Summer Assignment: AP Biology

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This deck includes 38 flashcards covering potential energy, atomic number, atomic mass, and related concepts. Use it to review key Chemistry ideas, focus on weak cards, and prepare for your exam with StudyLess.

1. 01

   Subatomic particle directly involved in chemical reactions between atoms

   Electrons

2. 02

   Essential element

   Elements that an organism needs to live a healthy life and reproduce

3. 03

   Atomic mass

   The total mass of an atom

4. 04

   Isotope

   Different forms of the same element

5. 05

   Electron shells

   A fixed region or energy level surrounding an atom's nucleus where electrons orbit

6. 06

   Energy

   The capacity to cause change

7. 07

   Which has more potential energy: boy at the top of a slide or boy at the bottom?

   Boy at the top

8. 08

   Which has more potential energy: electron in the first energy shell or electron in the third energy shell?

   Electron in the third shell

9. 09

   Which has more potential energy: water or glucose?

   Glucose

10. 10

    Neutron

    A subatomic particle found inside the nucleus with no electrical charge

11. 11

    Atomic mass of helium

    4.0026

12. 12

    Atomic number of helium

    2

13. 13

    Trace element

    Elements required by an organism in only minute quantities

14. 14

    Four elements making up 96% of all living matter

    Oxygen, Carbon, Hydrogen, and Nitrogen

15. 15

    Compound

    A substance consisting of two or more different elements combined in a fixed ratio

16. 16

    Electron

    A fundamental, negatively charged subatomic particle

17. 17

    Element

    Substance that cannot be broken down to other substances by chemical reactions

18. 18

    Atomic number

    Number of protons

19. 19

    Potential energy

    The energy that matter possesses because of its location or structure

20. 20

    What determines the chemical behavior of an atom?

    The distribution of electrons in the atom's electron shells.

21. 21

    How many valence electrons does sodium have?

    1

22. 22

    How many protons does sodium have?

    11

23. 23

    What does a double bond mean?

    Forms a molecule by sharing two pairs of valence electrons.

24. 24

    Difference between nonpolar and polar covalent bonds

    Nonpolar covalent: Electrons are shared equally (same electronegativity). Polar covalent: Electrons of the bond are not shared equally (different electronegativity).

25. 25

    Which element is most electronegative in water?

    Oxygen

26. 26

    Why is water considered a polar molecule?

    The unequal sharing of electrons due to oxygen's higher electronegativity creates partial positive charges on hydrogen and a partial negative charge on oxygen.

27. 27

    Describe the process of forming an ionic bond between sodium and chloride.

    An electron is transferred from sodium to chloride, forming a cation (Na+) and an anion (Cl-), resulting in an ionic bond.

28. 28

    Molecule

    Two or more atoms held together by covalent bonds

29. 29

    Electronegativity

    The attraction of a particular atom for the electrons of a covalent bond

30. 30

    Define anion and cation. Which is the anion in the NaCl example?

    Anion: Negatively charged ion. Cation: Positively charged ion. In the NaCl example, Cl- is the anion.

31. 31

    What is a hydrogen bond?

    A noncovalent attraction between a hydrogen atom and an electronegative atom.

32. 32

    Explain van der Waals interactions.

    Interactions between ever-changing regions of positive and negative charge that enable all atoms and molecules to stick to one another. Individually weak and occur only when atoms and molecules are very close together.

33. 33

    Order the following bonds and interactions from strongest to weakest: hydrogen bonds, van der Waals interactions, covalent bonds, ionic bonds.

    Strongest: Covalent bonds, Ionic bonds, Hydrogen bonds, van der Waals interactions: Weakest

34. 34

    Why is molecular shape crucial in biology, using morphine and endorphins as examples?

    Molecular shape determines how biological molecules recognize and respond to one another with specificity. Morphine has a similar shape to endorphins, allowing them to bind to the same specific receptor molecules on brain cells.

35. 35

    What is meant by dynamic equilibrium?

    The reactions are still going on in both directions but do not affect the concentrations of reactants and products.

