F - SO 3 Cl 2. The particles that have lost or gained electrons and have positive or negative charge.

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1 INTERACTIONS BETWEEN CHEMICAL SPECIES Part II? What are the names of each species? Br 2 Cl F - SO 4-2 H - OH - SO 3 Cl 2 H 2 O? Match the given species with the correct definitions and examples: Atom The particles that have lost or gained electrons and have positive or negative charge. H + Molecule The smallest particle of an element that retains the chemical property of it. H 2 Ion The species that are formed by aggregation of the same or different kinds of atoms. H Let s do something: Boiling of Water J Take little amount of water into a beaker. Put it on the heater. Observe water until it finishes. Then answer the following questions. 1- What is the chemical structure of water? 2- What type of a chemical specie is it? 3- What kinds of bonds are found in a) the structure of water particles and b) among the water particles? 4- What happens while water is boiling? (Think on the basis of bonds/interactions between particles.) a) b) 1

2 Electrolysis of Water All you need in order to see electrolysis in action is a battery and a couple pencils! (Adult supervision required.) Materials: 6-volt or 9-volt battery Two alligator clip leads Beaker or glass Piece of thin cardboard or cardstock Two #2 pencils Procedure: Fill the beaker or glass with distilled water. Carefully sharp both ends of each pencil. (These pencils are your electrodes. The graphite in them will conduct electricity, but won t dissolve into the water.) Cut a piece of the cardboard to fit over the beaker, then punch two holes in the center of the cardboard about an inch apart. Push the pencils through the holes and set them in the beaker. They should extend into the water, but not touch the bottom of the glass. The cardboard will hold them in place. Connect each pencil to the battery with an alligator clip lead attached to the exposed graphite (pencil lead). Observe and answer the following questions. Questions and Conclusion: 1- What did you observe? 2- What did you obtain on the end of each pencil? How did you understand this? 3- Does one pencil collect more bubbles than the other? Which one? Why do you think this is? 4- Which bonds of water were broken during electrolysis? 5- Compare the amount of energies which were required to boil water and for electrolysis of water? 6- Compare the strengths of broken bonds of water while boiling and during electrolysis. 2

3 Let s try to state that which of the following bonds can be broken easily and which of them very hard, why? H 2 O H 2 O H O H Question: What is the difference between given two bonds? Question: What are the types of given species? 3

4 Exercise: Write the types of chemical species and predict whether interactions between them are weak or strong: (Write an explanation for your choice!) Think on these questions to determine the strength of the interactions!!! H + H à H-H Explanation: Choose: WEAK STRONG K + + Cl - à K + -Cl - Explanation: Choose: WEAK STRONG Cl 2 + Cl 2 à Cl 2 Cl 2 Explanation: Choose: WEAK STRONG HCl + HCl à HCl HCl Explanation: Choose: WEAK STRONG Summary: STRONG interactions are formed by or their WEAK interactions are formed by or. 4

5 STRONG INTERACTIONS IONIC BOND A. Give the answers for the following questions. 1. What is tendency of metals for their valence electrons to become stable? 2. What is tendency of non-metals for their valence electrons to become stable? 3. What are the charges of metal as they are in their most stable state? 4. What are the charges of non-metal as they are in their most stable state when they meet with metals? 5. How does an interaction occur when the most stable states of elements come together? 6. What is the name of this interaction asked on the previous question? 7. What should be the Lewis structures of metals when they are in their most stable forms? (State the metals with M ) 8. What should be the Lewis structures of non-metals when they are in their most stable forms as they meet with metals? (State the non-metals with N, and write the Lewis structure of hydrogen individually by using its symbol H) 9. What is the general Lewis structure of ionic bonded compounds by using the abbreviations M and N? 5

