states that atoms will give up, accept, or share electrons in order to have 8 electrons in the outer shell.

Chapter 2 Chemical Foundation Of Life Flashcard Questions

1. Any substance that occupies space and has mass is called _______________.

 

2. An __________________ is a substance whose atoms all have the same number of protons (atomic number).

 

 

3. Smallest unit of matter that retains all of the chemical properties of an element is called __________________.

 

4. The best-known subatomic particles are
5. ______________________ that has ______________ charge.
6. ______________________ that has ______________ charge.

• _______________________ that has ______________ charge.

 

5. Please label the image below using the following vocabulary:

Nucleus, electron, proton, neutron.

 

6. The atomic particle that has positive charge and resides in the nucleus is called ________________.
7. The atomic particle that has no charge and resides in the nucleus is called ________________.
8. The atomic particle that has negative charge and is whizzing around the nucleus is called ________________.
9. Explore the properties of matter and elements by completing each sentence.
10. Atomic number
11. atoms, elements
12. hydrogens
13. isotopes
14. mass number
15. matter
16. Neutrons
17. Protons
19. Electrons
20. Molecule
21. water

• Any object that takes up space and has mass is considered to be ______________.
• Nonliving and living matter are composed of _______________.
• The atomic theory states that elements are comprised of_____________.
• Atoms with the same ___________are said to belong to the same element.
• The atomic number of an element reflects the number of ___________ in each atom of that element.
• The ____________ of an element reflects the number of protons and neutrons in each atom of that element.
• ______________ have a negative charge and are NOT located in the nucleus of the atom.
• An isotope is a form of an element that differs in the number of _____________.
• The bonding of two or more atoms forms a ______________.
• An example of a very important compound is the combination of two atoms of hydrogen and one oxygen to form _________________.
• The number of protons in the nucleus of an atom is called _________________.

 

10. __________________ is the sum of the number of protons and neutrons in the nucleus of an atom.

 

 

11. Electron mass is considered zero.
12. True
13. False

 

12. The atomic number of an atom normally tells you the number of electrons.
13. True
14. False
15. _____________________ are atoms of a single element that differ in their number of neutrons.

 

14. Atoms that have the same number of protons, but different mass numbers are called _________________.

 

 

15. _____________ ___________________ states that atoms will give up, accept, or share electrons in order to have 8 electrons in the outer shell.

 

16. The electrons on the outermost shell are called _____________ electrons.

 

17. The outermost shell of an atom is called ________________ shell.

 

18. _____________ ______________ occur when 2 or more atoms bond together to form molecules or when bonded atoms are broken apart.

 

 

19. _____________ are the starting participants in the chemical reaction.

 

20. ______________ are formed by the chemical reaction.
21. Label the chemical reaction below:
22. ___________ _______________ is a lasting attraction between atoms that enables the formation of chemical compounds.

 

23. 2 or more different elements bonded together are called ________________.

 

24. _________________ are the smallest part of a compound that still has the properties of that compound and is made of 2 or more atoms.

 

25. An atom or molecule that has either lost or gained electrons

 

1. Molecule
2. Isotope
3. Ion
4. None of the above

 

26. When two atoms do not have completely full outer shells, they may share electrons so that each has a full outer shell. This bond is called
27. Ionic
28. Covalent
29. Hydrogen
30. None of the above

 

27. polar covalent bond is a(an) ___________ sharing of electrons between atoms
28. Equal
29. Unequal
30. __________________ is the attraction of an atom for the electrons in a covalent bond.
31. Electronegativity
32. Ionic attraction
33. Electropositivity

 

29. Polarity of water molecules causes the hydrogen atoms in one molecule to be attracted to the oxygen atoms in other water molecules. This bond is called:
30. Ionic bond
31. Covalent bond
32. Hydrogen bond
33. Van der Waals bond

 

30. Van der Waals bond is easily broken.
31. True
32. False

 

31. Van der Waals bond is represented by a dotted line.
32. True
33. False
34. Write the type of the bond in the boxes below:

 

 

33. If an atom loses an electron, it will have a positive charge and it is called:
34. molecule
35. isotope
36. Anion
37. Cation

 

34. If an atom gains an electron, it will have a negative charge and it is called:
35. molecule
36. isotope
37. Anion
38. Cation

