Ionic Bonding Science 10
-
Upload
raymond-riley -
Category
Documents
-
view
26 -
download
0
description
Transcript of Ionic Bonding Science 10
![Page 1: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/1.jpg)
Ionic BondingScience 10
1
![Page 2: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/2.jpg)
Keeping Track of Electrons• The electrons responsible for the chemical
properties of atoms are those in the outer energy level.
• Valence electrons – The electrons in the outer energy level (in valence shell).
• Kernel (core) electrons -those in the energy levels below the valence shell.
2
![Page 3: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/3.jpg)
Keeping Track of Electrons
• Atoms in the same column• Have the same number of outer electrons
(valence electrons).• Easily found by looking up the group number on
the periodic table.• Group 2 - Be, Mg, Ca, .- 2 valence electrons• The last digit in the representative group
number gives the number of valence electrons
3
![Page 4: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/4.jpg)
Electron Dot diagrams (Lewis Structure)
• A way of keeping track of valence electrons.
• How to write them• Write the symbol.• Put one dot for each valence
electron• Don’t pair up until they have
to
X4
![Page 5: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/5.jpg)
The Electron Dot diagram for Nitrogen
Nitrogen has 5 valence electrons.
First we write the symbol.
NThen add 1 electron at a time to each side.Until they are forced to pair up.
5
![Page 6: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/6.jpg)
Write the electron dot diagram for
• Na• Mg• C• O• F• Ne• He
6
![Page 7: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/7.jpg)
Electron Configurations for Cations
• Metals lose electrons to attain noble gas configuration (Born losers).
• They make cations (positive ions).• If we look at electron configuration it
makes sense.• Na 2, 8, 1 - 1 valence electron• Na+ 2, 8 -noble gas configuration (Ne)
7
![Page 8: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/8.jpg)
Electron Dots For Cations• Metals will have very few valence electrons
CaCalcium has two valence electrons (Group 2)
8
![Page 9: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/9.jpg)
Electron Dots For Cations• Metals will have very few valence electrons• These will come off
Ca9
![Page 10: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/10.jpg)
Electron Dots For Cations• Metals will have very few valence electrons• These will come off• Forming cations (positive ions)
Ca2+
Calcium has lost two valence electrons10
![Page 11: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/11.jpg)
Electron Configurations for Anions
• Nonmetals gain electrons to attain noble gas configuration.
• They make anions (negative ions).• If we look at electron configuration it makes
sense.• S 2, 8, 6 - 6 valence electrons• S2- 2, 8, 8 -noble gas configuration (Ar).
11
![Page 12: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/12.jpg)
Electron Dots For Anions• Nonmetals will have many valence electrons.• They will gain electrons to fill outer shell.
P P3-
12
![Page 13: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/13.jpg)
Stable Electron Configurations• All atoms react to achieve noble gas
configuration.• Noble gases have 8 valence electrons .• Also called the octet rule.
Ar13
![Page 14: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/14.jpg)
Ionic Bonding - the basics• Metals form positive ions.• Non-metals form negative ions.• Anions and cations are held together by opposite
charges.• Ionic compounds are called salts.• The bond is formed through the transfer of electrons.
(From metals to nonmetals.)• Electrons are transferred to achieve noble gas
configuration.• The valence electrons determine the formula. (Simplest
ratio is called the formula unit.)
14
![Page 15: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/15.jpg)
Ionic Bonding
Na Cl
15
![Page 16: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/16.jpg)
Ionic Bonding
Na+ Cl-
Na lost 1 electron to form 1+ cation Cl gains 1 electron to form a 1- anionThe + and – attract (force of attraction is called an ionic bond) holds the ions together.The ratio is 1:1 so the formula is NaCl
16
![Page 17: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/17.jpg)
Counting ElectronsDuring the formation of an ionic compound the total
number of electrons lost (by metals in forming cations) must equal the total number of electrons gained (by non-metals in forming anions).
Ca Group 2 loses 2 e-
P Group 15 (5A) gains 3e-
To keep totals equal a LCM of 6 is used.Therefore: 3 x Ca = 3 x 2+ = 6+
2 x P = 2 x 3- = 6-
6 lost (+6) = 6 gained (6-) Charges cancel.