6 B. Answer the following questions for all given elements. 3Li, 4 Be, 7 N, 8 O, 9 F, 11 Na, 12 Mg, 13 Al, 15 P, 16 S, 17 Cl, 19 K, 20 Ca a) What is the type of each element? b) Write the Lewis structures of both their neutral and ion forms? c) Classify the ions as cations and anions. Cations Anions d) Form some ionic bonded compounds by using ionic Lewis structures of oppositely charged ions. Naming of Ionic Compounds: Ionic compounds are formed by electrostatic attractions between metal ions (positively charged ions are called as cations) and nonmetal (negatively charged ions are called as anions) ions. Formulas of ionic compounds are written by making total charge zero. Ionic compounds are named by using the names of their ions. Anion names of elements end with ide suffix. eg: Na + : Sodium & Cl - : Chloride è (+)+(-)=0 è NaCl: Sodium chloride 6

7 Let s see the mostly used cations and anions: I A H II A IIIA IV A V A VI A VII A Li Be N O F VIII A He Na Mg Al P S Cl K Ca VI B Fe I B Cu Ag II B Zn Br I Ba TRANSITION ELEMENTS The only Polyatomic Cation is Polyatomic Anions: NH 4 + : Ammonium OH - : Hydroxide SO 4-2 : Sulfate PO 4-3 : Phosphate NO 3 - : Nitrate HCO 3 - : Hydrogen carbonate (bicarbonate) CO 3-2 : Carbonate CrO 4-2 : Chromate Cr 2 O 7-2 : Dichromate Anions F - : Fluoride Cl - : Chloride Br - : Bromide I - : Iodide H - : Hydride OH - : Hydroxide NO - 3 : Nitrate NO - 2 : Nitrite CH 3 COO - : Acetate MnO - 4 : Permanganate CN - : Cyanide ClO - : Hypochlorite ClO - 2 : Chlorite ClO - 3 : Chlorate ClO - 4 : Perchlorate HCO - 3 : Bicarbonate HSO - 4 : Bisulfate O -2 : Oxide S -2 : Sulfur SO -2 4 : Sulfate SO -2 3 : Sulfite CrO -2 4 : Chromate Cr 2 O -2 7 : Dichromate C 2 O -2 4 : Oxalate MnO -2 4 : Manganate CO -2 3 : Carbonate P -3 : Phosphide N -3 : Nitride PO -3 4 : Phosphate PO -3 3 : Phosphite 7

8 F While naming ionic compounds, cation and anion names are said respectively: AlBr 3 : Aluminum bromide NaCl : Sodium chloride Ca 3 N 2 : Calcium nitride BeO : Beryllium oxide MgSO 4 : Magnesium sulfate NaNO 3 : Sodium nitrate AlPO 4 : Aluminum phosphate (NH 4 ) 2 CrO 4 : Ammonium chromate NOTE: If metal can take changing valences, its valence is stated in parenthesis with Roman numbers. CuCl : Copper (I) chloride CuCl 2 : Copper (II) chloride FeO : Iron (II) oxide Fe 2 O 3 : Iron (III) oxide Write the formulas and the names of ionic compounds that are formed by the following ions: K + and O -2 Ca +2 and Br - Ba +2 and I - Ag + and Cl - K + and P -3 Mg +2 and SO 4-2 Al +3 and NO 3 - NH 4 + and CO 3-2 Be +2 and OH - Zn +2-2 and CrO 4 Li + -2 and Cr 2 O 7 Na + - and HCO 3 Al +3-3 and PO 4 Fe +3 and O -2 Fe +2 and S -2 Cu + and N -3 Cu +2 and SO 4-2 8

9 Some compounds have common names that don t include names of elements: NaCl: Table salt è Sodium chloride NaOH: Coastic soda è NaHCO 3 : Baking soda/baking powder è CaO: Quicklime è Ca(OH) 2 : Slaked lime è CaCO 3 : Lime stone è Examine the web site in the QR-code and then answer the following questions. Properties of Ionic Compounds Worksheet 1) Explain why ionic compounds do not conduct electricity in their crystalline form. 2) Why do metals and nonmetals usually form ionic compounds, whereas two bonded nonmetals are never ionic? Explain. 3) Why is the formation of ionic compounds exothermic? 4) Why do ionic compounds tend to be hard? 5) Describe whether the following compounds are likely to be ionic or not ionic based on the properties given. Explain your reasoning. Compound 1 has a melting point of 545 degrees Celsius and dissolves well in water. Compound 2 is a brittle material that is used to melt road ice during storms. 9

10 Draw a diagram which contains the properties of ionic compounds: IONIC COMPOUNDS 10

11 COVALENT BOND Think about these photos and find the common properties of them: commitment-sharing/ Exercise: A- Give the answers for the following questions. 1. What is the tendency of non-metals to become stable? 2. Write the Lewis dot structures of 1 H and 17 Cl atoms: 3. How do the 1 H and 17 Cl atoms come together to form a compound? 4. What is the Lewis structure of the compound that is formed by 1 H and 17 Cl atoms? 5. What is the name of the interaction between 1 H and 17 Cl atoms? 11

12 B- Answer the following questions: a) What is the electron configuration and the types of given elements? - 6 X - 17 Y - 1 Z - 8 T b) State the tendency of elements given in the previous question to become stable. c) How many bonds should each of them form to become stable? d) State what kind of bonds they can make to become stable. e) What are the Lewis structures of following molecules? CS 2 CCl 4 H 2 S Cl 2 OF 2 NF 3 f) Why should the non-metals form covalent bond (or share valence electrons) among themselves instead of transferring electrons? g) How can you distinguish whether any compound ionically or covalently bonded? 12

13 Naming of Covalent Bonded Compounds The Latin number of the 1 st nonmetal and name + The Latin number of the 2 nd nonmetal and its anion name 1: Mono 2: Di 1-3: 2- Tri 3- ÖRNEK: 4: Tetra 4-5: 5- Penta 6: 6- Hexa 7-7: 8- Hepta 8: 9- Octa 9: Nona 10: Deca If the number of the first nonmetal is 1, Mono is not said!!! CO CO 2 NO N 2 O NO 2 N 2 O 4 N 2 O 5 OF 2 SF 6 : Carbon monoxide : Carbon dioxide : Nitrogen monoxide : Dinitrogen monoxide : Nitrogen dioxide : Dinitrogen tetra oxide : Dinitrogen penta oxide : Oxygen difluoride : Sulphur hexafluoride BUT, If the second nonmetal is 1, mono should be said before its anion name. ClF 7 : Chlorine heptafluoride Latin numbers that are used as prefixes in the names of covalent compounds: 1 à mono 2 à di 3 à tri 4 à tetra 5 à penta 6 à hexa Exercise: Write the names of given compounds: SO 2 N 2 O 4 SO 3 N 2 O 5 CS 2 ICl CCl 4 P 2 O 5 N 2 O PF 3 N 2 O 3 OF 2 NO ClO 2 NO 2 SCl 6 What are the common names of following compounds? H 2 O: NH 3 : CH 4 : 13

14 Reflection Exercise: Write the compound type whether ionic of covalent and then write the names of them. If the compounds have common name please write it also. Ca(OH) 2 : N 2 O 5 : Na 2 O: P 2 O 3 : AlCl 3 : PCl 3 : NaNO 3 : N 2 O 4 : LiNO 3 : OF 2 : CaSO 4 : CO 2 : Be(OH) 2 : NO: KNO 3 : SO 2 : K 2 O: NO 2 : CaO: H 2 O: NaCl: N 2 O: KOH: P 2 O 5 : NaOH: NH 3 : CaCO 3 : CO: MgNO 3 : HCl: Na 2 CO 3 : KCl: SO 3 : 14

15 METALLIC BOND Answer the following questions while watching the video: 1- How many electrons do metals have on their valence shell? A few electrons. 2- How are the electrons used to form ionic compounds between atoms? Electrons are transferred from metals to non-metals. 3- How are the electrons used to form covalent compounds between atoms? They are shared. 4- How do the electrons move around the atoms in metallic bond? They roam/wander around the atom and form a sea of electrons. 5- What type of a structure do the metals form? Metals form compact and orderly crystalline structure with delocalized electrons. 6- What is the definition of metallic bonding? A bonding that takes place from the attraction of metal atoms and the surrounding sea of electrons. 7- What are the physical properties of metals that are caused by the electron sea? Metallic Bond: (Video Metallic Bonding) 15

16 Properties of Metals: 16