Question

unit 6 combo skills and vocabulary day 1
name:
period:
classifying a compound as either a covalent compound or an ionic compound: as you should recall from the previous unit, metals
make up most of the periodic table while nonmetals are on the left side of it. seventeen elements are generally classified as nonmetals: hydrogen,
upper right side of the periodic table with the exception of hydrogen, which is on top of the alkali metal family. covalent compounds are
certain nonmetals only. ionic compounds contain both metals and nonmetals. the relevant subscript numbers are shown on
the right side of the table. classify the following compounds as either a covalent compound (c) or an ionic compound (i)

1. $h_2o$
2. $base$
3. $cscl$
4. $crf_3$
5. $se_2o_3$
6. $se_2cl_2$
7. $co$
8. $br_2o$
9. $nh_3o$
10. $ibr$
11. $na_2s$
12. $pbbr_2$
13. $scl_2$
14. $cl_2o_6$
15. $p_4o_{10}$

naming an ionic compound: ionic compounds have a simple two - word name. the first word is the first element name. the second word is
a modified word for the second element such that the word ends in an - ide suffix. carbon becomes carbide. nitrogen becomes nitride.
phosphorus becomes phosphide. oxygen becomes oxide. sulfur becomes sulfide. selenium becomes selenide. fluorine becomes fluoride.
chlorine becomes chloride. bromine becomes bromide. iodine becomes iodide. the numbers of each element as denoted by the subscripts
in the chemical formula are irrelevant. keep it simple: a two - word name. name the following ionic compounds. add the second word of the
name without capitalization

$csbr$

cesium bromide

1. $mgse$

magnesium

1. $li_3p$

lithium

1. $ca_3n_2$

calcium

1. $nai$

sodium

1. $sro$

strontium

1. $kcl$

potassium

1. $baf_2$

barium

1. $bes$

beryllium

1. $al_4c_3$

aluminum
naming a covalent compound: covalent compounds use a more complex naming system that is tied to the number of each element. if
there is no subscript associated with the first element, the first word is the first element name. if there is a subscript 2 associated with the
first element, then the prefix di must be used in front of the first element name. the second word is a modified word for the second element
such that the word ends in an - ide suffix. but, the second element name with the - ide suffix must have a prefix. if there is no subscript
associated with the second element, the prefix is mono. (if the prefix is mono, this becomes monoxide). if there is a subscript 2 associated with the second element, the prefix is di. if there is a subscript 3 associated with the second element, the prefix is tri.
if there is a subscript 4 associated with the second element, the prefix is tetra. if there is a subscript 5 associated with the second element,
the prefix is penta. if there is a subscript 6 associated with the second element, the prefix is hexa. circle the correct prefix from the choices

1. $n_2o$

dinitrogen mono di tri tetra penta hexa oxide

1. $so$

sulfur mono di tri tetra penta hexa oxide

1. $sf_6$

sulfur mono di tri tetra penta hexa fluoride

1. $pbr_3$

phosphorus mono di tri tetra penta hexa bromide

1. $s_2cl_2$

disulfur mono di tri tetra penta hexa chloride

1. $if_3$

iodine mono di tri tetra penta hexa fluoride

1. $br_2o_5$

dibromine mono di tri tetra penta hexa oxide

1. $ccl_4$

carbon mono di tri tetra penta hexa chloride
classifying a property as either being descriptive of an ionic compound or a covalent compound: ionic compounds are typically hard,
brittle, have high melting points, have high boiling points, are usually soluble in water, are conductive in the molten state, are conductive
when dissolved in water, and easily form crystals. covalent compounds are typically soft, flexible, have low melting points, have low
boiling points, are not usually soluble in water, are not conductive in the molten state, are not conductive when dissolved in water, and
easily form oils. choose the best answer for the following characteristics: ionic compounds (i) or nonmetal compounds (c)

1. low boiling point.
2. hard.
3. easily forms crystals.
4. not conductive when dissolved in water.
5. brittle.
6. typically soluble in water.
7. not conductive in the molten state.
8. low melting point.

