General Chemistry I
A solution of K2SO4, which has a volume of 75.0 mL, contains 0.0048 moles of potassium ions. What is the molarity of the K2SO4 solution?
(0.0048 mol K^1+/0.075L) x (1mol K2SO4/2 mol K^1+) = 0.032M K2SO4
what is the mass of 0.75 mol C6 H12
(0.75 mol C6 H12) x ( 84g/ 1 mol C6H12) = 63 g
The density of a nucleus in a hydrogen atom is 23 x 10^17 kg/m^3. If a single H atom has a mass of 1.67x 10^-18ug, what volume in mL does the nucleus of this atom occupy
(1.67x10 ^-18ug) x (1g/10^6ug) x (1 kg/1000g) x (1 m^3/ 2.3x10^17 kg) x ( (100cm)^3/(1m)^3)) x (1mL/1 cm^3) = 7.26 x 10 ^-39 mL
what is the mass of 1.8 mol CO2
(1.8 mol CO2) x (44g/ 1mol CO2)= 79 g
how many moles of molecules are in a 10.0g sample of a SF6 compound? How many atoms are in each sample?
(10.0g) x (1mol SF6/ 146g) = 0.0685 mol SF6; (0.0685 mol SF6)x (7 moles of atoms/ 1 mol SF6) = 0.480 mol atoms
how many moles of molecules are in a 10.0g sample of a CCl compound? How many atoms are in each sample?
(10g) x (1 mol CCl4/ 154 g) = 0.0649 mol CCl4; (0.0649 mol CCl4)x (5mol atoms/1mol CCl4) = 0.325 mol atoms
how many moles of molecules are in a 10.0g sample of a C6H14 compound? How many atoms are in each sample?
(10g) x (1mol C6H14 /86.2g) = 0.116 mol C6H14 (0.116 mol C6H14) x (20 mol atoms/ 1 mol C6H14) = 2.32 mol atoms
how many moles of atoms in 14 mg Ag
(14mg Ag) x(1g Ag/1000mg Ag) x (1mol Ag/ 108 Ag) = 1.3 x 10 ^-4 moles
how many moles of atoms in 17g K
(17g Mg)x (1 mol Mg/24.3 Mg) = 0.70 mol Mg
How many moles of O2 needed to completely combust 2.18 moles of C3H6
(2.18 mol C2H6)x (9mol O2/2mol C3H6) = 9.81 mol O2
how many moles of atoms in 2.2 kg Fe
(2.2kg Fe) x (1000g Fe/1kg Fe) x (1 mole Fe/55.85g Fe) = 39 mol Fe
what is the mass of 2.5 mol CaCl2
(2.5 mol CaCl2) x (111g /1 mol CaCl2) = 2.8 x 10^2 g = 0.28 kg
A weather report indicates a barometric pressure of 29.2 in. What is this pressure expressed in torr?
(29.2 in) x (25.4 mm/1 in) = 742 mmHg= 742 torr
how many moles of atoms in 5.0g K
(5.0gK)x (1mol K/39.1g K) = 0.13 mol K
how many carbon atoms are in 56.0 g of sucrose (C11 H22 011, Mm=342.3 g/mol)
(56.0g)x(1 mol/342.3 g) x (6.02x 10^23 molecules/1 mol C11H22O11) x (11 C atoms/1 molecule) = 1.08x 10^24 C atoms
how many atoms in 6.08 g of SO2
(6.08g SO2) x (1mol SO2.64g SO2) x (6.02x10^23 molecules/1 mol SO2) x(3 atoms/ 1 molecule SO2) - 1.7 x 10^23 atoms
Effective nuclear charge
(Zeff) is the "positive charge" felt by a valence electron. Zeff increases across a period (less effective shielding). Zeff decreases as l increases. (s > p > d > f)
%yield =
(actual yield/theoretical yield) x 100
group
(or family) - one of the vertical columns in the Periodic Table. Elements within a group exhibit similar chemical properties
wavelength
(λ) the distance a wave travels in 1 cycle
frequency
(ν) cycles per second (Hz = s-1)
NH4
+1 ammounium ion
H3O
+1 hydronium ion
what is the oxidation number of carbon in C2O4 ^2-
+3 2x + (4)(-2) = -2
What is the charge in coulombs of a mole of electrons? (This amount of charge is called a Faraday.) The charge of an electron from Table 1.1 is -1.6 x 10-19 C
-(1.6×10-19C /electron) × (6.0×1023 /electrons) = -9.6×104 C/mol
C2H3O2
-1 acetate ion
ClO3
-1 chlorate ion
ClO2
-1 chlorite ion
CN
-1 cyanide ion
OH
-1 hydroxide ion
ClO
-1 hypochlorite ion
NO3
-1 nitrate ion
NO2
-1 nitrite ion
ClO4
-1 perchlorate ion
MnO4
-1 permanganate ion
O2
-2 peroxide ion
what is the oxidation number of carbon in CH4
-4 x + (4) (+1) =0
for a given value of l ml =
-l,....,0,....+l
Where possible, lone pairs in a five electron-group system occupy equatorial positions.
...
d = m/V
...
What is the oxidation number for carbon in C (graphite )
0
electronegativity x
0 covalent greater than 2 ionic greater than 0 but less than 2 polar covalent ionic has most diff in en covalent shares e polar partial transfer of e- ionic transfer e-
The lewis structure of NO2 can be represented as: what are the formal charges on the atoms in order from left to right -1, 0,0 -2, +1, 0 0, +1, -2 0,0,0
0,0,0
1 mL =
1 cm^3
which numbers are significant
1-9 all zeros between non zeros zeros at the end of a number to the right of a decimal point (.4500) 4 sigifgs
Consider the reaction of 0.30 mol K with O2, 4K + O2 → 2K2O How many moles of molecular oxygen are required? How many moles of potassium oxide would form? What mass, in grams, of potassium oxide would form?
1. (0.30 mol K) x (1mol O2/4mol K) = 0.075 mol O2 2.(0.30mol K) x (2mol K2O/ 4 mol K) = 0.15 mol K2O 3.Mm = 2 mol K x 39.1 g/mol + 1 mol O x 16.0 g/mol = 94.2 g/mol (0.15 mol K2O) x (94.2 g K2O/ mol K2O) = 14 g K2O
Kinetic Molecular Theory of Gases
1. Gaseous particles are separated by great distances. Point masses have mass but mass no volume.! 2. Gas particles are in constant motion and collide often. Collisions are perfectly elastic.! 3. Gas particles do not exert attractive or repulsive forces on each other.! 4. The average kinetic energy is proportional to the Kelvin temperature. Any two gases at the same temperature will have the same average kinetic energy.!
trigonal planar geometry
120 AX3 3 bonding groups bent v shaped AX2E less than 120 2 bonding groups
what is the molar mass of (NH4)2SO4
132.15 g/mol
Linear
180 AX2 2 bonding groups
Dalton's atomic theory
1804 1. Elements are composed of atoms, which are indivisible.! 2. Atoms cannot be created or destroyed.! 3. Compounds are formed when elements combine.
what is the i of: NaCl KNO3 Na3PO4 C6H12O6
2 2 4 1
CO3
2- carbonate ion
CrO4
2- chromate ion
Cr2O7
2- dichromate ion
SO4
2- sulfate ion
SO3
2- sulfite ion
R sub H=
2.18 x 10 ^-18J
c =
2.998 x 10 ^8 m/s
a mix of Heliox gas contains 4.22 moles of He, and 0.490 moles of O2. If the total pressure of gases in the tank is 200 atm, what is the partial pressure of O2.
