(a)
Interpretation:
The Roman numeral periodic – table group number and valence electrons of
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- The valence electrons decide the manner in which an atom form a bond with another atom.
- The valence electron in an atom decides the combining capacity of the element.
- Except inner
transition elements valence electrons are present in s or psubshells of elements. - For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
(b)
Interpretation:
The Roman numeral periodic – table group number and valence electrons of
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- The valence electrons decide the manner in which an atom form a bond with another atom.
- The valence electron in an atom decides the combining capacity of the element.
- Except inner transition elements valence electrons are present in s or psubshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
(c)
Interpretation:
The Roman numeral periodic – table group number and valence electrons of
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- The valence electrons decide the manner in which an atom form a bond with another atom.
- The valence electron in an atom decides the combining capacity of the element.
- Except inner transition elements valence electrons are present in s or psubshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
(d)
Interpretation:
The Roman numeral periodic – table group number and valence electrons of
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- The valence electrons decide the manner in which an atom form a bond with another atom.
- The valence electron in an atom decides the combining capacity of the element.
- Except inner transition elements valence electrons are present in s or psubshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 4 Solutions
General, Organic, and Biological Chemistry
- How many valence electrons are needed to complete the outer valence shell of sulfur? a. 1 b. 2 c. 3 d. 4arrow_forwardThe noble metals gold, silver, and platinum are often used in fashioning jewelry because they are relatively .arrow_forwardFirst you need to find the number of valence electrons in NH2Cl. For counting purposes with Lewis structures, the number of valence electrons in an atom of a main group element is equal to the last digit in the group number of that element in the Periodic Table. N is in Group ________ H is in Group ________ Cl is in Group _________ In NH2Cl there is a total of ____________ valence electrons.arrow_forward
- The molecules NH3andBF3have the same general formula (AB3)but different shapes. Find the shape of each of the above molecules. Provide more examples of real molecules that have the same general formulas but different shapes.arrow_forwardIn forming an ionic bond with an atom of chlorine, a sodium atom will: a.receive one electron from the chlorine atom. b.receive two electrons from the chlorine atom. c.give up one electron to the chlorine atom. d.give up two electrons to the chlorine atom.arrow_forwardWhich simple ion would each of the following elements be expected to form? Which noble gas has an analogous electron configuration to each of the ions? msp;a.bromine,Z=35b.cesium,Z=55c.phosphorus,Z=15d.sulfur,Z=16arrow_forward
- Describe the general structure of an atom.arrow_forwardFor each element determine the charge of the ion that will most likely form based on the data? What do you look for? Why does this happen? Based on the data, locate the family/column number for each element on the periodic table.arrow_forwardd. The energy required to separate the ions in the calcium carbonate crystal lattice into individual calcium and carbonate ions as represented in the table below is known as the lattice energy. As shown in the table, the lattice energy of magnesium carbonate is more than the lattice energy of calcium carbonate. Explain why in terms of periodic properties and Coulomb's law.arrow_forward
- A1. Determine the number of core and valence electrons present in iodine.arrow_forwardPredict the common ionic charge for Group VIIA/17 elements; Group VIA/16 elements; Group VA/15 elements.arrow_forwardBe sure to answer all parts. Give the number of valence electrons in cobalt. Write out the electronic configuration for the valence electrons. Valence electrons: Electronic configuration for the valence electrons:arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks Cole
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning