Combo with "chem lab final" and 2 others
n=g/M
(P+an/v2)(V-nh)=nRT
V'1/p
(v1/v2)=(p2/p1)
V'T
(v1/v2)=(t1/t2)
What is the only possible value of mℓ for an electron in an s orbital?
0 Since the allowed values for mℓ range from −ℓ to +ℓ, once you know the value for ℓ you know the values for mℓ.
change 0.25g Al to moles
0.25/27+0,009M
how many grams of copper were produced?
0.51g CuCl/134.4g X 3/3 X 63.5Cu/1 mol= .24g Cu
if .51 g of CuCl2 is used =, how many g of Al must be used?
0.51g x 1mol/135g x 2/3 x 27/mol= 0.068g Al
Aufbau Principle
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s
Give the complete ground-state electron configuration for silicon (Si).
1s^2 2s^2 2p^6 3s^2 3p^2 using ground-state electron [Ne]3s^23p^2
copper (Cu) using noble-gas shorthand.
1s^22s^22p^63s^23p^64s^13d^10 [Ar]4s^13d^10
Ag₂O → Ag + O₂
2Ag₂O → 4Ag + O₂
Al + Fe₃N₂ → AlN + Fe
2Al + Fe₃N₂ → 2AlN + 3Fe
Al₂O₃ → Al + O₂
2Al₂O₃ → 4Al + 3O₂
BF₃ + Li₂SO₃ → B₂(SO₃)₃ + LiF
2BF₃ + 3Li₂SO₃ → B₂(SO₃)₃ + 6LiF
Fe + H₂O → Fe₃O₄ + H₂
3Fe + 4H₂O → Fe₃O₄ + 4H₂
H₂ + N₂ → NH₃
3H₂ + N₂ → 2NH₃
KOH + H₃PO₄ → K₃PO₄ + H₂O
3KOH + H₃PO₄ → K₃PO₄ + 3H₂O
ZnS + AlP → Zn₃P₂ + Al₂S₃
3ZnS + 2AlP → Zn₃P₂ + Al₂S₃
Si
3p↑↑ 3s⇌ 2p⇌⇌⇌ 2s⇌ 1s⇌ [Ne] 3s²3p²
Valence electrons in Pb
4
(NH₄)₃PO₄ + Pb(NO₃)₄ → Pb₃(NO₄)₄ + NH₄NO₃
4(NH₄)₃PO₄ + 3Pb(NO₃)₄ → Pb₃(PO₄)₄ + 12NH₄NO₃
Fe + O₂ → Fe₂O₃
4Fe + 3O₂ → 2Fe₂O₃
NH₃ + O₂ → NO + H₂O
4NH₃ + 5O₂ → 4NO + 6H₂O
Na + O₂ → Na₂O
4Na + O₂ → 2Na₂O
Planck's constant
6.624x10⁻²⁴
Valence electrons in Br
7
Determine the percent yield for the reaction. 2Mg(s)+O2(g)→2MgO(s) When 10.1g Mg is allowed to react with 10.4g O2, 12.0g MgO is collected.
71.7% The percent yield is the actual yield divided by the theoretical yield times 100%. Percent yield should always be less than 100
Beer's Law equation calculation of an unknown concentration from standards and Absorbance
A solution with a concentration of 0.14M is measured to have an absorbance of 0.43. Another solution of the same chemical is measured under the same conditions and has an absorbance of 0.37. What is its concentration C1 / C2 = A1 / A2 C1 = (A1 / A2) * C2 A1 = 0.37; A2= 0.43 & C2=0.14M C1 = 0.12M
q-test
A student makes five measurement of the density of a solution and obtains the values: 1.053, 1.060, 1.059, 1.070 and 1.058 g/mL. Is 1.070 a "bad point" which should be rejected? We arrange the values in ascending order: 1.053, 1.058, 1.059, 1.060, 1.070 The total spread between the highest and the lowest value is 1.070 - 1.053 = 0.017. The spread between the questionable value and the next value is 1.070 - 1.060 = 0.010. We now define Qexp as Qexp = spread/(total spread) = 0.010/.017 = 0.60 If Qexp > Qcrit the questionable result should be rejected. In this case, the number of observations is five and Qcrit = 0.64. Since 0.60 < 0.64 the questionable result should be retained.
Charles' Law
direct relationship between volume and temperature V1/T1 = V2/T2
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al + 3Cl2 ---> 2AlCl3 How many grams of aluminum chloride could be produced from 34.0 g of aluminum and 39.0 g of chlorine gas?
Al=168.11g AlCl3 Cl=49.58g AlCl3
A student tests four solids for their ability to complete an electrical circuit when dissolved in water by observing their ability to close a circuit containing a light bulb and obtains the following results: Solid Concentration (M) Strength of light emitted A 0.20 Bright B 0.20 Dim C 0.20 None D 0.20 Bright Which of the solids is a weak electrolyte when dissolved in water?
B Molecular compounds that are weak acids or weak bases are weak electrolytes. They dissociate into component ions incompletely in water. For example, ammonia is a weak electrolyte.
BaCl₂ + H₂SO₄ → BaSO₄ + HCl
BaCl₂ + H₂SO₄ → BaSO₄ + 2HCl
B₂Br₆ + HNO₃ → B(NO₃)₃ + HBr
B₂Br₆ + 6HNO₃ → 2B(NO₃)₃ + 6HBr
C + H₂ → CH₄
C + 2H₂ → CH₄
CH₄ + O₂ → CO₂ + H₂O
CH₄ + 2O₂ → CO₂ + 2H₂O
what is the formula for the ionic compound formed by calcium ions and nitrate ions?
Ca(NO3)²
Balance the equation
Ca3(PO4)2(s)+ SiO2(s)+C(s)→CaSiO3(s)+CO(g)+P4(s)
CaCO₃ + H₂SO₄ → CaSO₄ + CO₂ + H₂O
CaCO₃ + H₂SO₄ → CaSO₄ + CO₂ + H₂O
Cl₂ + NaBr → NaCl + Br₂
Cl₂ + 2NaBr → 2NaCl + Br₂
CuCl₂ + H₂S → CuS + HCl
CuCl₂ + H₂S → CuS + 2HCl
C₃H₈ + O₂ → CO₂ + H₂O
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
p = M/V Where: p = density M = mass V = volume
D x V = M That is, M=DxV
A quantity of CO gas occupies a volume of 0.42L at 2.0atm and 329K . The pressure of the gas is lowered and its temperature is raised until its volume is 5.0L
Find the density of the CO under the new conditions. d = 0.17 gL
The binding energy of electrons in a metal is 176kJ/mol
Find the threshold frequency of the metal. ν =4.41×1014 s^−1
standard dev example Find the t-test value for the following two sets of values: 7, 2, 9, 8 and 1, 2, 3, 4?
Formula for mean: x¯ = ∑x/n s=√E(x-⁻x)²/n-1 n1=4 x⁻=6.5 x1- 7, 2, 9,8 x1-x⁻1: 0.5, -4.5, 2.5, 1.5 (x1-x⁻1)²=0.25. 20.25, 6.25, 2.25 ∑(x1−x1¯)2 = 29 S1=3.11 second set- n2=4 x⁻2=2.5 x2: 1,2, 3, 4 x2-x2: -1.5, -0.5, 0.5, 1.5 (x2-x2)²: 2.25, 0.25, 0.25, 2.25 ∑(x2−x2¯)2 = 5 S2 = 1.29 do t-test→t = 6.5−2.5/√9.667/4+1.667/4 t = 2.3764 = 2.38
A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. Sort the conditions based on the gas described. Nitrogen has the greater value
Gas for which the molecules or atoms have the greatest average velocity Gas that would have a higher rate of effusion through a small hole opened in the flask
A laser pulse with wavelength 535nm contains 4.85mJ of energy.
How many photons are in the laser pulse? N =1.31×1016
H₂SO₄ + NH₄OH → (NH₄)₂SO₄ + H₂O
H₂SO₄ + 2NH₄OH → (NH₄)₂SO₄ + 2H₂O
Rank the following elements in order of decreasing atomic radius.
I Br Cl F
Graphing data: the slope of a graph of volume vs. mass
If you pick two points on your line (x1,y1) and (x2,y2) then the slope is equal to; slope = m = D y / D x = (y2 - y1) / (x2 - x1) Volume Hg, mL Mass Hg, g 1.00 13.5 2.00 28.3 4.00 52.4 5.00 69.9 8.00 95.1 12.00 162.3
T-Test
It is called the t-test, and it is used when comparing sample means, when only the sample standard deviation is known. Define the null and alternate hyptheses, Calculate the t-statistic for the data, Compare tcalc to the tabulated t-value, for the appropriate significance level and degree of freedom. If tcalc > ttab, we reject the null hypothesis and accept the alternate hypothesis. Otherwise, we accept the null hypothesis.