20. 8 atm Xi O2 = (0.490 mol/0.490 + 4.22) = 0.104 Po2 = Xi o2 Ptotal - (0.104)(200 atm).
STP is ___K and 1 atm
273
balance C2H6 + O2→ CO2+ H2O
2C2H6 +7O2 → 4CO2 + 6H2O
balance Ca+O2→CaO
2Ca+O2→2CaO
what is the valence electron config for carbon
2s^2 2p^2
What are the n and l quantum numbers for the electrons with the highest energy in the following atoms: Na Fe Pb Se
3 0 3 2 6 1 4 1
In Ca3(PO4)2 how many atoms in Ca, P, and O how many moles in Ca, P, and O
3, 2,8 3,2,8
PO4
3- phosphate ion
You add 1.00 kg of ethylene glycol (C2H6O2, 62.07 g/mol) antifreeze to 4450 g of water in your car's radiator. What is the molality of ethylene glycol?
3.62m
what is the # of protons, symbol, name, and electron configuration of an element with 17 neutrons, 15 electrons and a net charge of zero
32/15 P 15 p phosphorus [Ne] 3s2 3p3
what is the valence electron config for magnesium
3s2
what is the valence electron config for chlorine
3s2 3p5
balance Al+O2→Al2O3
4Al + 3O2 → 2Al2O3
what is the valence electron config for cobalt
4s2 3d7
How many unpaired electrons are present in each of the following? manganese thallium sulfur bromine
5 1 2 1
Give the number of s, p, d, and f electrons in each of the following atoms: Na Fe Pb Se
5 6 0 0 8 12 6 9 12 26 30 14 8 16 10 0
r sub n =
5.393 x 10^-11m (n^2/Z)
Complete the symbol for 52^Cr. Find: #of protons, neutrons, electrons, net charge, element name, and electron configuration
52/24 Cr ^3+ p=24 n= 52-24 = 28 e= 24-3 = 21 net charge = 3+ chromium [Ar] 3d^3 Cr= [Ar] 4s^1 3d^5 log 4's then 3d e-
avogadro's number
6.022 X 10 ^23
h =
6.626 x 10 ^-34 J*s
balance CO2+H2O→C6H12O6+O2
6CO2 +6H2O → C6H12O6 + 6O2
Octrahedral geometry
90 degress all over AX6 octahedral 6 bonding groups AX5E square pyramidal 5 bonding groups less than 90 AX4E2 square planar 4 bonding groups 90 degrees
mass number
A number of protons + number of neutrons atomic number (Z) + number of neutrons
AXmEn
A central atom X surrounding atom E nonbonding valence electron group m and n are integers
What is a dynamic equilibrium? Give two examples dynamic equilibria.
A dynamic equilibrium occurs when the rates of two opposing processes are equal. The result is that there is no net change although both processes continue.
mole
A mole (mol) is an amount of a substance where the formula mass (amu) of a formula unit = mass in grams.!
Explain how snow can disappear without melting.
A solid can be converted directly to the gas in a process called sublimation. If the temperature remains below the melting point, the solid does not melt. However, it will slowly sublime.
What is a unit cell?
A unit cell is the smallest repeat unit of the crystal.
trigonal bipyramidal
AX5 90 and 120 trigonal bi pryamidal 5 bonding groups AX4E seesaw less than 90 and less than 120 4 bonding groups AX3E2 t shaped 3 bonding groups less than 90 (ax) AX2E3 linear 2 bonding groups 180 degrees
What is the Ksp of AgCN if the concentrations of silver and cyanide ions in a saturated solution of silver cyanide are each 1.1x 10-8 M?
AgCN(s) Ag1+(aq) + CN1-(aq); Ksp = [Ag1+][CN1-] = (1.1 x 10-8)(1.1 x 10-8) = 1.2 x 10-16
Explain why the temperature of a solid liquid mixture does not change when it is heated.
Any additional heat that is added is used to melt the solid (increase the potential energy) not to increase the temperature (increase the kinetic energy).
which of the following would you expect to be diamagnetic Ar, Cs, C, or Fe
Ar all e- paired
halogen in the same period as lead
At
metalloid in the same family as gallium
B
Which of the pairs are most likely to form an ionic compound Cs and Fr As and Ge Ba and Br C and H
Ba and Br
His theory of the atom included fixed circular orbits for atoms
Bohr
Explain why bubbles form when a liquid boils.
Bubbles are cause by the molecules in the liquid that have sufficient kinetic energy to escape the liquid but are not at the surface. At the boiling point, the pressure in these bubbles is equal to the external pressure, so they do not collapse.
nonmetal in the same family as germanium
C
If the wavelength is 750, what is the frequency (s-1), Energy per photon, and energy per mole of photons (J/mol).
C = lambda v E = hv v= (2.998x 10^8 m/s) / (740 x10 ^9 m) = 3.997 x 10^14 s-1 Frequency = 4.00 x 10^14 E = (6.626x 10^-34 J*s)(3.997x 10 ^14 s-1) = 2.6486x 10^-19 J EperP = 2.65x10^-19 Emol= 6.02x10^23 photons.mol x (2.64865x10^-19J/photon) = 1594x10^8 J
K (temperature) =
C+ 273.15
Combustion Analysis
C?H?O? + O2 (g) (excess) --> CO2 (g) + H2) (g) unbalanced
Which molecule has the strongest intermolecular forces HCCH H2CCH2 H3CCH3 Ch3OH
CH3Oh
Rank Ch3F, CH3OH, and CH4 by boiling point, from lowest to highest and list the strongest type of intermolecular forces
CH4<CH3H<Ch3OH ch4 LDF CH3F dipole dipole Ch3OH hydrogen bonding
what is the cation, anion, and name of CaF2
Ca2+ F- Calcium fluoride
Indicate the substance with the higher melting point in each pair. Explain your choice. b. CaF2 or CS2
CaF2 is ionic while CS2 is molecular. Ionic bonds must be broken in order to melt an ionic solid while only relatively weak dispersion forces must be overcome to melt CS2. CaF2 has a much higher melting point. CaF2 is a solid at room conditions while CS2 is a liquid.
