Chapter 1.
1.1
(a) Nodal surface(마디 표면); A surface on which the probability of finding an electron is zero.
(p. 5)
전자가 발견될 확률이 0 인 평면
(b) Pauli exclusion principle(배타 원리); No two electrons in an atom may possess identical sets
(p. 8)
of the four quantum numbers.(한 원자에서 두 전자가 동일한 4개의 양자수 세트를 가질 수 없다)
(c) Paramagnertic(상자기성); Atoms containing one or more unpaired electrons are attracted by
(p. 15)
magnetic field.(한 개 이상의 홑전자를 포함하는 원자는 자기장에 끌림)
1.2
(a) Orbitals(오비탈); A region of space around the nucleus in which there is some arbitrary
high probability of finding an electron.(핵 주위에서 전자가 높은 확률로 발견될 수 있는 공간)
(b) Degenerate(축퇴); Two or more orbitals have same energy (p.9)
(c) Hund's rule; When filling a set of degenerate orbitals, the number of unpaired electrons
will be maximized and these electrons will have parallel spins. (p.9)(축퇴된 일련의 오비탈이
채워질 때, 홑전자 수는 최대가 되고 전자들은 같은 방향의 스핀을 가지게 된다)
1.3
n
4
l
0
ml
0
(4s)
1
-1
0
+1
(4p)
2
-2
-1
3
0
+1
(4d)
+2
-3
-2
1.4
n
l
ml
quantum number(양자수)
principal quantum number
(주 양자수)
angular momentum quantum number
(각운동량 양자수)
magnetic quantum number
(자기 양자수)
(+l ) = 4
value(값)
1 ~ ∞ positive integer
0 ~ (n-1) integer
(+l ) ~0~ (-l ) integer
→ n-1 = 4 → ∴ n(주양자수) = 5
1.9
p. 9; Fig. 1.12 와 text 참고 (가장 낮은 에너지 상태)
1.12
(a) Ca; [Ar] 4s2
(b) Cr; [Ar] 4s13d5
(c) Pb;[Xe] 6s24f145d106p2
-1
0 +1 +2 +3
(4f)
1.14
(a) Cl-; [Ar]
(b) Co2+; [Ar] 3d7
(c) Mn4+;[Ar] 3d3
1.15
Thallium(Tl); [Xe]6s2 4f14 5d10 6p1
Tl+; [Xe]6s2 4f14 5d10
∴
Tl3+; [Xe]4f14 5d10
1.17
Silver(Ag); [Kr]5s1 4d10
∴
Ag+; [Kr] 4d10
1.22
N;
[He]
↿⇂
2s
↿
↿
2p
Si;
[Ne] ↿⇂
3s
↿
↿
3p
↿⇂
↿
Fe; [Ar] ↿⇂
4s
↿
↿
3d
1.23
Element 113 ; Group 13 ( cf. Tl )
[Rn] 7s2 5f14 6d10 7p1
1+ ion; [Rn] 7s2 5f14 6d10
3+ ion; [Rn] 5f14 6d10
↿
↿
Chapter 2
2.1
(a)Rare earth metals; Group 3 elements (Sc, Y, and La) and the lanthanoid elements (La~ Lu)
(p. 22)
(b) van der Waals radius; half-distance between the nuclei of two atoms of neighboring
molecules (= two atoms in contact with each other but not bonded to each other)
(c)
Effective
nuclear
charge;
net
positive
charge
experienced
by
an
electron
in
a
multi-electron atom
2.4
Co(atomic number;27); only one common isotope having 32 neutrons
Ni(atomic number;28); two common isotopes having 30 and 32 neutrons
2.6
주화금속(coinage metal); Cu(copper), Ag(silver), Au(gold) are easily extracted from their ores
and have been known for thousands of years. They are resistant to corrosion and therefore
useful in coinage where a long circulation life is desirable.
2.11
(a) Pb
(b) Tc
(c) Hg
2.13
Sodium (Na); odd number of protons (Z = 11),
Magnesium (Mg); even number of protons (Z = 12)
∴ Na is likely to have fewer stable isotopes than Mg.
2.17
(a) Some non-metals and metal compounds have metallic lusters(금속 광택).
(b) Diamond has the highest thermal conductivity.
(c) Some non-metal, for example graphite, has a good electrical conductivity in two
dimensions.
2.19
Potassium(K) has the larger covalent radius than calcium(Ca) because the effective nuclear
charge (Zeff) on the outermost electrons increases as you move from left to right across a
period. As Zeff increases, the outermost electrons are more attracted to the positively charged
nucleus, so the covalent radius decreases.
2.22
Covalent radius;
Zr ([Kr] 5s2 4d2) > Hf([Xe] 4f14 5d2 6s2)
∵ The 4f electrons in Hf do not shield outer orbital very well.
2.24
K: (1s2) (2s2 2p6) (3s2 3p6) (4s1)
▷ 1s: σ =
1(0.35) = 0.35
e- in 1s
Zeff = 19 - 0.35 = 18.65
▷ 2s, 2p: σ =
7(0.35) +
2(0.85) = 4.15
e- in 2s,2p e- in 1s
Zeff = 19 - 4.15 = 14.85
▷ 3s, 3p: σ =
7(0.35) +
8(0.85) +
2(1.00) =
e- in 3s,3p e- in 2s,2p e- in 1s
11.25
Zeff = 19 - 11.25 = 7.75
▷ 4s: σ =
8(0.85) +
e- in 3s,3p
10(1.00) =
16.80
e- in 1s,2s,2p
Zeff = 19 - 16.80 = 2.20
2.27
Phosphorus (3s2 3p3) has a higher first ionization energy than silicon (3s2 3p2) because Zeff
increases left to right across a period.
2.31
Na [1s2 2s2 2p6 3s1], Mg [1s2 2s2 2p6 3s2]
▷ First ionization energy ; Na < Mg
∵ The 3s electrons in Mg experience higher effective nuclear charge.
▷ Second ionization energy ; Na > Mg
∵The second electron removed from Na is a core electron, while that from Mg is the
valence electrons. Removal of a core electron requires a much larger energy.
▷ Third ionization energy ; Na < Mg
∵The third electron removed from both Na and Mg is a 2p electron. The 2p electrons in
Mg experience higher effective nuclear charge.
2.36
Pb; [Xe] 4f14 5d10 6s2 6p2
Sn; [Kr] 4d10 5s2 5p2
The effective nuclear charge on the outer electrons(6s & 6p) of Pb > effective nuclear charge
on the outer electrons(5s & 5p) of Sn
(∵shielding effect by 4f electrons of Pb is low.)