(a)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(b)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(c)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(d)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
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Chapter 3 Solutions
Chemistry for Today: General, Organic, and Biochemistry
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- Order the elements S, Cl, and F in terms of increasing ionization energy. a. F, S, Cl b. S, F, Cl c. S, Cl, F d. F, Cl, S e. Cl, F, Sarrow_forward5. What elements make up 99% of muscle in living organisms? * A. Carbon, Sulfur, Oxygen, and Hydrogen B. Carbon, Nitrogen, Phosphorus, and Hydrogen C. Carbon, Nitrogen, Oxygen, Nitrogen, and some Sulfur D. Carbon, Nitrogen, Sulfur, Hydrogen and some Magnesiumarrow_forward1. Give the electron configuration for the valence electron of each of the following. a. I b. О C. As d. Ca e. Sn f. S g. Al h. Br į. P j. Pbarrow_forward
- What is the Pauli Exclusion Principle? * a. An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins b. An atomic orbital can hold a minimum of 6 electrons, each with opposite spins c. An atomic orbital can hold a maximum of 6 electrons, each with the same spin d. An atomic orbital can hold a minimum of 2 electrons, each with opposite spinsarrow_forwardWhich of the following elements has 7 valence electrons? Select one: a. C b. Br c. N d. S e. Bearrow_forwardPotassium has an atomic number of 19. What is its electron configuration? a. Shells 1, 2, and 3 are full and shell 4 has three electrons. b. Shells 1, 2, and 3 are full, and shell 4 has one electron. c. Shells 1 and 2 are full, and shell 3 has nine electrons.arrow_forward
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