What is the oxidation number of Ti in Calcium Tinanate
CaTi O Ca -- 1 (+2) O3 -- (-2) 3 +2 +x = 6 = 0 x -4
What is the hybridization on the central atom in each of these ions: NO2 ^-1 N3^-1 ClO2 ^-1
Central atom electron regions and hybridization 2 bonding + 1 lone pairs = 3 sp2 2bonding+0lonepairs=2 sp 2 bonding + 2 lone pairs = 4 sp3
What is the hybridization on the central atom in each of the molecules: PF3 COCl2 BF3
Central atom electron regions and hybridization 3bonding+1lonepairs=4 sp3 3 bonding + 0 lone pairs = 3 sp2 3bonding+0lonepairs =3 sp2
How many valence electrons participate in bonding the polyatomic ion ClO2-
Cl--7 O -- 6x2 + charge = 7+12+1=20e-
What are clays? Why do some clays swell in the presence of water while others do not?
Clays are also composed of Al, Mg, and/or Fe and Si and O. They are two dimensional layered structures. In one type of clay (kaolinite), the layers hydrogen bond, which reduces the space between the layers. Kaolinites do not swell because water cannot get between the layers. In smectic clays, the hydrogen bonding sites are burried within the layers, so there is no hydrogen bonding between layers. Consequently the layers are farther apart and water can get in between the layers, which causes the clay to swell.
what is the formula and name for a cation of Co^3+ and an anion of NO3^-
Co(NO3)3 cobalt (III)nitrate
Which of the following substances has a delocalized pi system HCCH CO3^2- CH3OH
Co3^2-
how to do empirical formulas
Convert the mass of each element to moles using the molar mass from the periodic table. Divide each mole value by the smallest number of moles calculated. Round to the nearest whole number. This is the mole ratio of the elements and is represented by subscripts in the empirical formula.
The threshold frequency of Cs is 4.38 x 1014 Hz . Calculate the threshold energy and the wavelength of an equivalent photon. (There is no ejected electron.)
E0 =hν0=hc/λ0 E0= (6.626 x 10-34 J•s) (4.38 x 1014 s-1) = 2.90 x 10-19 J λ0 =c/ν0 =3.00x108 ms-1/4.38x1014 s-1 =6.85x10-7 m =685nm
calculate the energy, frequency, and wavelength for the n=5 to n =2 electronic transition in a hydrogen atom
E= 2.18 x 10 ^-18J (1/5^2) - (1.2^2) = -4.58x10^-19 J/photon = E v=E/h= 4.58x10^=19 J/ 6.626x10 ^-34 J*s = 6.91x10^14 s-1 =v lambda = c/v = (2.998 m/s x10^8) / (6.91 x10^14 s-1) = 434nm
Photoelectric effect
Einstein: Light has particulate behavior (photons)
Group the following elements in pairs that are likely to have similar chemical properties: Ca, S, Sr, He, O, Ar.
Elements in a family are similar: Ca & Sr (2A) S & O (6A) He & Ar (8A)
how to find En for an element
En = -RH ( Z^2/n^2 ) for hydrogen (1/n^2)
Atomic line spectra
Energy of atoms is quantized; photon emitted when electron changes orbit.
The Ksp of iron(II) hydroxide is 8.0 x 10-16. What is the maximum concentration of Fe2+ ions that can exist in a solution in which [OH1-] = 1.0 x 10-7 M?
First, write the equilibrium reaction and the Ksp expression Fe(OH)2(s) Fe2+(aq) + 2OH1-(aq) Ksp = [Fe2+][OH1-]2 = 8.0 x 10-16 Next, solve the Ksp expression for the concentration of Fe2+ and substitute the know values. [Fe 2+]= (Ksp/[OH1-]2) =(8.0x10^-16)/(1.0×10-7)2 =8.0x10^-2 M
Oxygen can have a positive oxidation state when bound to only one element. What is the element? Use orbital energies to explain why this is so.
Fluorine in the only element with priority over oxygen that forms a negative ion. When O and F bond, F is -1, so O must be positive. The compound they form is OF2, in which case the O is +2. The reason is that fluorine is the only element that is more electronegative, which means that its valence orbitals are lower in energy than those on O. Consequently, the bonding electrons are assigned to the fluorine when assigning oxidation states.
gallium(III) oxide
Ga2O3
electromagnetic spectrum rays, wavelength, frequency, wavelength of visible light
Gamma X ultra violet visible infrared microwave radio wave gosh, xavier's, uncle is mega rad wade! wavelength (nm) 10^-3 10^-1 10 10^3 10^5 10^7 10^9 10^11 frequency (Hz) 10^20 10^18 10^16 10^14 10^12 10^10 10^8 10^6 ROY G BIV 400blue; 500 green, 600 orange, 700 red
how to get molecular formulas
Get the mass of each element by assuming a certain overall mass for the sample (100 g is a good mass to assume when working with percentages). (.7546) (100 g) = 75.46 g C. ... Convert the mass of each element to moles. ... Find the ratio of the moles of each element. ... Use the mole ratio to write the empirical fomula.
List the following bonds in order of increasing bond length: H-Cl, H-Br, H-O.
H-O < H-Cl < H-Br. The order of increasing atom size.
Which of the molecules has the shortest C-C bond HCCH H2CCH2 H3CCH3
HCCH
which of the following has the largest bond angles around the carbon atoms HCCH H2CCH2 H3CCH3
HCCH
Strong acids
HCl, HBr, HI, HNO3, HClO4, H2SO4
which has the highest first ionization energy K, B, N, or He
He
In which of the following molecules is hydrogen bonding between like molecules important?
Hydrogen bonding is important only in compounds with H-O, H-N or H-F bonds. Consequently, only ethanol molecules can hydrogen bond to one another.
Indicate whether each of the following substances would be more soluble in H2O or C6H14: a) HF b) CH3OH c) NaC2H3O2 d) CH4
Hydrogen bonding substances (HF and CH3OH) and ionic substances (NaC2H3O2) are more soluble in water than in a nonpolar solvents, while nonpolar substances (CH4) are more soluble in nonpolar solvents. h20 h20 h20 c6h14
law of multiple proportions
If elements A and B react to form two compounds, the different masses of B that combine with a fixed mass of A can be expressed as a ratio of small whole numbers. Example: Carbon Oxides I & II Carbon Oxide I : 57.1% oxygen and 42.9% carbon Carbon Oxide II : 72.7% oxygen and 27.3% carbon Assume that you have 100 g of each compound. In 100 g of each compound: g O = 57.1 g for oxide I & 72.7 g for oxide II g C = 42.9 g for oxide I & 27.3 g for oxide II
Explain why many gases are liquefied by increasing the pressure.
