6-10 1105-Sec2, Periodic Table, Problem supplementTrue-False (A=True, B=False)1. Atomic size decreases as you go down a vertical column.2. Ionization energy is the energy necessary to remove valence electrons from atoms.3. Increasing ionization energy means that generally less energy is required to remove anelectron from the elements going across a row, and it takes progressively more energy toremove an electron when going down a column.4. An atom that gives up an electron easily is more likely to take on another electron.5. Atoms with high ionization energy will be able to hold another electron more easily.6. Lower ionization energy indicates less attraction for additional electrons, and greaterionization energy indicates greater desire for electrons.7. Nonmetals like oxygen have the greatest chance to lo3e electrons.8. Inert gases have very little desire to gain or to lose electrons.9. A bond will result when one atom attracts the electrons of another atom.10. An ionic bond forms when one atom completely removes a valence electron from anotheratom.11. An ionic bond is any bond that is made from ions.12. Ionic bonds are the least common bonds in the minerals of the earth.13. Almost all inorganic substances are ionic in nature.14. Atoms with similar electronegativities form covalent bonds.15. The amount of ionic and covalent character is determined by the difference in theelectronegativities of the atoms making up the compound.16. An electron is completely taken away from another atom in a covalent bond.17. All metals are liquid at room temperature except mercury.18. Metallic bonds are directed bonds, but ionic and covalent bonds have bonding electrons thatroam.19. If the difference between the electronegativity of two elements is less than 1.7, the percentionic character of the bond is less than 51% percent so the bond is covalent. (Think andcheck the periodic table)

Ionization energy measure the amount of energy required to remove outermost electron.

Answered: Lower ionization energy indicates less…

Lower ionization energy indicates less attraction for additional electrons, and greater onization energy indicates greater desire for electrons.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Electron Affinity

When an element undergoes a chemical reaction, it either gains energy or loses energy. This gain or loss of energy is due to the phenomena that occur at atomic level. During reaction, atoms either gain electrons from other atoms or lose electrons to other atoms, and in that process, energy is produced.

P-Block Elements

Elements which are present on the right side of the periodic table are called p-block elements. In addition to the noble gases, they include the families of boron, mercury, nitrogen, oxygen and fluorine. These elements have diverse real-life implementations that we regularly experience around us.

Metals and Non-metals

The periodic table is composed of metals, semi-metals and nonmetal elements. The physical and chemical properties of metals and nonmetals differ from each other. The study of metals and nonmetals will help one to understand the appropriate application of the particular element.

Question

6-10

1105-Sec2, Periodic Table, Problem supplement
True-False (A=True, B=False)
1. Atomic size decreases as you go down a vertical column.
2. Ionization energy is the energy necessary to remove valence electrons from atoms.
3. Increasing ionization energy means that generally less energy is required to remove an
electron from the elements going across a row, and it takes progressively more energy to
remove an electron when going down a column.
4. An atom that gives up an electron easily is more likely to take on another electron.
5. Atoms with high ionization energy will be able to hold another electron more easily.
6. Lower ionization energy indicates less attraction for additional electrons, and greater
ionization energy indicates greater desire for electrons.
7. Nonmetals like oxygen have the greatest chance to lo3e electrons.
8. Inert gases have very little desire to gain or to lose electrons.
9. A bond will result when one atom attracts the electrons of another atom.
10. An ionic bond forms when one atom completely removes a valence electron from another
atom.
11. An ionic bond is any bond that is made from ions.
12. Ionic bonds are the least common bonds in the minerals of the earth.
13. Almost all inorganic substances are ionic in nature.
14. Atoms with similar electronegativities form covalent bonds.
15. The amount of ionic and covalent character is determined by the difference in the
electronegativities of the atoms making up the compound.
16. An electron is completely taken away from another atom in a covalent bond.
17. All metals are liquid at room temperature except mercury.
18. Metallic bonds are directed bonds, but ionic and covalent bonds have bonding electrons that
roam.
19. If the difference between the electronegativity of two elements is less than 1.7, the percent
ionic character of the bond is less than 51% percent so the bond is covalent. (Think and
check the periodic table)

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