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General Chemistry Fundamentals
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General Chemistry Fundamentals
General Chemistry Fundamentals
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1
Question
What does Dalton’s Law of Partial Pressure state about gas mixtures?
Page 1
Answer
The total pressure exerted by a mixture of gases equals the sum of the partial pressures of the individual gases.
2
Question
What is the formula for total pressure in a gas mixture according to Dalton’s Law?
Page 1
Answer
\(P_{total} = P_1 + P_2 + P_3 + \dots + P_n\)
3
Question
How is the partial pressure of an individual gas calculated using the ideal gas law?
Page 1
Answer
\(P = \frac{nRT}{V}\), where n is moles, R is gas constant, T is temperature in Kelvin, and V is volume.
4
Question
In the example with 56 g N₂ and 96 g O₂ in a 2 L container at 300 K, what is the partial pressure of N₂?
Page 1
Answer
24.62 atm, calculated as \((2 \ mol)(0.08206 \ L\cdot atm/mol\cdot K)(300 \ K) / 2 \ L\).
5
Question
In the N₂ and O₂ mixture example at 300 K in 2 L, what is the partial pressure of O₂ and total pressure?
Page 1
Answer
O₂ partial pressure is 36.93 atm; total pressure is 61.55 atm.
6
Question
What is the formula for the mole fraction of a gas in a mixture?
Page 1
Answer
\(x_a = \frac{n_A}{n_T}\), where \(n_A\) is moles of gas A and \(n_T\) is total moles.
7
Question
In a gas mixture with 3 moles O₂ and 2 moles N₂, what are the mole fractions?
Page 2
Answer
O₂ mole fraction is 0.60; N₂ mole fraction is 0.40.
8
Question
What are quantum numbers described as in atomic theory?
Page 2
Answer
They are the address of an electron, explaining the size, shape, and orientation of orbitals.
9
Question
Name the four quantum numbers that describe an electron in an atom.
Page 2
Answer
Principal (n), azimuthal/angular momentum (l), magnetic (m_l or m), and spin (s).
10
Question
What does the principal quantum number n describe about an orbital?
Page 2
Answer
It describes the size of the orbital, energy of the electron, shell, and average distance from nucleus.
11
Question
What are the possible values for the principal quantum number n?
Page 2
Answer
Positive integers: 1, 2, 3, 4, etc.; n cannot be 0.
12
Question
What does n=1, n=2, and n=3 correspond to in terms of electron shells?
Page 2
Answer
n=1 is K shell, n=2 is L shell, n=3 is M shell.
13
Question
What properties does the azimuthal quantum number l describe?
Page 2
Answer
It describes the shape of the orbital, subshell, and orbital angular momentum.
14
Question
What are the possible values of the azimuthal quantum number l for a given n?
Page 2
Answer
l = 0, 1, 2, …, (n − 1).
15
Question
What orbital types do l=0, l=1, l=2, and l=3 represent?
Page 2
Answer
l=0 is s orbital, l=1 is p orbital, l=2 is d orbital, l=3 is f orbital.
16
Question
What does the magnetic quantum number m_l specify, and what are its values for a given l?
Page 2
Answer
It gives the orientation of orbitals in space; values from −l to 0 to +l (2l + 1 possibilities).
17
Question
How many orbitals are in s, p, and d subshells based on m_l?
Page 3
Answer
s (l=0): 1 orbital; p (l=1): 3 orbitals; d (l=2): 5 orbitals.
18
Question
What does the spin quantum number s indicate, and what are its possible values?
Page 3
Answer
It gives the direction of electron spin; values are +½ (clockwise) or −½ (anticlockwise).
19
Question
What is the total number of subshells in an orbit, orbitals in an orbit, and maximum electrons in an orbit?
Page 3
Answer
Subshells = n; orbitals = n²; maximum electrons = 2n².
20
Question
What is the total number of orbitals and electrons in a subshell given l?
Page 3
Answer
Orbitals = 2l + 1; electrons = 2(2l + 1) = 4l + 2.
21
Question
What is electronic configuration defined as for an atom?
Page 3
Answer
It is the map or address system describing how electrons are distributed among shells and orbitals.
22
Question
What is the electron configuration of phosphorus?
Page 3
Answer
\(1s^2 2s^2 2p^6 3s^2 3p^3\)
23
Question
How many orbitals are in s, p, d, and f sublevels, and maximum electrons each?
Page 4
Answer
s: 1 orbital (2 e⁻); p: 3 orbitals (6 e⁻); d: 5 orbitals (10 e⁻); f: 7 orbitals (14 e⁻).
24
Question
How is electron configuration notation structured?
Page 4
Answer
Number for principal shell, letter for subshell (s,p,d,f), superscript for number of electrons.
25
Question
What are the three rules governing electron configurations?
Page 4
Answer
Aufbau Principle, Pauli Exclusion Principle, Hund’s Rule.
26
Question
What does the Aufbau Principle state about filling orbitals?
Page 4
Answer
Electrons fill from lowest energy orbital first, proceeding to higher levels.
27
Question
What is the Aufbau filling order for orbitals up to 7p?
Page 4
Answer
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p.
28
Question
What does Pauli Exclusion Principle state about electrons in an orbital?
Page 5
Answer
No more than 2 electrons per orbital; they must have opposite spins and unique quantum numbers.
29
Question
What does Hund’s Rule require for degenerate orbitals?
Page 5
Answer
Fill each halfway first (single electrons with parallel spins), then pair up.
30
Question
What are the electron configurations for the first 10 elements?
Page 5
Answer
H: 1s¹; He: 1s²; Li: 1s²2s¹; Be: 1s²2s²; B: 1s²2s²2p¹; C: 1s²2s²2p²; N: 1s²2s²2p³; O: 1s²2s²2p⁴; F: 1s²2s²2p⁵; Ne: 1s²2s²2p⁶.