Increasing the external pressure increases the boiling point. Thus, if the pressure of the gas is increased to the point that the boiling point drops below the external pressure, the gas liquefies.
If a photon ejects an electron from a metal with 7.29x10^-20 J of kinetic energy, what is the threshold frequency of this metal?
KE/h = v-vo = 7.29 x 10^-20J / 6.626x10^-34 J*s = 4.00x10^14 s-1 -v0 -v0 = -2.8992 x10^14 s-1 vo = 2.90 x10^14 s-1
Π = iMR
M = molarity R = 0.0821 atm·L/mol·K T = Kelvin temperature i = van't Hoff factor
Dilutions formula
M1V1= M2V2
considered the father of the modern periodic table
Mendeleev
which atom has the smallest radius Na+ Mg ^2+ Ne N^3-
Mg^2+
Determined the charge of an electron
Millikan's Oil Drop Experiment
In a 5.00 g sample of Ca2 S3, how many moles of Ca2S3 does it contain? How many moles of sulfur does it contain ? How many grams of sulfur does it contain?
Mm = (2mol Cal) (40.0g/mol) + (3mol S) (32.0 g/mol) = 176 g/mol n= (5.00 g Ca2 S3)x (1mol/Ca2 S3/ 176g Ca2S3) = 0.0284 (0.0284 mol Ca2S3) x (3 mol S/1 mol Ca2S3) = 0.0852 mol S (0.0852 mol S) x (32.0 g S/mol S) = 2.73gS
manganese(II) sulfide
MnS
balance using smallest integer coefficients N2+H2→NH3
N2+3H2→2NH3
Describe nanotubes and explain why they are important. How is the structure of a nanotube related to that of graphite?
Nanotubes are cylinders of carbon. Their structure can be viewed as a sheet of graphite that has been rolled into a cylinder. They are metallic conductors or semiconductors depending on how the sheet is rolled. They have been used as molecular wires and in the construction of transistors and logic devices. They are important building blocks in the new field of molecular electronics.
observation
Natural phenomena and measured events; can be stated as a natural law if universally consistent.
law of definite proportions
No matter the source, a particular compound is composed of the same elements in the same parts (fractions) by mass.
A solution is known to contain one of the following cations: Na1+, Ag1+, or Fe2+. The addition of chloride ion to part of the solution had no apparent effect, but addition of CrO42- ion resulted in a precipitate. What is the identity of the cation in the original solution?
No precipitate formed when Cl1- ion was added, so the solution does not contain Ag1+. The precipitate that forms with the addition of CrO42- ions must be FeCrO4 because Na2CrO4 is soluble. Thus, the solution contains Fe2+ ions.
What is the pressure inside a 7.20-L container filled with 0.254 moles of CO2 at 35 oC?
P = nRT/V (O.254) (0.0821) (308)/ 7.20 =0.892 atm
balance P4O10 + H2O → H3PO4
P4O10 + 6H2O → 4H3PO4
You are asked to design an air bag for a car. The bag should be filled with gas to a pressure of 829 mm Hg, at a temperature of 22C . The bag will have a volume of 45.5 L once it has expanded upon an impact. How many grams of N2 (g) must be produced to fill the air bag? (760 mm Hg = 1atm, R = 0.0821 L*atm/mol*K).
PV = nRT n---> g n= (PV)/(RT) =((829 mmHG x (1atm/760mmHg)) x(45.5L) divided by ((0.821 (L*atm/mol K)) x (22+ 273K) = 2.049 moles N2 2.049 moles N2 x (28.02gN2/1mol N2) = 57.4 g N2
FF2 (28.00g/mok( gas is added into a 1.33L chamber to a pressure of 2.70 atm at 4C . What is the mass of F2 in this chamber?
PV=nRT where R = 0.0821 L*atm/mol*K n=PV/RT =(2.70 atm)(1.33L)/ (0.9821 L*atm/mol*K)(4C+273K) =0.1579 mol x (28g/1 molF2) = 4.42g F2
What's the formula if the compound formed between Pb and Cl, given the formulas TlCl and BiCl3
Pb falls between Tl and Bi on the periodic table so the number of chlorine atoms per lead atom is predicted to be between the 1:1 and 3:1 ratios of the given compounds. Consequently, the formula is PbCl2
Blackbody radiation
Planck: Energy is quantized; only certain values allowed
proposed that the energy of a wave is quantized
Plank
only metal in the same group as sulfur
Po
experiment
Procedure to test hypothesis; measures one variable at a time.
R =
R = 0.0821 atm·L/mol·K
Delta E -
RH [(1/n^2 sub i ) - (1/n^2 sub f)]
which atom is most electronegative out of S, Sg, Sn, and Sr
S
what's the formula if the compound formed between Sc and Br, given the formulas KBr and CaBr2
Sc is after Ca so the Sc:Br ratio should be the one following the trend of 1:1 and 1:2. The formula should be ScBr3.
List one set of possible quantum numbers for the last electron lost by a scandium atom to form Sc^3+ n= l= ml= ms=
Sc: [Ar] 4s2 3d1 losc 4s e- 1st, 3de- last n=3 l=2 ml= -2,-1, 0,1,2 (any) ms= +½ or -1/2
What is the symbol of the following species: 34p+ 36 e 26 p + 23 e 47p + 47e
Se^2- Fe^3+ Ag
model (theory)
Set of conceptual assumptions that explains data from accumulated experiments; predicts related phenomena
shielding of electrons
Shielding by other electrons reduces the full nuclear charge to an effective nuclear charge, Zeff = Z - σ
How does the thermal energy compare to the energy of attraction between molecules in a solid and in a gas?
Solid: Energy of attraction > Thermal energy Gas: Thermal energy > Energy of attraction
Once the maximum amount of solute is dissolved, the solution is considered to be: soluble if slightly soluble if insoluble
Soluble if [solute] ≥ 0.10 M Slightly soluble if 0.01M < [solute] < 0.10 M Insoluble if [solute] ≤ 0.01 M
What are the two steps involved in solvation?
Solvation consists of creating cavities in the solvent and placing the solute particles in the cavities.
strontium bromide
SrBr2
monoprotic acids HCl-> H+ + Cl- HNO3 -> H+ + NO3- CH3COOH double yields H++CH3COO-
Strong electrolyte, strong acid Strong electrolyte, strong acid Weak electrolyte, weak acid
diprotic acids H2SO4 yields H+ + HSO4- HSO4 double yield H+ + SO42-
Strong electrolyte, strong acid Weak electrolyte, weak acid
Prefixes used with SI Units
T G M k h d u d c m u n p 12 9 6 3 2 1 0 -1 -2 -3 -6 -9 -12 tera giga mega kilo hecto deca (base) deci centi mili micro nano pico
hypothesis
Tentative proposal that explains observations.
further experiment
Tests predictions based on model
Explain the hydrophobic effect.
