Practice Questions: Atomic Particles, Universal Forces, and Chemical Bonding | Lecture notes Chemistry

Practice Questions

Topic 1

For questions 1-9, match the description with the correct sub atomic particle(s)

a. Electron b. Proton c. Neutron d. Proton & neutron e. Proton & electron

1. Responsible for stabilizing the nucleus

2. Can be transferred or shared; responsible for

chemical bonding between atoms

3. Has a positive charge

4. Located in the nucleus

5. Makes up most of the mass of an atom

6. Does not have a charge; i.e. has a neutral

charge

7. Attracts and holds electrons to the atom

8. Creates Coulombic attraction

9. Has a tiny mass that is practically zero

10. How many protons does an atom of beryllium have? Beryllium as 4 protons

11. How many neutrons does an atom of nitrogen have? Nitrogen has a mass of 14 and 7 protons, so 14-7=7 neutrons

12. How many neutrons are in an atom of cesium? Cesium has a mass of 133 and 55 protons, so 133-55= 78 neutrons

13. How many electrons are there in a neutral atom of sodium? There are 11 electrons in a neutral sodiim atom

14. How many electrons are there in a sodium ion? Na loses 1 e- when it forms an ion, so there are 10 e- in a Na ion

15. How many electrons are in a neutral iodine atom? There are 53 e- in a neutral iodine atom

16. How many electrons are there in a iodide ion? Iodine gains 1e-, so there are 54 e- in an iodide ion

17. Iron has two oxidation numbers, 2 and 3. How many electrons are in an ion of iron (II) and in an iron (III)

ion? 24 e- 23e-

18. Which of the four universal forces--note, this should introduce

questions 19-23--there is no answer for #18

For questions 10-22, match the universal force with its role.Note the numbering error--- should be 19 through 22.

19. Hold matter together da. Strong force

20. Holds the atom together bb. Electromagnetic force

21. Holds the nucleus together ac. Weak force

22. Hold particles in the nucleus together cd. Gravitational force

23. Rank those forces from strongest to weakest: strong, electromagnetic, weak, gravitational

24. Write the number 2,600,000,000 in scientific notation 2.6 x 10 9

25. Write the number 0.0000000000000000000000000642 in scientific notation 6.42 x 10 -26

Topic 2 questions

26. Forces that hold atoms together are intra molecular forces

27. Forces that hold compounds together are inter molecular forces

Use the table to the right to answer questions 28 & 29

28. Which list below correctly ranks the molecules from lowest to highest boiling

points?

a. H2O  N2  O2  He

b. N2  H2O  He  O2

c. He  H2O  N2  O2

d. He



H2O ***

29. Which list below correctly ranks the molecules from weakest to strongest intermolecular forces?

a. H2O  N2  O2  He

b. N2  H2O  He  O2

c. He  H2O  N2  O2

d. He



H2O ***

30. In order to freeze into ice, the molecules that make up water have to:

a. get hotter

b. get colder

c. speed up

d. slow down ***

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Practice Questions

Topic 1

For questions 1-9, match the description with the correct sub atomic particle(s)

a. Electron b. Proton c. Neutron d. Proton & neutron e. Proton & electron

1. Responsible for stabilizing the nucleus

2. Can be transferred or shared; responsible for

chemical bonding between atoms

3. Has a positive charge

4. Located in the nucleus

5. Makes up most of the mass of an atom

6. Does not have a charge; i.e. has a neutral

charge

7. Attracts and holds electrons to the atom

8. Creates Coulombic attraction

9. Has a tiny mass that is practically zero

10. How many protons does an atom of beryllium have? Beryllium as 4 protons

11. How many neutrons does an atom of nitrogen have? Nitrogen has a mass of 14 and 7 protons, so 14-7=7 neutrons

12. How many neutrons are in an atom of cesium? Cesium has a mass of 133 and 55 protons, so 133-55= 78 neutrons

13. How many electrons are there in a neutral atom of sodium? There are 11 electrons in a neutral sodiim atom

14. How many electrons are there in a sodium ion? Na loses 1 e- when it forms an ion, so there are 10 e- in a Na ion

15. How many electrons are in a neutral iodine atom? There are 53 e- in a neutral iodine atom

16. How many electrons are there in a iodide ion? Iodine gains 1e-, so there are 54 e- in an iodide ion

17. Iron has two oxidation numbers, 2 and 3. How many electrons are in an ion of iron (II) and in an iron (III)

18. ion?Which of the four universal forces -- note, this should introduce 24 e- 23e-

questions 19-23--there is no answer for # For questions 10-22, match the universal force with its role. Note the numbering error--- should be 19 through 2 2.

