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1. What are the properties of IONIC substances? These substances: -Solid Hard and brittle (like salt) at room temp -Conduct electricity when dissolved.

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Presentation on theme: "1. What are the properties of IONIC substances? These substances: -Solid Hard and brittle (like salt) at room temp -Conduct electricity when dissolved."— Presentation transcript:

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2 1. What are the properties of IONIC substances? These substances: -Solid Hard and brittle (like salt) at room temp -Conduct electricity when dissolved in water -High boiling/melting points

3 2. What are the properties of COVALENT substances? These substances: -MOST are liquids/gases at room temp -Do not conduct electricity when dissolved in water -Most can not dissolve in water -Low boiling/melting points

4 3. What’s the difference between ionic BONDING and covalent BONDING? Ionic Covalent Transfer electronsShared electrons Metal/nonmetalsNonmetals Has a chargeNo charge Single bonds onlyCan have double/triple bonds

5 4. Why do atoms form bonds? Atoms are trying to fill their valence orbit with a stable octet of electrons- in the case of hydrogen it’s a duet

6 5. What are diatomic molecules? Name 7 of them. Diatomic molecules are molecules that are made up of 2 identical atoms to become a molecule. H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2

7 6. How many electrons are involved in covalent bonding?____ 2 shared electrons or a pair of electrons

8 7. What is bond dissociation energy? The energy needed to separate a covalent bond

9 8. What properties determine bond strength? The number of bonds. As the number of electrons being shared increases this shorted the distance between the atoms becoming stronger- more energy to separate them.

10 9. Provide the Lewis structure, the VSEPR shape and determine the polarity for the following Lewis Structure VSEPR shapePolarity H2SH2S Bent Polar SO 2 Bent Polar BH 3 Trigonal planer Non SF 4 Trigonal Bipyramidal Non

11 10. What are the 10 prefixes to molecular compound naming? Mono- 1 Di- 2 Tri- 3 Tetra- 4 Penta- 5 Hexa- 6 Hepta- 7 Octa- 8 Non-9 Deca- 10

12 11. What is the difference between a nonpolar covalent bond and a polar covalent bond? Provide an example. Nonpolar covalent bond is where the electrons are shared equally between the atoms. Ex: Cl-Cl Polar covalent bond is where the electrons are not shared equally between the atoms. Ex: H-Cl

13 12. Can a molecule have polar covalent bonds and be nonpolar? Explain your answer. Yes, they can. CCl 4, the bond between Carbon and Chlorine is a polar covalent bond (chlorine has most of the electrons) but the overall molecule would be nonpolar.

14 13. Rank the following bonds according to increasing polarity. a. C-H b. N-H c. Si-H d. O-H e. Cl-H Think electronegativity! Silicon has the lowest electronegativity so ( c) is the least polar Carbon is next (a) Nitrogen is more electronegative (b) Chlorine is bigger so second best (e) Oxygen is the most so (d)

15 14. Match the following- answers can be used more than once or have multiple answers. 1. Induced dispersion 2. Dipole-dipole 3. Hydrogen bonding a. H-H _____e. nonpolar covalent____ b. H-F _____f. polar covalent____ c. C-Cl____g. attraction to nucleus & electrons ___ d. O-O ____h. attraction to adjacent atoms___ or 3 1 1, 2, 3

16 Name or Formula Ionic or Covalent ANSWER Li 2 O Nitrogen dibromide SBr 6 Aluminum phosphide Boron monosulfide SO 2 CN 2 Potassium nitride Chlorine trifluoride Nitrogen disulfide Magnesium phosphide IonicLithium oxide CovalentNBr 2 CovalentSulfur hexabromide IonicAlP CovalentBS CovalentSulfur dioxide CovalentCarbon dinitride Ionic K3NK3N CovalentClF 3 CovalentNS 2 IonicMg 3 P 2


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