Mg + HCl → MgCl₂ + H₂
Mg + 2HCl → MgCl₂ + H₂
The limiting reactant is the ĵreactant that can form the least amount of product. The given mass of Mg will form less MgO than the given mass of O2.
Mg(s)
Pauli Exclusion Principle
fill in singly before pairing px py pz
Which statements about a sample of gas containing molecules of different masses are true?
More-massive gas molecules in the sample have lower rms speed than less-massive ones The average kinetic energy depends only on the temperature. However, a heavier molecule will move more slowly than a lighter molecule if both have the same kinetic energy.
The student is now told that the four solids, in no particular order, are aluminum chloride (AlCl3), sugar (C6H12O6), acetic acid (CH3COOH), and sodium bromide (NaBr). Assuming that conductivity is correlated to the number of ions in solution, rank the four substances based on how well a 0.20 M solution in water will conduct electricity.
Most Conductive to Least conductive Aluminum chloride sodium bromide acetic acid sugar
Beer's Law Dilution of solutions
MsVs=MdVd
Lim Reag Example A 24 g sample of N2 reacts with 13 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? Write the balanced equation.
N2+3H2→2NH3 24gN2 X (1 mol/28g N2)*(2 mol NH3/1 mol N2) * (17g NH3/1 mol NH3) 13gH2* (1 mol H2/2g H2)*(2 mol NH3/3 mol H2)*(17g NH3/1mol NH3)= 73.67 29.14 NH3 is formed
SiCl₄ → Si + Cl₂
SiCl₄ → Si + 2Cl₂
Using a graph from a computer program to find the equivalence point of an acid/base titration What is the molarity of an acid titrated with a base?
So i got a lab and i found out that the molarity of NaOH is .185mol/L, now i need to find HCl's molarity. I used 25ml of diluted HCl into a flask and i titrated 46.01mL of NaOH to cause the phenothalyne to change color. How do i find the molarity of HCl? MaVa = MbVb Ma x .025L = .185mol/L x .04601L Ma x .025L = .008512mol Ma = .34mol/L
how many grams of calcium are required to react with 7.75g water to produce calcium hydroxide and hydrogen gas?
The equation is Ca(s)+ 2H2O(l)-> Ca(OH)2(s)+ H2(g) 18g=1 mole of water 7.75g of water= 7.75/18 = 0.43 moles No of moles of calcium needed= 1/2 that of water needed = 0.215 moles 1 mole of calcium =40 g 0.215 moles of calcium= 40x0.215 = 8.6g
It is important to realize that not all molecules in a sample will have the same kinetic energy
The speed of a particle with average kinetic energy is called the root mean square (rms) speed, vrms.
The Kinetic Molecular Theory of Gases
To understand how gas molecules behave in terms of motion, speed, and energy. relationship between temperature and the average speed Increasing the temperature of a gas sample increases the average kinetic energy (speed) of the molecules.
Combined Gas Formula
a law combines Lussac's, Charles's, and Boyles's Law, indirect P1V1/T1=P2V2/T2
Elements with 5 or more valence electrons tend to
gain electrons
Both gases have the same value
gas for which the molecules or atoms have the greatest average kinetic energy Gas that exerts the greater partial pressure
Elements with 3 or fewer valence electrons tend to
lose
3 moles Al/2 moles CCuCl2
molar ratio of balanced equation
Give a combination of four quantum numbers that could be assigned to an electron occupying a 5p orbital.
n, l, ml, ms = 5,1,0,0.5
Which of the following statements are true?
*There are gas molecules that move slower than the average *The average kinetic energy of gas molecules decreases with decreasing temperature. *All the gas molecules in a sample cannot have the same kinetic energy. *The average speed of gas molecules decreases with decreasing temperature
he shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?
+3 and +6
What are the possible values of mℓ for an electron in a d orbital?
-2,-1,0,1,2 Since the allowed values for mℓ range from −ℓ to +ℓ, once you know the value for ℓ you know the values for mℓ.