The CH2 groups of organic compounds are nonpolar and interact very poorly with water. Compounds with many CH2 groups interact so poorly with water that they are called hydrophobic. When a hydrophobic compound is placed in water, the water molecules orient so as to minimize their interaction with the compound. As a result, hydrophobic compounds are not soluble in water.
What is the Fermi level
The Fermi level is the energy of the occupied orbital that has the greatest energy.
What is a band gap?
The band gap is the energy separation between the valence and conduction bands.
Explain why the boiling point of a substance increases as the pressure increases.
The boiling point is the temperature at which the vapor pressure equals the external pressure. If the external pressure is increased, then the temperature must increase to produce the greater vapor pressure.
Consider the U-V, W-X, and Y-Z bonds. The valence orbital diagrams for the orbitals involved in the bonds are shown in the margin. Use an arrow to show the direction of the bond dipole in the polar bonds or indicate "not polar" for the nonpolar bond(s). Rank the bonds in order of increasing polarity.
The bond dipole points toward the more electronegative atom in the bond, which is the atom with the lower energy orbital. The magnitude of the dipole increases as the electronegativity difference (orbital energy difference) increases. The W-X bond is not polar because the orbital energies of W and X are identical, and the Y-Z bond in more polar than the U-V bond because the energy separation of the bonding orbitals is greater. W-X < U-V < Y-Z
What two opposing forces dictate the bond length? (Why do bonds form and what keeps the bonds from getting any shorter?)
The bond length is the distance at which the repulsion of the two nuclei equals the attraction of the valence electrons on one atom and the nucleus of the other.
Explain at the molecular level why graphite can be used as a lubricant but diamond cannot.
The covalent bonds in graphite are in a plane while the planes interact through dispersion forces. The dispersion forces are weak and the planes slide freely over one another making graphite a lubricant. In diamond, the covalent bonding is three-dimensional and there are no weak interactions.
UseCoulomb'slawtoexplainwhyNa1+ionsandtheCl1-ionsexistasseparatedionsinliquidwater(ε=79) but pair together as uncharged NaCl units in liquid carbon tetrachloride (ε = 2).
The force of attraction between the opposite charges is given by Coulomb's law to be F ∝ (+1)(-1) / εr2. The greater the force of attraction, the more likely it is that the charges will pair. The value of e in water is about 40 times greater than in carbon tetrachloride. This means that the ions are 40 times more likely to pair in carbon tetrachloride than in water, or that the distance between the ions in carbon tetrachloride must be 40 ~ 6 times greater than in water to experience the same force of attraction.
Indicate the substance with the higher melting point in each pair. Explain your choice. a. CsBr or AlN
The force of attraction of two ions depends on the product of the charges on the ions. Therefore, the force of attraction between an Al3+ ion and a N3- ion is greater than that between a Cs1+ ion and a Br1- ion. Consequently, AlN has the higher melting point.
Define the term "heat of fusion". The heat of fusion of water at 0 oC is 6.0 kJ/mol. Write the chemical equation for the process to which this number applies.
The heat of fusion is the heat required to melt some amount, usually a mole or a gram, of substance. The "heat of fusion of water" applies to the following process H2O(s) → H2O(l), i.e., to the melting of one mole of water at its melting point.
Differentiate between a monolayer and a micelle. Under what conditions is a detergent expected to form each?
The hydrophobic tail of a detergent avoids interacting with water in one of two ways. If the concentration of the detergent is very small, then the tails do not enter the water. Rather, the polar head interacts with the water while the hydrophobic tail sticks out of the water forming a monolayer across the top of the water. With an increase in concentration and some agitation, the tails are forced into the water where they interact with one another by forming small spheres called micelles. The surface of the spheres is composed of the polar heads, which interact with the water while the interior of the micelles consists of an organic solvent comprised of the hydrophobic tails.
Use ionization energies to explain why +4 ions are very rare.
The ionization energy increases with each electron that is removed because the effective nuclear charge increases with each removed electron. Thus, removing an electron from a +3 ion to produce a +4 ion requires a substantial amount of energy.
limiting reactant
The limiting reactant will be completely used up in the reaction. The reactant that is not limiting is in excess - some of this reactant will be left over.
How can the number of electrons involved in metals and nonmetals achieving noble gas configurations be predicted for the main group (A Groups) elements?
The number of electrons gained by a nonmetal is eight minus its group number. The number lost by a metal is equal to its group number.
Why did not the oil droplets in Millikan's experiment all have the same charge? What did the charges all have in common?
The number of electrons that adhered to the droplet varied, so the charge on the droplets also varied. The observed charges were all multiples of one number, the charge on the electron.
Which has a greater potential energy at 270 K, ice or water vapor? Explain.
The potential energy of the vapor is greater than that of the solid at any temperature.
solubility
The solubility of a compound is defined as the amount of the compound that dissolves in a certain amount of liquid. !
solute vs solvent
The solvent is usually the substance in a solution that is in the greatest amount. A solute is a substance that is dissolved in the solvent to make a solution. Water is the solvent and NaCl is the solute in a salt water solution.
Why are ionic substances solids under normal conditions?
To melt ionic substances, ionic bonds must be broken. Ionic bonds are strong interactions and require a great deal of energy to break. Thus, ionic substances are solids at normal conditions.
Define the term "isoelectronic".
Two atoms are isoelectronic when they have the same electron configuration.
What property of water makes it a good solvent for ionic compounds? How is this property expressed in Coulomb's Law?
Water is a good solvent for ionic compounds because it is a very polar molecule. This property of water is expressed by the dielectric constant, ε, in Coulomb's law.
gas in the fifth period
Xe
atomic number
Z number of protons in a nucleus
zinc acetate
Zn(CH3COO)2 or Zn(C2H3O2)2 acetate ion is represented by either formula. The first better indicates the structure of the ion, but both are common
Indicate the substance with the higher melting point in each pair. Explain your choice. c. H2S or ZnS
ZnS (zinc blende) is a covalent solid in which covalent bonds must be broken in the melting process. H2S is a molecular substance in which only dispersion forces and weak dipole-dipole forces must be overcome in the melting process. ZnS has a much higher melting point and is a solid at room conditions while H2S is a gas.
concentration of a nitrate ion in a 0.25 M KNO3 aqueous solution
[NO3 ^-1] = (0.25 mol KNO3/L) x (1mol NO3^-3/mol KNO3) = .25 M
concentration of a nitrate ion in a 0.10 M Al(NO3)3 aqueous solution
[NO3^-1] = ((.10 mol Al(NO3)3)/L) x (3 mol NO3^-1/ mol AlNO33) = 0.30M
concentration of a nitrate ion in a .20 M Ca(NO3)2 aqueous solution
[NO3^-1] = ((.20 mol Ca(NO3)2/ L) ( 2mol NO3^-1/mol Ca NO32) = 0.40 M
NH4 ^-1 is classified as
a cation
covalent bond
a chemical bond in which two or more electrons are shared by two atoms.