Explanation:

Step1: Classify compounds as ionic or covalent

• Ionic compounds are formed between metals and non - metals.
• Covalent compounds are formed between non - metals only.
• \(H_{2}O\): C (non - metals \(H\) and \(O\))
• \(Se_{2}Cl_{2}\): C (non - metals \(Se\) and \(Cl\))
• \(Na_{2}S\): I (metal \(Na\) and non - metal \(S\))
• \(BaSe\): I (metal \(Ba\) and non - metal \(Se\))
• \(CO\): C (non - metals \(C\) and \(O\))
• \(PbBr_{2}\): I (metal \(Pb\) and non - metal \(Br\))
• \(CsCl\): I (metal \(Cs\) and non - metal \(Cl\))
• \(Br_{2}O\): C (non - metals \(Br\) and \(O\))
• \(SCl_{2}\): C (non - metals \(S\) and \(Cl\))
• \(CrF_{3}\): I (metal \(Cr\) and non - metal \(F\))
• \(NH_{3}O\): C (non - metals \(N\), \(H\) and \(O\))
• \(Cl_{2}O_{6}\): C (non - metals \(Cl\) and \(O\))
• \(Sc_{2}O_{3}\): I (metal \(Sc\) and non - metal \(O\))
• \(IBr\): C (non - metals \(I\) and \(Br\))
• \(P_{4}O_{10}\): C (non - metals \(P\) and \(O\))

Step2: Name ionic compounds

• For \(Li_{3}P\): lithium phosphide
• For \(NaI\): sodium iodide
• For \(KCl\): potassium chloride
• For \(BeS\): beryllium sulfide
• For \(MgSe\): magnesium selenide
• For \(Ca_{3}N_{2}\): calcium nitride
• For \(SrO\): strontium oxide
• For \(BaF_{2}\): barium fluoride
• For \(Al_{4}C_{3}\): aluminum carbide

Step3: Name covalent compounds

• For \(N_{2}O\): dinitrogen monoxide
• For \(SF_{6}\): sulfur hexafluoride
• For \(S_{2}Cl_{2}\): disulfur dichloride
• For \(Br_{2}O_{5}\): dibromine pentoxide
• For \(SO\): sulfur monoxide
• For \(PBr_{3}\): phosphorus tribromide
• For \(IF_{5}\): iodine pentafluoride
• For \(CCl_{4}\): carbon tetrachloride

Step4: Classify properties

• Low boiling point: C (covalent compounds have low boiling points)
• Easily forms crystals: I (ionic compounds easily form crystals)
• Brittle: I (ionic compounds are brittle)
• Not conductive in the molten state: C (covalent compounds are not conductive in the molten state)
• Hard: I (ionic compounds are hard)
• Not conductive when dissolved in water: C (covalent compounds are not conductive when dissolved in water)
• Typically soluble in water: I (ionic compounds are typically soluble in water)
• Low melting point: C (covalent compounds have low melting points)

Answer:

1. \(H_{2}O\): C
2. \(Se_{2}Cl_{2}\): C
3. \(Na_{2}S\): I
4. \(BaSe\): I
5. \(CO\): C
6. \(PbBr_{2}\): I
7. \(CsCl\): I
8. \(Br_{2}O\): C
9. \(SCl_{2}\): C
10. \(CrF_{3}\): I
11. \(NH_{3}O\): C
12. \(Cl_{2}O_{6}\): C
13. \(Sc_{2}O_{3}\): I
14. \(IBr\): C
15. \(P_{4}O_{10}\): C
16. \(Li_{3}P\): lithium phosphide
17. \(NaI\): sodium iodide
18. \(KCl\): potassium chloride
19. \(BeS\): beryllium sulfide
20. \(MgSe\): magnesium selenide
21. \(Ca_{3}N_{2}\): calcium nitride
22. \(SrO\): strontium oxide
23. \(BaF_{2}\): barium fluoride
24. \(Al_{4}C_{3}\): aluminum carbide
25. \(N_{2}O\): dinitrogen monoxide
26. \(SF_{6}\): sulfur hexafluoride
27. \(S_{2}Cl_{2}\): disulfur dichloride
28. \(Br_{2}O_{5}\): dibromine pentoxide
29. \(SO\): sulfur monoxide
30. \(PBr_{3}\): phosphorus tribromide
31. \(IF_{5}\): iodine pentafluoride
32. \(CCl_{4}\): carbon tetrachloride
33. Low boiling point: C
34. Easily forms crystals: I
35. Brittle: I
36. Not conductive in the molten state: C
37. Hard: I
38. Not conductive when dissolved in water: C
39. Typically soluble in water: I
40. Low melting point: C