C₂H₆ + O₂ → CO₂ + H₂O
2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O
Fe + H₂SO₄ → Fe₂(SO₄)₃ + H₂
2Fe + 3H₂SO₄ → Fe₂(SO₄)₃ + 3H₂
HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
HCl + Na₂CO₃ → NaCl + H₂O + CO₂
2HCl + Na₂CO₃ → 2NaCl + H₂O + CO₂
HgO + Cl₂ → HgCl + O₂
2HgO + Cl₂ → 2HgCl + O₂
HgO → Hg + O₂
2HgO → 2Hg + O₂
H₂ + O₂ → H₂O
2H₂ + O₂ → 2H₂O
H₂O₂ → H₂O + O₂
2H₂O₂ → 2H₂O + O₂
KClO₃ → KCl + O₂
2KClO₃ → 2KCl + 3O₂
KNO₃ + H₂CO₃ → K₂CO₃ + HNO₃
2KNO₃ + H₂CO₃ → K₂CO₃ + 2HNO₃
NH₃ + H₂SO₄ → (NH₄)₂ + SO₄
2NH₃ + H₂SO₄ → (NH₄)₂ + SO₄
Na + H₂O → NaOH + H₂
2Na + 2H₂O → 2NaOH + H₂
Na + Br₂ → NaBr
2Na + Br₂ → 2NaBr
NaCl + F₂ → NaF + Cl₂
2NaCl + F₂ → 2NaF + Cl₂
NaClO₃ → NaCl + O₂
2NaClO₃ → 2NaCl + 3O₂
NaOH + H₂SO₄ → Na₂SO₄ + H₂O
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O
O
2p⇌ ↑ ↑ 2s⇌ 1s⇌ [He] 2s² 2p⁴
Ne
2p⇌⇌⇌ 2s⇌ 1s⇌ [He] 2s²2p⁶
Valence electrons in Al
3
P + O₂ → P₄O₁₀
4P + 5O₂ → P₄O₁₀
According to the quantum-mechanical model for the hydrogen atom, which of the following transitions would produce light with the longer wavelength: 3p→2s or 4p→3p?
4p→3p
Valance in N
5
Which of the following set of quantum numbers (ordered n, ℓ, mℓ, ms) are possible for an electron in an atom?
5, 3, -3, 1/2 5, 3, 0, 1/2 3, 2, 2, -1/2
How many grams of glucose and of water are in 500 g of a 5.3% by-mass glucose solution
5.3g/100gx 500g solution=26.5g 500g-26.5g=436.5g water
Ag₂S → Ag + S₈
8Ag₂S → 16Ag + S₈
λ Z/s⁻¹
=C 3x 10² m/s
Solid Concentration (M) Strength of light emitted A 0.20 Bright B 0.20 Dim C 0.20 None D 0.20 Bright The student is told that one of the four solids tested is actually aluminum chloride,AlCl3. Which of the solids could be AlCl3?
A and D All ionic substances and strong acids are strong electrolytes.
A 0.22-caliber handgun fires a 29-g bullet at a velocity of 775 m/s.
Calculate the de Broglie wavelength of the bullet. λ = 2.9×10−35m Is the wave nature of matter significant for bullets?-NO Although quantum mechanics applies to all objects, most everyday objects are too large to exhibit any noticeable wavecharacteristics.
The constant motion of gas molecules causes diffusion and effusion.
Diffusion is the gradual mixing of two substances resulting from the movement of their particles. Effusion is the gradual escape of gas molecules through microscopic holes in their container.
To what volume should you dilute 25mL of a 11M H2SO4 solution to obtain a 0.17M H2SO4 solution?
Dilutions are a core technique for any chemist, and the following equation, which is represented in two different ways, can be used to relate the molarity and volume of the original solution to the molarity and volume of the diluted solution: V=1.6L M1V1=M2V2 MconcVconc=MdilVdil In the second representation of the equation, "conc" and "dil" represent "concentrated" and "diluted."
Delta E=
E2-E1=hZ=hc/λ
Diffusion
Hairspray in the bedroom can be smelled in the hallway
Consider the following precipitation reaction: 2Na3PO4(aq)+3CuCl2(aq)→ Cu3(PO4)2(s)+6NaCl(aq)
What volume of 0.183M Na3PO4 solution is necessary to completely react with 93.7mL of 0.117M CuCl2? V =39.9 mL
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s)
What volume of O2 gas (in L), measured at 765mmHg and 19∘C, is required to completely react with 50.0g of Al? V = 33.1L
Effusion
When a hole is made in the top of a coke bottle dioxide gas moves out of the bottle over time OR a leak in a gas cylinder causes the volume to decrease
conducts electricity
NaCl solution
NaOH + HNO₃ → NaNO₃ + H₂O
NaOH + HNO₃ → NaNO₃ + H₂O
Predict products from an acid/base reaction
Neutralization is the reaction of hydronium ions (H3O) and hydroxide ions (OH) to produce water molecules. Example: H3O + OH -> 2H2O In case of polyprotic acids (acids that can donate more than none proton per molecule) like H3PO4 see this example: H3PO4 + H2O-> <- H3O + H2PO4 H2PO4 + H2O -><- H3O + HPO4 HPO4 + H2O-> <- H3O + PO4
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains 0.248mol FeS and 0.646mol HCl.
Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left? n = 0.150 mol
The allowed values for mℓ range from −ℓ to +ℓ and the allowed values for ℓ are integers between zero and n−1.
Once you know the value for n, you can determine the acceptable ℓ values, and from there the acceptable mℓ values. The ms values are fixed at either 1/2 or −1/2.
Here is a more complex redox reaction involving the dichromate ion in acidic solution: 3S2− + 14H+ + Cr2O72− → 3S +2Cr3+ + 7H2O Classify each reactant as the reducing agent, oxidizing agent, or neither.
Oxidizing agent: Cr2O7^2- Reducing agent:S2- Neither:H+
For the given reactions, classify the reactants as the reducing agent, oxidizing agent, or neither. 3O2 + 4Fe → 2Fe2O3 H2 + Br2 → 2HBr
Oxidizing agents- O2 and Br2 Reducing agents- H2 and Fe
Rank the following elements in order of largest to smallest
P S Cl Ar
Calculate the amount of solute in a percent solution
Percent by mass =mass of solute mass of solution X100%
P₄ + O₂ → P₄O₁₀
P₄ + 5O₂ → P₄O₁₀
S₈ + O₂ → SO₃
S₈ + 12O₂ → 8SO₃
Determine the theoretical yield for the reaction. 2Mg(s)+O2(g)→2MgO(s) When 10.1g Mg is allowed to react with 10.4g O2, 12.0g MgO is collected.
The theoretical yield is determined from the limiting reactant. The mass of Mg must be converted to moles of Mg to moles of MgO to grams of MgO. m = 16.7g
Compare the volume of 22.1g of helium to 22.1g of argon gas (under identical conditions). term-0
The volume would be greater for helium gas. Helium has a lower atomic mass than argon. The same mass of helium gas would contain a greater number of moles and have a larger volume.
Find the volume of 0.100M hydrochloric acid necessary to react completely with 1.53g Al(OH)3
V = 0.588L
A weather balloon is inflated to a volume of 29.7L at a pressure of 735mmHg and a temperature of 25.9∘C. The balloon rises in the atmosphere to an altitude where the pressure is 375mmHg and the temperature is -14.6∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude
V balloon =50.3L The number of moles in the weather balloon will remain constant. According to the ideal gas law, the changes in pressure and temperature will cause a change in volume. Volume and pressure are inversely related, while volume and temperature are directly related
What is the volume occupied by 22.1g of argon gas at a pressure of 1.38atm and a temperature of 308K ?
V=10.1 L The ideal gas law is used to determine the volume of argon gas. The mass should first be converted to moles by dividing by the atomic mass.
Calculate the concentration of an acid (or base) from experimental data
Veq=Vb= MaVa/ Mb= (0.100 M)(50.0 mL) 0.200 M =25.0 mL
A 1.00 L flask is filled with 1.20g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.350atm .
What is the partial pressure of argon, PAr, in the flask? PAr = 0.735 atm Before ethane was added, the percent by volume of argon in the flask was 100% and the partial pressure of argon was equivalent to the total pressure of the flask. The total volume of the flask, the temperature of the flask, and the amount of argon remain constant after ethane was added; therefore the partial pressure of argon is the same before and after ethane was added. The total pressure of the flask is now equal to the combined partial pressures of both argon and ethane.
A 1.00 L flask is filled with 1.20g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.350atm .
What is the partial pressure of ethane, Pethane, in the flask? Pethane = 0.615 atm Dalton's law of partial pressures states that the total pressure of a system is equal to the sum of the partial pressures of the component gases in the mixture. The expression for Dalton's law of partial pressure is Ptotal=PA+PB+... The partial pressure of an individual gas can be used in stoichiometric calculations involving chemical reactions.
An electron has an uncertainty in its position of 499pm
What is the uncertainty in its velocity? Δv =1.16×105 ms
An electron in a hydrogen atom relaxes to the n=4 level, emitting light of 114 THz.
