

 

so generally Cs is really low and and He is really high 

 

 

Term
Pick 3 elements and do the electron configurations.
Definition
check on google
Term
Which elements have the highest second ionization energies?
Definition
alkali metals, they have a very big difference between their first and second
Term

what is electronegativity?

 

what is the trend on the periodic table?

Definition

how much an element hogs electrons in a covalent bond

 

up and to the right

 

Cs low, F highest (noble gases don't form covalent bonds)

 

same trend as ionization energy

 

 

Term

what is metallic nature in chemistry?

 

how does it trend?

Definition

a willingness to give away electrons

 

down and to the left it increases

 

Cs has has high metallic nature F has low

Term
how does atomic radius trend?
Definition

increases down and to the left, because when you move to the right, it increases your protons so it pulls in the electrons stronger

in a period, the more protons you have, the small the atom

Term
what is a metallic bond?
Definition

bonds that metals make,

 

they give up their electrons and form a sea of electrons they all share, the electrons can be moved around. This is why metals are maleable and good conductors

Term
what does empirical mean?
Definition

figured out through experience or experiment

 

ratio of elements in a molecule

Term
what is amu?
Definition

atomic mass units

 

the mass of the atom or molecule, it the weighted average of all the molecules or atoms in nature. C amu is 12.0107 so there is a lot more C with a mass of 12 then 14

 

amu is the mass of the neutrons + mass of protons

Term
what is a mole?
Definition

it avogadros number = 6.02 * 1023

 

1 mole of C twelve = 12 grams of C twelve

 

or 6.02 * 1023 atoms of C twelve = 12 grams of C twelve

 

it's the conversion from grams to amu's

 

1 gram = 1 mole of amu's

Term

how do you solve for mass composition or get empirical formula from mass composition?

 

9% Mg

91% I

Definition

assume there is 100 grams

9 grams of Mg

91 grams of I

 

 

MgI2

Term
what is pressure?
Definition

force/area

 

PV = nRT

 

assuming the particles aren't attacted to each other and the particle volumes are insignificant

Term

What is temperature?

 

what is heat?

Definition

temperature is the average kinetic energy of particles

 

heat is the transfer of energy from one substance to another measured in 1 calorie = 4.184 Joules

 

potential energy is in bonds

Term
what is the difference between mass and weight?
Definition

mass is the amount of matter in an object

 

weight is the amount of force pulling an object to the center of the earth

Term
what is the aufbau principle?
Definition
you always fill the lowest energy shell first with electrons
Term
What is Hunds rule?
Definition
when there is more than 1 subshell at a particular energy level, only one electron fills each subshell until each subshell has on electron.
Term
is an electrolyte ionically bonded or covalently bonded?
Definition
ionic, it disassociates into ions in water
Term

(1.5 * 103g) + (2.3 * 102g) =?

 

(9.25*10-2 m) * (1.37*10-5 m) =?

Definition

have to have same power for add and subtract = (1.73 * 103 g)

 

multiply the coefficients and add the exponents = (1.27*10-6 m2)

Term
how many significant digits are in 0.0023?
Definition

2 because you can write it as 2.3 *10-3

 

 

Term

how many sig figs?

 

0.000230340

Definition

6

 

zeroes inbetween non-zeroe numbers and after are significant.

Term

how many sig figs?

 

50,500?

Definition

3

if it doesn't contain a decimal, the zeroes after nonzero digits aren't normally considered significant

Term

how do you determine sig figs to report in you answer?

 

1) add/subtract

 

 

2) multiply/divide

Definition

1) fewest number of decimals

 

2) fewest # of sig figs in calculations (exact or counted #'s used in conversions don't count)

Term

what is the change from a gas to a solid called?

 

 

 

Definition
deposition
Term
what is the change from a solid to a gas called?
Definition
sublimation
Term
what is energy?
Definition
the ability to do work (a force of a certain magnitude that diplaces the object)
Term
what is a barometer?
Definition
an instument to measure pressure in mm Hg. It has a long tube upsidedown on a round container. As the pressure of the air goes up, it pushes the Mercury in the tube up. 760 mm Hg is 1 atm or atmospheric pressure at sea level
Term
what is a manometer?
Definition

an instrument to measure pressure of a gas ina container

 

a container connected to a U-shaped piece of glass with mercury in the bottom of the U

Term

what is Boyle's law?

 

suppose you have 5.00 liters of a gas at 1.00 atm pressure and then to decrease the volume to 2.00 liters. What's the new pressure?

Definition

Pressure and Volume have and inverse relationship, if volume goes up pressure goes down.

 

P1V1 = P2V2

 

2.5 atm

Term
What is Charle's law?
Definition

the relationship of Volume and Temperature is directly related

you have to use Kelvin

 

V1/T1 = V2/T2  when pressure is held constant and temp in K

 

 

Term
What is Gay-Lussac's law?
Definition

The relationship between the temperature and pressure of a gas is directly related. Increase temp and you increase pressure. (assuming volume and amount is constant)

 

P1/T= P2/T2

 

 

Term
what is Avogadro's law?
Definition

volume and moles or amount of particles are directly proportional

 

V1/n1 = V2/n2 

Term
What is the combined gas law?
Definition
P1*V1/T1 = P2*V2/T2
Term
what is van der Waal's equation?
Definition

you need it when you do not have ideal gases

 

(P+(an2/V2))*(V-nb) = nRT

Term
what is Dalton's law?
Definition

in a mixture of gases, the total pressure is the sum of the partial pressures of each individual gas.