36. 36

    Matter

    Anything that takes up space and has mass

37. 37

    Proton

    A tiny, positively charged subatomic particle found inside the center of every atom

38. 38

    Carbon atom properties: atomic mass, atomic number, electrons, neutrons

    Atomic mass: 12, Atomic number: 6, Electrons: 6, Neutrons: 6

39. 39

    Adhesion definition

    The clinging of one substance to another.

40. 40

    What is demonstrated when you see beads of water on a waxed car hood?

    Both cohesion (water clinging to itself) and adhesion (water clinging to the car).

41. 41

    Which property explains the ability of a water strider to walk on water?

    Surface tension, due to water molecules being hydrogen-bonded to each other and the water below, but not the air above.

42. 42

    Specific heat definition

    The amount of heat that must be absorbed or lost for 1g of that substance to change its temperature by 1°C.

43. 43

    How does water's specific heat compare to alcohol's?

    Water's specific heat (1 cal/(g*°C)) is unusually high compared to alcohol's (0.6 cal/(g*°C)).

44. 44

    How does hydrogen bonding contribute to water's high specific heat?

    Heat must be absorbed to break hydrogen bonds, and is released when they form, thus small temperature changes occur as heat is absorbed/released to disrupt/form bonds.

45. 45

    How does water's high specific heat contribute to the moderation of temperature?

    Large bodies of water absorb/release heat with minimal temperature change, stabilizing temperatures and creating a favorable environment for marine life.

46. 46

    Evaporation definition

    The transformation from a liquid to a gas.

47. 47

    Heat of vaporization definition

    The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state.

48. 48

    What is evaporative cooling?

    As a liquid evaporates, the surface of the liquid that remains behind cools down.

49. 49

    List two effects of evaporation on living organisms.

    1. Cooling of plant tissues as water evaporates from leaves. 2. Dissipation of body heat in humans through sweat evaporation.

50. 50

    Why does ice float?

    Because it is less dense than liquid water; water expands as it solidifies.

51. 51

    Why is the property of ice floating important for life on Earth?

    If ice sank, ponds and oceans would freeze solid from the bottom up, making life impossible.

52. 52

    Calorie definition

    The amount of heat it takes to raise the temperature of 1g of water by 1°C.

53. 53

    What does it mean that water has a high specific heat?

    Water requires a lot of heat to change its temperature by 1°C for 1g.

54. 54

    Solvent definition

    The dissolving agent of a solution.

55. 55

    Solution definition

    A liquid that is a completely homogeneous mixture of two or more substances.

56. 56

    Solute definition

    The substance that is dissolved.

57. 57

    In coffee with sugar, what is the solvent and what is the solute?

    Coffee is the solvent, and sugar is the solute.

58. 58

    Explain why water is such a fine solvent.

    The partially negative oxygens attract cations, and the partially positive hydrogens attract anions, allowing water molecules to surround and shield individual ions.

59. 59

    Hydrophilic definition

    Any substance that has an affinity for water.

60. 60

    Hydrophobic definition

    Any substance that does not have an affinity for water (nonionic & nonpolar substances that repel water).

61. 61

    Explain why oil floats on water in terms of hydrogen bonding.

    Oil molecules have relatively nonpolar covalent bonds, preventing them from forming hydrogen bonds with water and causing them to repel water.

62. 62

    What is a polar molecule?

    A molecule with an unevenly distributed charge.

63. 63

    Why is water considered polar?

    Due to the unequal sharing of electrons (oxygen is more electronegative than hydrogen) and its bent shape.

64. 64

    Explain why ice floats, focusing on the critical temperature of 4°C.

    Above 4°C, water behaves like other liquids. As it cools from 4°C to 0°C, molecules slow down and hydrogen bonds lock them into a crystalline lattice, expanding the volume and making ice less dense than liquid water.

65. 65

    Explain hydrogen bonding.

    Two molecules are held together as the partially positive hydrogen of one molecule is attracted to a partially negative oxygen of a nearby molecule.

66. 66

    How many hydrogen bonds can a single water molecule form?

    Four

67. 67

    Cohesion definition

    The hydrogen bonds holding the substance together.