Indicate all of the forces that exist between molecules in the condensed states of the following: a) CCl4 b) CH2O dispersion, dipole-dipole c) CO2 d) HF dispersion e) H3C-OH
a dispersion b dispersion dipole dipole c dispersion , d dispersion dipole-dipole, hydrogen bonding e dispersion, dipole-dipole, hydrogen bonding
molecular formula
a formula giving the number of atoms of each of the elements present in one molecule of a specific compound.
empirical formula
a formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms
Miscibility
a liquid's ability to mix with another liquid without separating into two phases. ! • "Like dissolves Like"!
i is
a measure of solute particles are dissolved in a solution van't hoff factor
NH3 is classified as
a molecule
every triple bond has
a sigma and pi bond
every pi bond has
a sigma bond
H bonding
a special dipole-dipole interaction between a H bonded to an electronegative N,O or F atom, which can interact with a different O, N, or F atom (in another molecule).
compound
a thing that is composed of two or more separate elements; a mixture.
Consider the reaction of 6 mol Fe and 6 mol O2 to produce Fe3O4. a) Write the balanced chemical equation. b) How many moles of Fe3O4 could be produced? c) How many moles of excess reactant remain after the reaction is done?
a) 3Fe + 2O2 → Fe3O4 b) (6mol Fe) × (1molFe3O4 /3 mol Fe) =2molFe3O4; (6molO2) × (1molFe3O4 / 2mol O2)=3molFe3O4 Less can be made from Fe, so it is the limiting reactant and 2 mol Fe3O4 can be produced. c) DeterminehowmuchO is needed to react with the Fe: (6molFe) × (2molO2 / 3 mol Fe) =4mol O2 react There were 6 mol O2 initially and 4 mol react, so 2 mol O2 is left over.
List the following systems of charged particles from most negative to most positive energies of interaction. Also list the forces from most attractive to most repulsive. Use Equations 1.3 and 1.4, but we need only relative values. Therefore, k and ε can be ignored because they are constant. The charges are all multiples of the fundamental charge (1.6x10-19 C) and can be used without conversion. Finallly, all r values have the same units, so they do not have to be converted to meters. a) +2 and +2 charges separated by 10 nm b) -2 and +3 charges separated by 11 nm c) +2 and +1 charges separated by 6 nm
a) +2 and +2 charges separated by 10 nm Fa ∝ (+2)(+2)/10^2 = +0.0400 Ea ∝ (+2)(+2)/10 = +0.40 b) -2 and +3 charges separated by 11 nm Fb ∝ (-2)(+3)/11^2 = -0.0496 Eb ∝ (-2)(+3)/11 = -0.545 c) +2 and +1 charges separated by 6 nmFc ∝ (+2)(+1)/8^2 = +0.0556 Ec ∝ (+2)(+1)/6 = +0.50 Energy: most negative = Eb, Ea, Ec = most positive. Force: most attractive = Fb, Fa, Fc = most repulsive
Indicate which of the following substances has the higher boiling point and the type of force that is most responsible for the difference: a) CCl4 or CF4 CCl4 b) CH3-CH3 or CH3-NH2 CH3NH2 c) H2Se or Kr H2Se d) KF or HF KF
a) CCl4 - dispersion b)CH3NH2 - hydrogen bonding c) H2Se - dipole-dipole d)KF - ionic bonds
What are the predominant solute species in aqueous solutions of the following? Write the molecule or the separated ions as appropriate. a) CO2 b) CaCl2 c) PF3 d) K2Cr2O7 e) KOH
a) CO2 CO2 b) CaCl2 Ca2++2Cl1- c) PF3 PF3 d) K2Cr2O7 2K1+ + Cr2O72- e) KOH K1+ + OH1-
If metallic nickel crystallizes in an FCC unit cell... a. what is the mass in g of Ni (58.59g/mol) atoms in a unit cell b. what is the volume of the unit cell (in m^3) if the atomic radius of Ni is 1.24 A( 1A = 10 ^ -10m) c. what is the density of Ni (in g/m^3)
a. 4 atoms x (1 mol/6.02x10^23 atoms) x (58.5g/1 mol Ni) = 3.893 x 10^22g b. V- a^3 a= square root of 8*r a = Square root (8x 1.24A) = 3.507A V = (3.507A) = 43.14A^3 43.14A^3 x (10^-10m/1A)^3 = 4.31x10^-29 m^3 = V c. D= m/v =3.893 x 10^-22g/ 4.31 x 10 ^-29m^3 =9.02X10^6 g/m^3
A solution is prepared by dissolving 25.0 g of sodium sulfate in enough water to prepare 250. mL of solution. a) What is the molarity of sodium sulfate in the solution? b) What are the molarities of the sodium and sulfate ions in the solution? c) How many moles of sodium ions are present in 17 mL of the solution?
a. Mm of Na2SO4 = 2 mol Na x 23.0 g/mol + 1 mol S x 32.0 g/mol + 4 mol O x 16.0 g/mol = 142.0 g/mol 25.0 g Na2SO4 x (1 mol Na2SO4/L of solution) = 0.176 mol Na2SO4 Molarity = mol Na2SO4/L of solution = 0.176 mol / .250 L= 0.704 M b. [Na^1+] = (0.704 mol Na2So4/ L of solution) x (2mol Na^1+/ 1mol Na2SO4) = 1.41 M [SO4^2-] = (0.704mol Na2SO4/ Lsolution) x (1mol SO4^2-/ 1 mol Na2So4) = 0.704M c. 17mL x (1L/1000mL)x (1.41 mol Na^1+/L) = o.024mol Na+1
an electron with no kinetic energy can be ejected from a metal surface by a yellow photon with a wavelength of 612nm. a. whats the threshold frequency (s^-1) of this yellow photon b. Calculate the energy (J) of a single yellow photon c. If the total energy of the yellow photons striking the surface of the metal is 6.496 x 10^-18J. How many electrons could be ejected from the metal? d. If ultraviolet light is used to irradiate the metal instead of yellow light, will an electron be ejected from the metal? Why?
a. v=c/λ =3.00 x 10^8 m/s divided by 612 x 1-^-9m =4.90 x10^14 s-11 or H2 b. E=h/v = hc/λ (6.626 x 10^-34 J*s) x (4.90 x 10^14 s-1) E= 3.25 x 10^-19 J c. Etotal/ E photon = (6,496x 10 ^-18J)/(3.25 x 10-19 J) = 2o photons which equals 20 electrons 1 e- for each proton d. yes because UV light is higher frequency energy than yellow light and is above the threshold. These e- will have kinetic energy when ejected.
