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50 notecards = 13 pages (4 cards per page)

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Chapters 2 and 3

front 1

Once labor begins in childbirth, contractions increase in intensity and frequency until delivery. The increasing labor contractions of childbirth are an example of which type of regulation?

back 1

positive feedback

front 2

In comparing covalent bonds and ionic bonds, which of the following would you expect?

back 2

Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons

front 3

What is the maximum number of hydrogen atoms that can be covalently bonded in a molecule containing two carbon atoms?

back 3

6

front 4

Which statement is true of all atoms that are anions?

back 4

The atom has more electrons than protons.

front 5

When two atoms are equally electronegative, they will interact to form

back 5

nonpolar covalent bonds

front 6

In what way are elements in the same column of the periodic table the same?

back 6

They have the same number of electrons in their valence shell.

front 7

A water sample from a hot thermal vent contained a single-celled organism that had a cell wall but lacked a nucleus. What is its most likely classification?

back 7

Archaea

front 8

What results from an unequal sharing of electrons between atoms?

back 8

a polar covalent bond

front 9

What is the difference between covalent bonds and ionic bonds?

back 9

Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the electrical attraction between atoms.

front 10

A covalent bond is likely to be polar when

back 10

one of the atoms sharing electrons is much more electronegative than the other atom.

front 11

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by

back 11

polar covalent bonds.

front 12

Why does ice float in liquid water?

back 12

Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water.

front 13

Based on your knowledge of the polarity of water molecules, the solute molecule depicted here is most likely

back 13

positively charged.

front 14

Which of the following is a hydrophobic material?

back 14

wax

front 15

Water molecules are able to form hydrogen bonds with

back 15

compounds that have polar covalent bonds.

front 16

Which of the following solutions would require the greatest amount of base to be added to bring the solution to neutral pH?

back 16

gastric juice at pH 2

front 17

Increased atmospheric CO2 concentrations might have what effect on seawater?

back 17

Seawater will become more acidic, and carbonate concentrations will decrease.

front 18

The bonds that are broken when water vaporizes are

back 18

hydrogen bonds between water molecules.

front 19

The partial negative charge in a molecule of water occurs because

back 19

the electrons shared between the oxygen and hydrogen atoms spend more time around the oxygen atom nucleus than around the hydrogen atom nucleus.

front 20

Sulfur is in the same column of the periodic table as oxygen, but has electronegativity similar to carbon. Compared to water molecules, molecules of H2S

back 20

will not form hydrogen bonds with each other.

front 21

A covalent chemical bond is one in which

back 21

outer-shell electrons of two atoms are shared so as to satisfactorily fill the outer electron shells of both atoms.

front 22

Which of the following would be regarded as compounds?

back 22

H2O and CH4, but not O2

front 23

The atomic number of nitrogen is 7. Nitrogen-15 is heavier than nitrogen-14 because the atomic nucleus of nitrogen-15 contains how many neutrons?

back 23

8

front 24

Protists and bacteria are grouped into different domains because

back 24

protists have a membrane-bounded nucleus, which bacterial cells lack.

front 25

Which bond or interaction would be difficult to disrupt when compounds are put into water?

back 25

covalent bond

front 26

One difference between carbon-12 () is that carbon-14 () has

back 26

two more neutrons than carbon-12

front 27

The main source of energy for producers in an ecosystem is

back 27

Light

front 28

A 0.01 M solution of a substance has a pH of 2. What can you conclude about this substance?

back 28

It is a strong acid that ionizes completely in water

front 29

You have two beakers. One contains a solution of HCl at pH = 1.0. The other contains a solution of NaOH at pH = 13. Into a third beaker, you slowly and cautiously pour 20 mL of the HCl and 20 mL of the NaOH. After complete stirring, the pH of the mixture will be

back 29

7.0

front 30

Which of the following takes place as an ice cube cools a drink?

back 30

Kinetic energy in the drink decreases

front 31

Why does evaporation of water from a surface cause cooling of the surface?

back 31

The water molecules with the most heat energy evaporate more readily.

front 32

Temperature usually increases when water condenses. Which behavior of water is most directly responsible for this phenomenon?

back 32

the release of heat by the formation of hydrogen bonds

front 33

Which type of bond must be broken for water to vaporize?

back 33

hydrogen bonds

front 34

Liquid water's high specific heat is mainly a consequence of the

back 34

absorption and release of heat when hydrogen bonds break and form.

front 35

In what way are elements in the same column of the periodic table the same?

back 35

They have the same number of electrons in their valence shell.

front 36

Prokaryotes are classified as belonging to two different domains. What are the domains?

back 36

Bacteria and Archaea

front 37

In the term trace element, the modifier trace means that

back 37

the element is required in very small amounts.

front 38

Why is each element unique and different from other elements in chemical properties?

back 38

Each element has a unique number of protons in its nucleus.

front 39

About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living matter?

back 39

carbon, hydrogen, nitrogen, oxygen

front 40

Which of the following is not considered to be a weak molecular interaction?

back 40

a covalent bond

front 41

Compared with 31P, the radioactive isotope 32P has

back 41

one more neutron.

front 42

Which of the following effects is produced by the high surface tension of water?

back 42

A water strider can walk across the surface of a small pond.

front 43

Which of the following is a hydrophobic material?

back 43

wax

front 44

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called?

back 44

a hydrogen bond

front 45

Which of the following are qualities of any good scientific hypothesis?
I. It is testable.
II. It is falsifiable.
III. It produces quantitative data.
IV. It produces results that can be replicated.

back 45

I and II

front 46

Which of the following explains most specifically the attraction of water molecules to one another?

back 46

hydrogen bond

front 47

Nitrogen (N) is much more electronegative than hydrogen (H). Which of the following statements is correct about the atoms in ammonia (NH3)?

back 47

Each hydrogen atom has a partial positive charge; the nitrogen atom has a partial negative charge.

front 48

Which of these individuals is likely to be most successful in an evolutionary sense?

back 48

an organism that dies after five days of life but leaves 10 offspring, all of whom survive to reproduce

front 49

Hydrophobic substances such as vegetable oil are

back 49

nonpolar substances that repel water molecules.

front 50

When the body's blood glucose level rises, the pancreas secretes insulin and, as a result, the blood glucose level declines. When the blood glucose level is low, the pancreas secretes glucagon and, as a result, the blood glucose level rises. Such regulation of the blood glucose level is the result of

back 50

negative feedback.