Concept explainers
(a)
Interpretation:
The large sized ion or atom from the given atoms or ion has to be identified.
Concept introduction:
In periodic table, down the column there is increase in atomic radii due to accumulation of electrons in outermost shell orbitals and decreases across group from left to right due to increase in effective nuclear charge across group.
(b)
Interpretation:
The large sized ion or atom from the given atoms or ions has to be identified.
Concept introduction:
In periodic table, down the column there is increase in atomic radii due to accumulation of electrons in outermost shell orbitals and decreases across group from left to right due to increase in effective nuclear charge across group.
(c)
Interpretation:
The large sized ion or atom from the given atoms or ions has to be identified.
Concept introduction:
In periodic table, down the column there is increase in atomic radii due to accumulation of electrons in outermost shell orbitals and decreases across group from left to right due to increase in effective nuclear charge across group.
(d)
Interpretation:
The large sized ion or atom from the given atoms or ions has to be identified.
Concept introduction:
In periodic table, down the column there is increase in atomic radii due to accumulation of electrons in outermost shell orbitals and decreases across group from left to right due to increase in effective nuclear charge across group.
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General Chemistry: Atoms First
- Identify the species with the larger radius in each of the following pairs. (a) O Ga3+ O Ca2+ (b) O S (c) O Mg2+ O Al3+ (d) O Mg O Naarrow_forward11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).arrow_forwardProvide a brief explanation for each of the following: (a) O2-is larger than O. (b) S2- is larger than O2-. (c) S2- is largerthan K+. (d) K+ is larger than Ca2+.arrow_forward
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- Write the electron configuration for each of the followingions, and determine which ones possess noble-gasconfigurations: (a) Sr2+, (b) Ti2+, (c) Se2-, (d) Ni2+, (e) Br-,(f) Mn3 + .arrow_forwardFor each of the following sets of atoms and ions, arrange the members in order of increasing size. (a) Oa- O s- Ar O An O Ar O s2- (b) O s2- O 02- O Se2- O Se?- O Se?- O s- O 02- O s- O 02- (c) O Mg O Na+ O Na O Nat O Lit O Lit O Lit O Mg O Mg (d) O Na+ O Na+ O Mg?+ OF OF OF O Mg2+ O Mg2+ O Natarrow_forward(D) Zr (Z=40) and Hf (Z = 72) 7. Which halogen has the greatest first ionization energy? (A) F (B) Cl (C) Br (D) I 3. The isotope "Zn undergoes what mode of radioactive decay? (A) Alpha emission (C) Gamma emission (B) Beta emission (D) Positron emission 9. What is the bond order of carbon monoxide, CO? (A) 1.5 (B) 2.0 (C) 2.5 (D) 3.0 50. Which statements about the Lewis structure of thearrow_forward
- 7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°arrow_forwardWhich element in each of the following sets would you expect to have the lowest third ionization energy, IE3? (a) O Na O Al O Mg (b) O Ga ок O Mg (c) O Ca O Sc OK оооarrow_forward4. Write an appropriate set of four quantum numbers (n, l, ml & ms) that could be representative of a valence electron in each of the following atoms or ions. (a) Bi (m (b) Sr (c) Mo (d) Ru2+ (e) Euarrow_forward
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