The green molecules (G2) react with the blue molecules (B2) to form molecules of G3B in the container shown in the text. Each circle represents one mole of the atom, and the atomic masses of G and B are 10 and 30, respectively. a) How many grams of G2 and B2 are in the container? b) How many G3B molecules can be produced? c) What is the balanced chemical equation for the reaction? d) How many grams of G3B would be produced? e) What mass of G2 or B2 molecules would be left over?
a.) The molar mass of G2 = 2(10) = 20 g/mol. There are 6 mol, so the mass of G2 is (6 mol)(20 g/mol) = 120 g The molar mass of B2 = 2(30) = 60 g/mol. There are 3 mol, so the mass of B2 is (3 mol)(60 g/mol) = 180 g b.)There are 6 mol G2 or 12 mol G atoms, which is enough to produce 4 mol G3B molecules. There are 6 mol B atoms, which is enough to proude 6 mol of G3B molecules. Thus G2 is the limiting reactant and only 4 mol G3B can be produced. c) 3G2 + B2 → 2G3B d)The molar mass of G3B is 3(10) + 30 = 60 g/mol. In part b, we saw that 4 mol is produced, so the mass is (4 mol)(60 g/mol) = 240 g G3B e) G2 is the limiting reactant, so no G2 remains. Use the balanced equation to determine how many moles of B2 would react with 6 mol G2. 6molG2 × (1molB2/3mol G2) =2molB2 react , so 3 - 2 = 1 mol remains or 60 g B2 remains. Note that conservation of mass is obeyed: initial mass=120gG2 +180gB2 =300g; final mass=240gG3B+60gB2 =300g.
Electronega1vity
ability of an atom to attract and hold onto electrons in a covalent bond. halogens group 8 aren't en en increases going up and across to right
triprotic acids H3PO4 H2PO4- H+ + H2PO4- H+ + HPO42- HPO42- H+ + PO43-
all weak electrolytes, weak acids
molarity M
amount (mol) of solute / volume (L) of solution
molality (m)
amount of (mol) of solute/ mass (kg) of solvent
base quantity of electrical current
ampere A
N^3- is classified as
an anion
Si is classified as
an atom, element
P4 is classified as
an element, and a molecule
CH3COO ^-1
anion
core electrons
are not in the outermost shell
dipole-dipole forces
attractive forces between polar molecules
Br is named
bromine
speed of light
c= 3.00 x 10^8 m/s
base quantity for luminous intensity
candela cd
C3H6O is classified as
compound, molecule
SO2 is classified as
compound, molecule
solubility rules
compounds of NH4^+1 and group 1A metal ions are soluble compounds of NO3-1 ClO4^-1 ClO3^1-, and C2H3O2^-1 are soluble compounds of Cl^1- Br^1- and I^1+ are soluble except those of Ag Cu Ti Hg and Pb compounds of SO4^2- are soluble except those of Ca^2+ Sr^2+ Ba^2+ and Pb^2+ most other ionic compounds are insoluble; i.e. most other combinations of ions form precipitates in water.
Cu is named
copper
Polar covalent bond or polar bond
covalent bond with greater electron density around one of the two atoms
Each of the following substances is a solid at room temperature. Indicate whether each is a molecular, metallic, ionic, or covalent solid. SI Ag I2
covalent solid metallic molecular
Davisson/Germer: Electron beam is diffracted by metal crystal
deBroglie: All matter travels in waves; energy of atom is quantized due to wave motion of electrons
Use electronegativities to describe the nature (purely covalent, mostly covalent, polar covalent, or ionic) of the following bonds. P-Cl K-O N-H TI-Br
deltax = 3.0 -2.1 =0.9 polar covalent delta x = 3.5 -0.8 =2.7 ionic delta x = 3.0-2.1 =0.9 polar covalent delta x = 2.8 - 1.7 =1.1
what is the name of N2S4
dinitrogen tetrasulfide
Metallic trends
down increasingly metallic to the left increasingly metallic most metallic at bottom left most non metallic going up the right
a mixture of atoms and elements has
each unit has one single atom
explained the photoelectric effect in terms of the particle nature of light, photons
einstein
shell
electrons with the same value of n
subshell
electrons with the same values of n and l
orbital
electrons with the same values of n, l, and ml
O3 is classified as
element and molecule
Fe is classified as
element, atom
true or false: CH3OH is expected to be more viscous than HOCH2CH2OH.
false more h - bonds (less viscous)
Intermolecularforces(IMF)
forcesbetweenmolecules.! - Extremely Important for behavior of condensed phases of matter.! - IMFs are generally weaker than bonds
Intramolecular forces
forceswithinmolecules! - Physical BONDS!
parts per million
g of solute/ 10^6 g of solution
mass fraction
g of solute/ too g of solution
nobel gases
group 8 inert/non reactive
Alkali metals
high reactive more reactive down a group group 1 lose 1 e- to form 1+ ions
solutions
homogenous mixture of two or more substances. Substances that exhibit similar types of IMFs dissolve in each other. "like dissolves like"
KE=
hv - hv0
valence electrons are
in the outermost shell. ! - largest value of n! - bonding electrons!
Solids have large ___ forces thus, motion is restricted
intermolecular
Fe is named
iron
order by decreasing radius and decreasing first ionization energy, and decreasing electro neg Na K Cl C Ge Sn Al C B Cs Zn O
k na cl cl na k cl na k sn ge c c ge sn c ge sn al b c c b al al b c cs zn o o zn cs o zn cs
base quantity of temperature
kelvin K
base quantity of mass
kilogram kg
Pb is named
lead
on the phase diagram, what phase is most dense, what is the triple point, what is the critical pint, what process occurs at point B, lowest point, how to find the boiling point
liquid triple point is when the substance can be either a solid liquid or gas the critical point is the highest point E sublimation and deposition happens at the lowest point, point B the boiling point is found near the gas at the end.
Relative Strength of interactions affecting bond angles:
lone pair-lone pair > lone pair-bonding pair > bonding pair-bonding pair
Mn is named
manganese
Surface Tension
manifestation of cohesive forces between liquid molecules, where they tend to minimize their surface area.