19. Hold matter together d a. Strong force

20. Holds the atom together b b. Electromagnetic force

21. Holds the nucleus together a c. Weak force

22. Hold particles in the nucleus together c d. Gravitational force

23. Rank those forces from strongest to weakest: strong, electromagnetic, weak, gravitational

24. Write the number 2,600,000,000 in scientific notation 2.6 x 10 9

25. Write the number 0.0000000000000000000000000642 in scientific notation 6.42 x 10 -

Topic 2 questions

26. Forces that hold atoms together are intra molecular forces

27. Forces that hold compounds together are inter molecular forces

Use the table to the right to answer questions 28 & 29

28. Which list below correctly ranks the molecules from lowest to highest boiling

points? a. H 2 O  N 2  O 2  He b. N 2  H 2 O  He  O (^2)

c. He  H 2 O  N 2  O (^2) d. He  N 2  O 2  **H 2 O *****

29. Which list below correctly ranks the molecules from weakest to strongest intermolecular forces?

a. H2O  N2  O2  He b. N2  H2O  He  O

c. He  H2O  N2  O d. (^) He  N2  O2  **H2O *****

30. In order to freeze into ice, the molecules that make up water have to:

a. get hotter

b. get colder

c. speed up

d. **slow down *****

c

a

b

d

c

b

e

a

Figure 1

Use the phase diagram for CO 2 to

answer the following questions 31

to 34:

31. To change carbon dioxide from a

liquid to a gas you would need to ____________.

a. Increase the temperature and/or

**decrease the pressure *****

b. Decrease the temperature

and/or increase the pressure

c. Decrease both the temperature

and pressure

d. Increase both the temperature

and the pressure

32. Increasing the pressure around a

liquid will…

a. increase the boiling point of the liquid. ***

b. decrease the boiling point of the liquid.

c. not affect the boiling point of the liquid

33. To change carbon dioxide from a liquid to a solid you would need to ____________ (hint: make sure you look

closely at Figure 2 when choosing your answer).

a. Increase the temperature and/or decrease the pressure

b. Decrease the temperature and/or increase the pressure ***

c. Decrease both the temperature and pressure

d. Increase both the temperature and the pressure

34. Increasing the temperature of carbon dioxide from -100° C to -40° C at 1 atm of pressure would change it from

a solid to a vapor. This process is known as

a. Freezing

b. Melting

c. Condensation

d. Sublimation***

Topic 3 questions

Figure 1 depicts energy levels in an atom of an

unknown element that has been heated, and

produced green , indigo , red , yellow, and violet

color emissions. The direction of the arrow

indicates which direction the electron moves.

35. Which arrow represents the electron gaining

energy?

a. a

b. b

c. c

d. d

e. e

f. f

F

43. What is an ion? An ion is a charged atom with an uneven number of electrons because its lost or gained them

44. What type of ions do metals form? What type of ions do non-metals form? Metals form positive ions b/c they've

45. How many valence electrons and electron shells do each of the following elements have:

a. Helium 2 valence electons, 1 electron shells

b. Chlorine 7 valence electrons, 3 electron shells

c. Sodium 1 valence elctron, 3 electron shells

d. Calcium 2 valence electrons, 4 electron shells

e. Sulfur 6 valence elctrons, 3 electron shells

46. Pick two different elements on the periodic table, and determine based on their positions, which one has the

higher ionization energy and larger atomic radius. Answers will vary depending on the elements you chose, but that radius increases down, and decreases across. Ionization energy is opposite.

