Unit 4 Exam Chemical Bonding Study Guide

Unit 4 Exam

Chemical Bonding

Study Guide

Test Date:________________

Test Format:

Multiple Choice Questions

Open Response

Topics to be tested:

Notes ? be responsible for all material we discussed in class

Worksheets ? look at your answers, correct mistakes and be prepared for them to reappear on

test

Large Topics you should know the details of...

o Covalent bond o Determine multiple bonds in covalent compounds o Differentiate cation and anion o Drawing Lewis structures for ionic and covalent compounds o Identify polyatomic ions o Ionic bond o Naming compounds o Octet rule o Predict the type of bond between two atoms (ionic, covalent, or no bonding) o Valence electrons o Writing chemical formulas o Periodic trends (electronegativity, atomic radius, ionization energy)

1. What happens during ionic bonding? Valence electrons are transferred from a metal to a nonmetal creating cations and anions that are attracted to each other.

2. How are ionic bonds held together? Electrostatic forces between a cation and anion.

3. Ionic bonds are between M_e_ta_l_s _(c_at_io_n_s) and __N_on_m_e_ta_ls_(a_n_io_n_s)__.

4. What is an ion? How can a neutral atom become an ion?

An atoms that has lost or gained electrons creating a charge. 5. What are positively charged ions called? _____C__a__t_io__n_s________ How does an atom become

positively charged? Loses electrons

6. What are negatively charged ions called? _____A__n_i_o__n_s________ How does an atom become negatively charged? Gains electrons

7. What is an oxidation number?

Charge that ions normally make when bonding

8. When do you use Roman Numerals in naming compounds?

To show the charge of multivalent ions.

9. What is the octet rule?

Most atoms need 8 valence electrons in their outermost shells in order to be stable.

10. What is a polyatomic ion?

An ion with more than one element.

11. What happens during covalent bonding?

Valence electrons are shared between two nonmetals. 12. Covalent bonds are between _N__o__n_m__e__t_a_l_s______________.

13. Oxygen's atomic number is ______, so it will have ______ valence electrons and it wants to lose/gain (circle one) ______ more electrons to fill the shell. The resulting ion's charge after bonding is ______________.

14. Sodium's atomic number is _______, so it will have ______ valence electrons, and wants to lose/gain (circle one) ______ more electrons to fill the shell. The resulting ion's charge after bonding is _____________.

15. Draw a lewis dot diagram of what happens when Ca bonds with chlorine.

16. Draw a lewis dot diagram of what happens when Sr bonds with oxygen.

17. Draw a lewis dot diagram of what happens when 3 Hydrogens bond to one Nitrogen creating NH3

18. Draw a lewis dot diagram of what happens when 2 Fluorines bond to one Sulfur creating SF2

19. Draw a lewis dot diagram of what happens when 4 Chlorines bond to one Carbon creating CCl4

20. List the prefixes used in naming covalent compounds:

Number of atoms

Prefix

1

Mono

2

Di

3

Tri

4

Tetra

5

Penta

6

Hexa

7

Hepta

8

Octa

9

Nona

10

Deca

State whether the following compounds are ionic or covalent compound and give their names:

Ionic or Covalent

Name of Compound

21. HgBr 22. SO3 23. P2O5 24. KCl 25. Ba(NO3)2

Ionic Covalent Covalent Ionic Ionic

mercury (I) bromide sulfur trioxide Diphosphorus pentoxide potassium chloride barium nitrate

Name the following covalent compounds:

26. NO2 27. CO

_N__it_ro__g_e_n_d__io_x_i_d_e________________ _C__a_rb__o_n_m__o_n_o_x_i_d_e_______________

28. S3Cl5 29. S8O5 30. Br2I 31. SiF4

_T_r_is_u_l_f_e_r_p_e_n_t_a_c_h_l_o_r_id_e___________ _O__c_ta_s_u__lf_e_r_p_e_n_t_o_x_i_d_e____________ _D__ib_r_o_m__id_e__m__o_n_o_i_o_d_id_e___________ _S_i_li_c_o_n__te_t_r_a_fl_u_o_r_i_d_e_____________

Write the formula for the following covalent compounds:

32. Phosphorus trichloride 33. Phosphorus monoxide 34. Disilicon tetrachloride 35. Trinitrogen hexafluoride 36. Pentabromine heptachloride 37. Diphosphorus pentoxide

_____________________ ____________________ _____________________ ____________________ ____________________ ____________________

Name the following ionic compounds:

38. NH4Cl 39. Mg(OH)2 40. Zn(NO3)2 41. Ag3PO4 42. Pb3N2 43. Ti(CN)4

_A_m__m_o__n_iu_m__c__h_lo_r_id__e_________ _M__a__g__n_e__s_i_u__m___h__y_d__r_o__x_i_d__e__________ _Z__in__c__(_I_I_)_n__i_t_r_a__t_e_________________ _S_il_v_e_r_p_h_o__s_p_h_a_t_e___________ _L_e_a_d__(I_I)_n_i_t_ri_d_e______________ _T_it_a_n_i_u_m__(_IV_)_c_y_a_n__id_e_________

Write the formula for the following ionic compounds:

44. Calcium Iodide

____________

45. Tin (IV) sulfide

____________

46. Sodium bicarbonate

____________

47. Copper (II) sulfate

_____________

48. Iron(III) phosphate

_____________

49. Lithium chloride

____________

50. Draw the electron dot structure for each molecule. a. O2

d. H2O

b. NCl3

e. N2

c. CH4

f. CO2

51. A chemical bond formed when atoms share two pairs of electrons is called a(n).__C_o_v_a_l_e_n_t_b_o_n_d_____

52. How many electrons are in a single covalent bond? ___double covalent bond?___ triple covalent bond? __ 53. What is the trend of electronegativity on the periodic table?

Increases up and to the right

54. What is the trend of ionization energy on the periodic table?

Increases up and to the right

55. What is the trend of atomic radius on the periodic table?

Increases down and to the left

 ................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download