 

35. Ions with opposite charges attract and form ionic bonds.
36. True
37. False

 

36. Match the statements and the types of bonds listed below:

Covalent bonds, ionic bonds, hydrogen bonds

• Bonds between water molecules.
• Electrons are transferred between 2 atoms creating positively and negatively charged atoms, which are then attracted to one another.
• Strong chemical bond due to the sharing of electrons.
• Bonds between charged molecules or portions of a molecule.
• Na⁺ + Cl^– à NaCl
• Bonds between hydrogen and oxygen atoms within a water molecule
• Weak attraction between slightly charged parts of molecules, which are readily broken and reformed.

 

37. __________ ________________ bonds are written as H-H.
38. __________ ________________ bonds are written as O=O.
39. __________ ________________ bonds are written as N≡N.
40. Nonpolar covalent bond is a(an) ___________ sharing of electrons between atoms
41. Equal
42. Unequal
43. Water’s hydrogen bonds help it dissolve other polar molecules.
44. True
45. False
46. _________________ molecules cannot attract water.
47. Hydrophobic
48. Hydrophilic
49. Polar
50. Nonpolar
51. A and C
52. Oil and water do not mix because water is non-polar, and oil is polar.
53. True
54. False
55. ________________ ___________________ accounts for most of the properties of water that make life possible.
56. Hydrogen bonds
57. Covalent bonds
58. Oxygen bonds
59. Carbon bonds
60. The chemical bond within a water molecule is a ______ bond.
61. Covalent bond
62. Hydrogen bond
63. Ionic bond
64. Van der Waals bond

 

46. The characteristic that causes water molecules stick together is called ____________.

 

47. The characteristic that causes water molecules stick to other polar molecules is called ____________.
48. Match the statements and the types of bonds listed below:
49. Positive
50. Covalent
51. Electron
52. Hydrogen
53. hydrogen chloride
54. ionic, one pair
55. sodium chloride
56. Stronger
57. 3 pairs
58. 2 pairs
59. Weaker

 

1. An ion is formed when one atom transfers at least one __________ to another atom, causing a charge imbalance in each atom.
2. when sodium reacts with chlorine, an ionic compound called ____________ results.
3. The typical ____________ bond occurs when two atoms share at least one pair of electrons.
4. Hydrogen will only share _____________ of electrons when forming a covalent bond.
5. The more bonds shared covalently between two atoms, the ____________ the bond becomes.

 

 

49. Capillary action in a glass tube is caused by the _______________.
50. Adhesion
51. Cohesion
52. None of the above

 

50. Substances that dissociate in water, releasing excessive amount of hydrogen ions (H⁺) are called _____________.
51. Substances that dissociate in water, releasing excessive amount of hydroxide ions (OH^–) are called ______________.
52. Write which one is acidic and which one is basic.

 

 

 

 

In the statement below choose which is acidic, basic or neutral.

 

53. When Hydrogen ion concentration [H⁺] equals hydroxide ion concentration [OH^–], the solutions is _____________.

 

54. When Hydrogen ion concentration [H⁺] is greater than hydroxide ion concentration

[OH^–], the solutions is _____________.

55. When Hydroxide ion concentration [OH^–] is greater than hydrogen ion concentration

[H⁺], the solutions is _____________.

56. A solution which resists pH changes is
57. A buffer
58. A hydrophobic solution
59. An acid
60. A hydrophilic solution
61. A base

 

57. Alkalosis, cramping, and irritability can occur when our blood pH rises above 7.45.  Acidosis, seizures, coma and death can occur when our blood pH falls below pH 7.35.  To prevent these conditions, our blood usually has chemicals which
58. keep pH at neutral state.
59. can take up excess hydrogen ions.
60. can produce more water molecules.
61. can take up excess hydroxide ions.
62. can take up both excess hydrogen ions and excess hydroxide ions.

 

58. A chemistry student measures the pH of a solution as 7.1. The student adds five milliliters of an acid to the solution and finds that the pH of the solution is still 7.1. What conclusion could be made from these observations?
59. The original solution was buffered.
60. The original solution was weakly basic.
61. The original solution was weakly acidic.
62. The original solution was strongly acidic.
63. The original solution was strongly basic.