Topic 5

47. Summarize the similarities and differences between ionic and covalent bonds.

_Ionic bonds form through the transfer of electrons between cations (metals) and anions (non-metals). Their electronegativity difference is ~ greater than or equal to 1. ** Covalent bonds form through the the sharing of electrons between non-metals. Polar covalent bonds show electronegativity difference between 1.69 and 0.4; they display an uneven sharing of electrons. Non-polar bonds show an electronegativity difference less than or equal to 0.4, and evenly share electrons_**

48. What is the octet rule, and how can it be used to determine the number of electrons an atom will gain or

lose when it becomes an ion? Atoms want to gain or lose electrons to stabilize, and the most stable elements are those with full valence shells: the Noble gases. All but Helium have 8 valence electrons, and the prefix for 8 is "oct-", hence the "octet rule." Metals have fewer valence electrons than non-metals, and its "easier" for them to lose electrons to stabilize and take on the electron configuration of the closest Noble gas, which are "behind" them on the periodic table. Non-metals are the opposite, they gain electrons to take on the configuration of the closest Noble gas, which are "in front" of them on the periodic table.

Practice Questions: Atomic Particles, Universal Forces, and Chemical Bonding, Lecture notes of Chemistry

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Partial preview of the text

Download Practice Questions: Atomic Particles, Universal Forces, and Chemical Bonding and more Lecture notes Chemistry in PDF only on Docsity!

1. Responsible for stabilizing the nucleus

2. Can be transferred or shared; responsible for

3. Has a positive charge

4. Located in the nucleus

5. Makes up most of the mass of an atom

6. Does not have a charge; i.e. has a neutral

7. Attracts and holds electrons to the atom

8. Creates Coulombic attraction

9. Has a tiny mass that is practically zero

10. How many protons does an atom of beryllium have? Beryllium as 4 protons

11. How many neutrons does an atom of nitrogen have? Nitrogen has a mass of 14 and 7 protons, so 14-7=7 neutrons

12. How many neutrons are in an atom of cesium? Cesium has a mass of 133 and 55 protons, so 133-55= 78 neutrons

13. How many electrons are there in a neutral atom of sodium? There are 11 electrons in a neutral sodiim atom

14. How many electrons are there in a sodium ion? Na loses 1 e- when it forms an ion, so there are 10 e- in a Na ion

15. How many electrons are in a neutral iodine atom? There are 53 e- in a neutral iodine atom

16. How many electrons are there in a iodide ion? Iodine gains 1e-, so there are 54 e- in an iodide ion

17. Iron has two oxidation numbers, 2 and 3. How many electrons are in an ion of iron (II) and in an iron (III)

18. ion?Which of the four universal forces -- note, this should introduce 24 e- 23e-

19. Hold matter together d a. Strong force

20. Holds the atom together b b. Electromagnetic force

21. Holds the nucleus together a c. Weak force

22. Hold particles in the nucleus together c d. Gravitational force

23. Rank those forces from strongest to weakest: strong, electromagnetic, weak, gravitational

24. Write the number 2,600,000,000 in scientific notation 2.6 x 10 9

25. Write the number 0.0000000000000000000000000642 in scientific notation 6.42 x 10 -

26. Forces that hold atoms together are intra molecular forces

27. Forces that hold compounds together are inter molecular forces

28. Which list below correctly ranks the molecules from lowest to highest boiling

29. Which list below correctly ranks the molecules from weakest to strongest intermolecular forces?

30. In order to freeze into ice, the molecules that make up water have to:

a. get hotter

b. get colder

c. speed up

c

a

b

d

d

c

b

e

a

Use the phase diagram for CO 2 to

answer the following questions 31

to 34:

31. To change carbon dioxide from a

a. Increase the temperature and/or

b. Decrease the temperature

c. Decrease both the temperature

d. Increase both the temperature

32. Increasing the pressure around a

liquid will…

a. increase the boiling point of the liquid. ***

b. decrease the boiling point of the liquid.

c. not affect the boiling point of the liquid

33. To change carbon dioxide from a liquid to a solid you would need to ____________ (hint: make sure you look

a. Increase the temperature and/or decrease the pressure

b. Decrease the temperature and/or increase the pressure ***

c. Decrease both the temperature and pressure

d. Increase both the temperature and the pressure

34. Increasing the temperature of carbon dioxide from -100° C to -40° C at 1 atm of pressure would change it from

a. Freezing

b. Melting

c. Condensation

d. Sublimation***

Topic 3 questions

Figure 1 depicts energy levels in an atom of an

unknown element that has been heated, and

produced green , indigo , red , yellow, and violet

color emissions. The direction of the arrow

indicates which direction the electron moves.

35. Which arrow represents the electron gaining

a. a

b. b

c. c

d. d