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(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
Bundle: Chemistry for Today: General, Organic, and Biochemistry, Loose-Leaf Version, 9th + LMS Integrated OWLv2, 4 terms (24 months) Printed Access Card
- 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_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_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_forward
- The Group on the Periodic Table that BEST demonstrates the concept that elements in the same Group are NOT required to have the same chemical properties is Group a. I A (1) b. IV A (14) c. VII A (17) d. VIII A (18)arrow_forwardSelect the element in each pair with the higher ionization energy.a. Br or I b. Mg or Src. Si or P d. I or Xearrow_forwardWhich statement is an example of the Pauli Exclusion Principle? a. Atoms with a full octet shell have more stability. b. When filling orbitals with the same energy levels, electrons fill them singly first, and then form pairs when every orbital has a single electron. c. Two electrons in an orbital must have opposite spins d. Electrons must fill the lowest energy levels firstarrow_forward
- Give the correct abbreviated electron configuration for each of the following atoms or ions: a. Ge b. W c. Bi d. Co3+ e. Br-arrow_forwardOrder 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_forwardWhat 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_forward
- 1. 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_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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