Hg is named
mercury
ionic compounds and naming
metal and non metal name of cation (metal) and base name (nonmetal) with ice NaCl sodium chloride
most elements listed in the periodic table are
metals
base quantity of length
meter m
base quantity for amount of substance
mole
unsaturated solution
more solute can dissolve
supersaturated solution
more than the max rampant of solute is present solute will precipitate out
which transition shown here will emit a photon with the shortest wavelength n=4 to n=64 n= 3 to n =1 n=2 to n=5 n=10 to n=2
n=3 to n=1 has highest E
PV=
nRT
True or false: CH3F is capable of forming hydrogen bonds
no H-F bond FALSE
pauli exclusion principle
no two electrons in an atom can have the same four quantum numbers.
Identify each of the following as a weak, strong, or non electrolyte: CCl4 H2CO3 CH3OH NH4NO3 HNO3
non weak (acid but not strong) non strong strong (strong acid)
qualitative observation
non-measured object or property without numbers. i.e. heavy rock, water sample contains a small amount of benzene, colors forming from a reaction.
e-configuration and number of valence electrons 1A
ns^1 1
e-configuration and number of valence electrons 2A
ns^2 2
e-configuration and number of valence electrons 3A
ns^2 np^1 3
e-configuration and number of valence electrons 4A
ns^2 np^2 4
e-configuration and number of valence electrons 5A
ns^2 np^3 5
e-configuration and number of valence electrons 6A
ns^2 np^4 6
e-configuration and number of valence electrons 7A
ns^2 np^5 7
e-configuration and number of valence electrons 8A
ns^2 np^6 8
Which is the most electronegative atom in each of the following groups? NOP O S Se Si P S
o o s
quantitive observation
observed object or property is measured or quantified. i.e. weight, mass, concentration, volume, etc
period
one of the horizontal rows in the Periodic Table. As one progresses across the elements in a period, properties change gradually from one extreme to another.
resonance structure
one of two or more Lewis structures for a single molecule that cannot be represented accurately by only one Lewis structure. not real bonding depictions
linear atomic mixed orbitals formed hybridized orbitals remaining
one s one p two sp two p
tetrahedral atomic mixed orbitals formed hybridized orbitals remaining
one s three p four sp^3 none
trigonal bipryramidal atomic mixed orbitals formed hybridized orbitals remaining
one s three p one d five sp^3d four d
octahedral atomic mixed orbitals formed hybridized orbitals remaining
one s three p two d six sp^3d^2 three d
trigonal planar atomic mixed orbitals formed hybridized orbitals remaining
one s two p three sp^2 one p
colligative properties depend
only on the number of solute particles not the type.
Amorphous solids
order over only very short distances (local order)
what are the protons, neutrons, and electrons of: 207^Pb^2+
proton = 82 neutrons = 207-82 = 125 electrons = 82-2 = 80
dynamic equilibrium
reached when the rate of evaporation and condensation are equivalent.
showed that the nucleus is a dense region a the center of the atom
rutherford's gold foil experiment
base quantity of time
second
Si is named
silicon
Ag is named
silver
Na is named
sodium
alkaline earth metals
somewhat reactive readily lose 2 electrons to form 2+ ions group 2
what is the hybridization around nitrogen in NO2
sp^2
Sr is named
strontium
chemical properties
substance is converted to another substance
physical properties
substance retain identity
pure substance
substances that are made of only one type of atom or molecule, and the purity of a substance is the measure of the extent to which a given substance is pure. The physical properties of a pure substance include well-defined melting and boiling points.
critical temperature (Tc)
temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure.
tetrahedral geometry
tetrahedral AX4 109.5 4 bonding groups AX3E trigonal pyramidal less than 109.5 3 bonding groups AX2E2 bent v shaped less than 109.5 2 bonding groups
each electron configuration given below is supposed to be for a sulfur atom in its ground state. for each config, say what part is wrong and explain why based on the rule or principle violated in each case [Ne] 3s^1, 3p^5 [Ne] 3s^4, 3px^2, 3py^2, 3pz^0 [Ne] 3s^3, 3p^3
the 1 on 3s^1 is wrong Aufbau filing order violated. this is an excited state everything at the top (^_) is wrong Hands rule violated the ^3 in the 3s^3 is wrong pauli exclusion principle should be [Ne] 3s^2 3p^4
actual yield
the actual amount of product formed
bond angle
the angle formed by the nuclei of two surrounding atoms with the nucleus of the central atom
theoretical yield
the calculated amount of product that could form if the reaction goes to completion.!
Polarizability
the ease with which the electron distribution in the atom or molecule can be distorted. Polarizability increases with: • greater number of electrons • more diffuse electron cloud Dispersion forces usually increase with molar mass. 
Electromagnetic radiation
the emission and transmission of energy in the form of electromagnetic waves. (Maxwell, 1873)
amplitude
the height of a wave crest or depth of a trough
saturated solution
the maximum amount of solute is dissolved
critical pressure (Pc)
the minimum pressure that must be applied to bring about liquefaction at the critical temperature.
Osmosis
the movement of solvent particles from a dilute solution to a concentrated solution through a semipermeable membrane.
vapor pressure
the pressure exerted by the vapor on the liquid
Osmotic pressure
the pressure that must be applied to prevent the net flow of solvent.
Viscosity
the resistance of a liquid to flow
Sn is named
tin
what is the name of S3O8
trisulfur octoxide
true or false: all ideal gases have the same average kinetic energy at the same temperature
true
true or false: kinetic molecular theory assumes there are no attractive or repulsive forces between particles
true
Crystalline solids
well defined repeating patterns (long range order)
what numbers are not significant
zeros for cosmetics alone infant of a decimal. 0.--- zeros used to locate a decimal point .004
Bonding order =
½ (BE-ABE)
boiling-point eleva2on
ΔTb =Tb -T°b= iKbm
freezing-point depression
ΔTf =T°f -Tf = iKfm
osmo2c pressure (π)
π = iMRT
Covalent Crystals
• Lattice points occupied by atoms • Held together by covalent bonds • Hard, high melting point
Ionic Crystals
• Lattice points occupied by cations and anions • Held together by electrostatic attraction • Hard, brittle, high melting point • Poor conductor of heat and electricity
Metallic Crystals!
• Lattice points occupied by metal atoms • Held together by metallic bonds • Soft to hard, low to high melting point • Good conductors of heat and electricity
Molecular Crystals
• Lattice points occupied by molecules • Held together by non-covalent intermolecular forces • Soft, low melting point • Poor conductor of heat and electricity
What counts as a group of electrons?
• single bond • double bond • triple bond • lone pair • free radical
unit cell has:
⅛ atom at 8 corners ½ atom at 6 faces
vapor-pressure lowering
∆P1 = X2P°1
nomenclature of oxyanions
prefix per suffix -ate +7, XO4 ^-1 -ate +5, XO3 ^-1 -ite +3, XO2 ^-1 prefix hypo suffix -ite +1, XO ^-1