What is the value of n for the level in which the electron originated? n =6
A 9.00mL ampule of a 0.140M solution of naphthalene in hexane is excited with a flash of light. The naphthalene emits 19.0J of energy at an average wavelength of 349 nm
What percentage of the naphthalene molecules emitted a photon? percentage =4.40 %
isoelectronic
atoms have the same number of electrons ex. O²⁻ and Na⁺=10e
Boyle's law
indirect relationship between pressure and volume P1 x V1 = P2 x V2
The magnetic quantum number mℓ
corresponds to the orbital in which the electron is located. Instead of 2px, 2py, and 2pz, the three 2p orbitals can be labeled −1, 0, and 1, but not necessarily respectively. As a rule, mℓ can have integer values ranging from −ℓ to +ℓ
The principal quantum number n
corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an electron in the 2p subshell has a principal quantum number of n=2 because 2p is in the second shell.
spin quantum number ms
corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas −1/2 means a "down" spin.
azimuthal or angular momentum quantum number ℓ
corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, d as 2, and f as 3. For example, an electron in the 2p subshell has ℓ=1. As a rule, ℓ can have integer values ranging from 0 to n−1.
2Al(s)+3CuCl2(aq)→3Cu(s)+2AlCl3(aq)
g→m= .51gCuCl2 Cu63.54 + Cl 70 .51.133.5=0.004M
Avogadro's Law
he direct relationship between the # of moles and volume V1/n1= V2/n2
One mole of nitrogen and one mole of neon are combined in a closed container at STP.
how big is the container? V = 44.8L
Volume is
inversely proportional to pressure Directly proportional to temperature and # of mols
How many mL of a base is needed to neutralize an acid?
molarity of an acetic acid solution if 34.57 mL of this solution are needed to neutralize 25.19 mL of 0.1025 M sodium hydroxide CH3COOH (aq) + NaOH (aq) -----> Na+(aq) + CH3COOH-(aq) + H2O (l) (25.19 mL) (1 L/ 1000 mL) = 0.02519 L (0.02519 L) (0.1025 mol / L) = 0.002582 mol NaOH →change to acetic acid 34.57ml X 1L/1000ml= 0.03457L 0.002582mol/0.03457L=0.07469M acetic acid
Do the same for an electron occupying a 6d orbital.
n, l, ml, ms = 6,2,-2,-0.5
Diamagnetic substances contain
no net electron spin and are repelled from a magnetic field
Paramagnetic substances contain
one or more unpaired electrons and are attracted to a magnetic field
What/how does acid-base indicator phenolphthalein show?
phenolthalein is a weak acid. When you add a solution of HPh to an acidic solution, the acid HPh does not ionise. Because the HPh molecule is colourless, the acidic solution is colourless. If yo now add a solution of a base (as in a titration) when all the acid has been neutralise, the HPh is able to dissociate and turn pink
Formula for Standard Deviation
s=√E(x-⁻x)²/n-1 x = Values given x¯ = Mean n = Total number of values
T-test sample calc
t-obt=x1-x2√s1²/n1+s2²=n2 t-obt= obtained t x1 and x2= means of the two groups s1 and s2 = variances n1 and n2= number of participants in each group
Which elements do you expect to lose electrons in their chemical reactions? Which do you expect to gain electrons?
tend to lose electrons- Al and Pb tend to gain electrons- Br and N
Gay-Lussac's Law
the direct relationship between pressure and temperature P1/T1 = P2/T2
Ideal Gas Law V'N
the ideal law with all factors at STP, including # of moles (v1/v2)=(n1/n2) or PV=nRT
Valence electrons are
the total number of electrons in the outermost shell. Knowing how many valence electrons are in elements is helpful in deciding whether elements will lose or gain electrons in a reaction. In this case, Al contains 3 valence electrons
The frequency of a light emission is proportional
to the energy difference between two levels. Therefore, the frequency of the light would be greater
The rms speed may be expressed by the following equation:
vrms=√3RT/M R= ideal gas constant T=absolute temperature M=molar mass of the substance in kilograms per mole.
Before using the de Broglie relation
λ = h/mv, the mass of the bullet needed to be converted to kilograms using the conversion factor 1000 g = 1 kg. Since the units for Planck's constant are kg⋅m2/s, this will allow the mass of the bullet to properly cancel during the calculation.
