LECTURE CHAPTER 2 REVIEW

Question 1

The _____ states that energy cannot be created or destroyed.

Question 2

The atomic number of an element indicates the number of _____ of a specific element?

Question 3

What condition must exist for an atom to be electrically balanced?

Question 4

What are ions?

Question 5

How can radioactive isotopes be used in medical science?

Question 6

What are valence electrons? If the atomic number of potassium is 15. How many electrons are found in the valence shell of this atom in its non-ionic state?

Question 7

The _____, states that except for the first energy shell (stable with two electrons), atoms are stable with _____ electrons in their valence shell (Note: Yet, understand that shells 2 through 7 can hold more electrons.)
a. The numbers listed represent the first, second, and third energy levels, respectively. On this basis, which of the following three is an unstable atom? (1) 2, 8; (2) 2,8,2; (3) 2, 8, 8
b. Atom X is electrically balanced and has ten protons. How many electrons are in its valence shell?
c. Atom Z has an atomic number of 74. What can you determine from this number?
+ d. Be able to draw the planetary model for the atoms of elements 1 through 18 (Hydrogen to Aragon). Place electrons in their correct orbitals and label protons, neutrons, and electrons by using the following symbols protons = , neutrons = , and electrons = e–.

Question 8

The formula H2O means there are _____ hydrogen and _____ oxygen atoms.

Question 9

Chemical energy is an example of _____, which is stored or inactive energy.

Question 10

A _____ is an atom that has lost one or more of its electrons.

Question 11

Salts, like NaCl (table salt), H2SO4, and MgSO4 are _____ compounds.

Question 12

The chemical behavior of an atom is determined by the _____ in its outermost energy shell.

Question 13

In an _____ bond, the atoms completely transfer electrons from one to another.

Question 14

In a _____ bond, the atoms share electrons.

Question 15

A _____ bond is a weak chemical bond formed when a partially positive hydrogen atom in a molecule is attracted to a partially negative atom in another molecule. It is most easily seen between _____ molecules.

Question 16

What do the chemical symbols, H - H, O = O, and N ≡ N mean?

Question 17

What is the difference from an endergonic and exergonic chemical reaction? Give examples.

Question 18

What influences the speed or rate of a chemical reaction?

Question 19

The reaction A + B → AB is an example of _____ reaction.

Question 20

The reaction AB + CD → AD + CB is an example of _____ reaction.

Question 21

Monosaccharides joining together to make a disaccharide is a good example of a _____ reaction.

Question 22

Two good examples of a colloid would be Jell-O or _____.

Question 23

Tell whether the following solutions are considered an acid or a base: pH of 9, pH of 2, pH of 7,
pH of 8, pH of 12, pH of 7.4

Question 24

What are the differences between mixtures and compounds?

Question 25

What will happen to the pH of water if MgOH is dissolved in it?

Question 26

Adding acid tends to _____ the hydrogen ion concentration of a solution.

Question 27

What is a buffer?

Question 28

What is an organic molecule? Give examples.

Question 29

What is an inorganic molecule? Give examples.

Question 30

What does it mean when it is said that water is a polar molecule?

Question 31

What is cohesion and adhesion? What are examples of water portraying these characteristics?

Question 32

What takes place in a dehydration synthesis reaction? hydrolysis reaction? What happens to water in each of the reactions?

Question 33

Which functional group(s) would cause a molecule like citric acid to be acidic?

Question 34

Which functional group(s) are present in an amino acid?