 

Ptotal = Pa + Pb + Pc

Term
What is Graham's law?
Definition

how gases diffuse and effuse(Helium escaping through a rubber balloon over time)

 

v1/v2 = sqrt(M2/M1)

 

M = molecular or atomic weights

 

v = velocity of diffusion

Term
What is the conversion from moles to Volume for a gas at STP?
Definition
1 mol/22.4 L
Term

what is vapor pressure?

 

why would something want to evaporate?

Definition

the pressure at which the vapor and liquid pressures are at equillibrium

 

 

high kinetic energy(high temp)

low intermolecular forces (methane,carbon bonds-unlike water has hydrogen bonding)

light molecules

(these will have a high vapor pressure) high volitility

 

 

 

Term
what is the boiling point?
Definition
when the vapor pressure equals the atmospheric pressure
Term
what is heat of fusion?
Definition

the heat required to change from a solid to liquid state. for a period of heat and time, a solid doesn't increase in temp with added heat. The heat is used to break the bonds. So you can have 0 degree ice and 0 degree water

 

same as heat of melting

Term
what is heat of vaporization?
Definition

the additional heat to turn a liquid to a gas. at 100 degrees it takes additional heat to break the bonds and changes phases. You can have 100 dregree water and vapor

 

same as heat of condensation

Term
how do you convert Ka to pKa?
Definition
take the -log(Ka)
Term
how do you convert pKa to Ka?
Definition
Ka=10-pKa
Term
what are the solubility rules to determine what is precipitate?
Definition

Inorganic Compounds

Ammonium (NH 4 + ),potassium (K + ), sodium (Na + ) : All ammonium, potassium and sodium salts are soluble. Exceptions: some transition metal compounds.

Bromides (Br), chlorides (Cl) and iodides (I): Most bromides are soluble. Exceptions: salts containing silver, lead, and mercury.

Acetates (C2H3O2): All acetates are soluble. Exception: silver acetate is only moderately soluble.

Nitrates (NO3): All nitrates are soluble.

Sulfates (SO42–): All sulfates are soluble except barium and lead. Silver, mercury(I), and calcium sulfates are slightly soluble. Hydrogen sulfates (HSO4) (the bisulfates) are more soluble than the other sulfates.

Generally Insoluble Inorganic Compounds

Carbonates (CO 3 2– ), chromates (CrO 4 2– ), phosphates (PO 4 3– ), silicates (SiO 4 2– ): All carbonates, chromates, phosphates and silicates are insoluble. Exceptions: those of ammonium, potassium and sodium. An exception to the exceptions is MgCrO 4 , which is soluble.

Hydroxides (OH): All hydroxides (except ammonium, lithium, sodium, potassium, cesium, rubidium) are insoluble. Ba(OH)2, Ca(OH)2 and Sr(OH)2 are slightly soluble.

Silver (Ag+): All silver salts are insoluble. Exceptions: AgNO3 and AgClO4. AgC2H3O2 and Ag2SO4 are moderately soluble.

Sulfides (S2): All sulfides (except sodium, potassium, ammonium, magnesium, calcium and barium) are insoluble.

Aluminum sulfides and chromium sulfides are hydrolyzed and precipitate as hydroxides.

Term

steps to balance redox

 

Fe + Cl2 yields Fe3+ + Cl-

Definition
  1. write half reactions (LEO and GER)
  2. balance atoms other than O and H
  3. balance O's by adding water
  4. balance H's by adding H+
  5. balance charge by adding electrons
  6. make number of electrons equal and add half reactions
  7. if basic, add OH atoms to balance H+
Term
define allotrope
Definition
is the property of some chemical elements to exist in two or more different forms, known as allotropes of these elements. Allotropes are different structural modifications of an element;[1] the atoms of the element arebonded together in a different manner. For example, the allotropes of carbon include diamond (where the carbon atoms are bonded together in a tetrahedral lattice arrangement), graphite (where the carbon atoms are bonded together in sheets of a hexagonal lattice), graphene (single sheets of graphite), and fullerenes (where the carbon atoms are bonded together in spherical, tubular, or ellipsoidal formations). The term allotropy is used for elements only, not for compounds.
Term

define colligative properties

 

Definition

In chemistry, colligative properties are properties of solutions that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the type of chemical species present.[1] This number ratio can be related to the various units for concentration of solutions. Here we shall only consider those properties which result because of the dissolution of nonvolatile solute in a volatile liquid solvent.[2] They are independent of the nature of the solute particles, and are due essentially to the dilution of the solvent by the solute. The word colligative is derived from the Latin colligatus meaning bound together.[3]

Colligative properties include:

  1. Relative lowering ofvapor pressure
  2. Elevation of boiling point
  3. Depression of freezing point
  4. Osmotic pressure.

not density

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