(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
- Using data from Chapter 2, calculate the change in energy expected for each of the following processes. a. Na(g)+Cl(g)Na+(g)+Cl(g) b. Mg(g)+F(g)Mg+(g)+F(g) c. Mg+(g)+F(g)Mg2+(g)+F(g). d. Mg(g)+2F(g)Mg2+(g)+2F(g)arrow_forwardUse trends within the periodic table and indicate which member of each of the following pairs gives up one electron more easily: a.Li or K b.C or Sn c.Mg or S d.Li or Narrow_forwardDescribe electron spin. How does electron spin affect the total number of electrons that can be accommodated in a given orbital? What does the Pauli exclusion principle tell us about electrons and their spins?arrow_forward
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- 5. 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_forwardWhich of the following elements has 7 valence electrons? Select one: a. C b. Br c. N d. S e. Bearrow_forward4. Consider this chemical equation: Br + e > Br + energy Which concept does this chemical equation correspond with? A. atomic radius B. ionization energy C. electron affinity D. electronegativity E, metal reactivityarrow_forward
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