Chapter 4 - Inorganic Chemistry

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Terms to Know in This Chapter:

matter

element (sing.)

compound (sing.)

mixture (sing.)

molecule [MOLL eh cule]

diatomic molecule

polyatomic molecule

atom

nucleus (sing.) [NEW klee us]
nuclei (pl.) [NEW klee eye]

mass

weight

atomic number

atomic weight (mass)

protium [PRO tee um]

deuterium [due TERR ee um]

tritium [TREH tee um]

ion [EYE on]

cation [CAT ion]

anion [AN ion]

isotope [EYE so tope]

orbitals (pl.)

s orbital

p orbital

d orbital

f orbital

g orbital

h orbital

i orbital

spatial orientation [SPAY shull]

energy level

electron configuration

electron (sing.)

quantum numbers n,l,m,s

spin

ionic bond

covalent bond

hydrogen bond

Van der Waals [Valls]

polar covalent bond

nonpolar covalent bond

acid

base

salt

hydrogen ion

hydroxide ion [high DROX ide]

neutralization reaction

pH

buffer

carbonic acid [car BON ik]

hydrochloric acid [hi drow CHLOR ik]

hydrofluoric [hi drow FLUR ik]

metal

nonmetal

synthetic

Pauli's Exclusion Principle

Heisenberg's Uncertainty Principle

sweet, sour, salt, bitter

taste

litmus [LIT mus]

equilibrium

What You Need to Know:

You should be able to:

1. define an element and pure substance,
2. explain which atoms are naturally occurring and which are synthetic,
3. distinguish between a diatomic molecule and polyatomic molecule and be able to list the diatomic molecules,
4. tell the relative weights (masses) and charges associated with a proton, a neutron, and an electron,
5. distinguish between mass and weight,
6. calculate the number of neutrons for any element,
7. determine which element you are dealing with when you know the atomic weight (mass) and the number of neutrons,
8. calculate the charge of an atom in its ground state (naturally occurring state),
9. determine the number of electrons and protons and neutrons of any atom in its ground state,
10. write the electron configuration for selected elements on the periodic chart,
11. give the name of the element when provided with the electron configuration,
12. explain an isotope,
13. explain how an ion is formed,
14. explain the difference between a cation and anion,
15. describe how an ionic bond may form,
16. describe a covalent bond,
17. distinguish between a polar covalent bond and nonpolar covalent bond,
18. explain a hydrogen bond,
19. explain what constitutes an acid and give its characteristics,
20. explain what constitutes a base and give its characteristics,
21. explain the formation of a salt,
22. define pH and explain how the scale works, what constitutes a strong or weak acid or base, and what is neutral,
23. explain a buffer system and how it functions, and
24. give an example of a common buffer system in your body.
    

Exercises: Fill in the Blank.

1. A material composed of a single type of matter would be called either a pure substance or a(n): .
2. Water (H₂O)is an example of both and a while H₂ would be considered only a . (molecule or compound)
3. Neptunium is an element not found naturally on the earth and is thus considered to be a element. (natural or synthetic).
4. An atom with an atomic mass of 139 and an atomic number of 57 would have neutrons. The name of that element would be and if there were another substance that also had an atomic number of 57 but an atomic mass of 141, then we would consider that element to be a(n) of the first element mentioned (ion, isomer, isotope)
5. An element that has an atomic mass of 184 and 110 neutrons in its nucleus would be the element .
6. Calcium may lose two electrons and thus become a positively charged ion called a(n) . (cation or anion)
7. Oxygen may often gain two electrons and have a -2 charge and thus become a(n) . (cation or anion)
8. The electron configuration for Strontium would be .
9. The electron configuration for Indium (In) would be
10. The proper sequence of filling of electrons is as follows:
11. An element with the electron configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d¹⁰6p⁴ would be the element .
12. The element would have an electron configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰.
13. The oxygen ion would have an electron configuration of
14. A molecule formed from the electrostatic attraction of unlike charged particles would be called a(n) bond.
15. A(n) bond occurs when the positive region of a hydrogen atom attracts the negative region of another atom, ion, or molecule.
16. The overall charge on an atom in its ground state (naturally occurring state) is .
17. The overall charge on a molecule is .
18. The overall charge on a compound is .
19. Water is an example of a(n) bond while hydrogen gas (H₂) is an example of a(n) bond.(ionic, polar covalent, nonpolar covalent)
20. An unequal sharing of electrons results in a(n) bond.