17
![Page 18: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/18.jpg)
Ionic Bonding
• All the electrons must be accounted for, total lost = total gained!
Ca P
18
![Page 19: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/19.jpg)
Ionic Bonding
Ca P
19
![Page 20: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/20.jpg)
Ionic Bonding
Ca2+ P
20
![Page 21: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/21.jpg)
Ionic Bonding
Ca2+ P
Ca21
![Page 22: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/22.jpg)
Ionic Bonding
Ca2+ P3-
Ca22
![Page 23: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/23.jpg)
Ionic Bonding
Ca2+ P3-
Ca P23
![Page 24: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/24.jpg)
Ionic Bonding
Ca2+ P3-
Ca2+ P24
![Page 25: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/25.jpg)
Ionic Bonding
Ca2+ P3-
Ca2+ P
Ca
25
![Page 26: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/26.jpg)
Ionic Bonding
Ca2+ P3-
Ca2+ P
Ca
26
![Page 27: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/27.jpg)
Ionic Bonding
Ca2+ P3-
Ca2+P3-
Ca2+
27
![Page 28: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/28.jpg)
Ionic Bonding
Ca3P2
Formula UnitThe Ca to P ratio is 3:2 so:
3 x 2+ = 6+ 2 x 3 – = 6 –6+ + 6– = 0
(# e– lost = # e– gained)
28
![Page 29: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/29.jpg)
+1 +2 +3 +4 -3 -2 -1 0
Most Transition Metals do not have form cations of one fixed charge, they tend to have variable charges.
29
![Page 30: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/30.jpg)
Properties of Ionic compounds:• High melting points.• Conduct electricity when dissolved in water or in
molten state. • They do not conduct electricity in solid state because
the electrons are not able to move.• Ionic substances tend to be electrolytes - a substance
that dissolves in water to produce a solution that will conduct electricity.
• Solid are a crystal lattice.
30
![Page 31: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/31.jpg)
Some common binary ionic compounds:
• NaCl – table salt• KCl – potash• AlCl3 antiperspirant
• CaCl2 – road salt
31
![Page 32: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/32.jpg)
Naming fixed binary ionic compounds
• Ionic compounds are formed between metals and non-metals. When naming them, we name the Cation (metal) first, then we name the anion (non-metal) last- changing the last part of the name of the element to “ide”.
• Ex: chlorine – chloride• oxygen – oxide• nitrogen - nitride
32
![Page 33: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/33.jpg)
Formula Writing and Naming:Fixed Binary ionic compounds
• Formula: write the cation first and anion last.• Name: Name the cation first (use the element name) • Name the anion but change the ending to “ide”
So, Formula: KClName: potassium chloride
33
![Page 34: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/34.jpg)
Example- Show the formation of the compound formed between Na and O.
Formula Na2O
Name: sodium oxide34
![Page 35: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/35.jpg)
Show the formation of CaCl2.
Name: calcium chloride
35
![Page 36: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/36.jpg)
• Show the formation of the following fixed binary ionic compounds using electron-dot structures (Lewis structures). Also write the names of the compounds.
• a) K3P• b) NaF• c) Al2O3
• Predict the formula and name the compounds formed when the following elements react.
• a) K and F• b) Li and O• c) Mg and P
36
![Page 37: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/37.jpg)
Write the formula and the name for the ionic compound formed from each of the following ions.
• a) Ca2+ and Cl-
• b) Al3+ and N3-
• c) Be2+ and O2-
• d) Be2+ and N3-
• e) K + and S2-
37
![Page 38: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/38.jpg)
Practice: Name the following binary ionic compounds:
A) MgOB) Al2SC) K3ND) ZnF2
E) CaCl2F) LiClG) CsFH) NaBrI) BaF2
J) HCl
Magnesium oxideAluminum sulfidePotassium nitridezinc fluoridecalcium chlorideLithium chlorideCesium fluorideSodium bromideBarium bromideHydrogen chloride
38
![Page 39: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/39.jpg)
What about those ones in the “middle”?
• Metals, so they form positive ions (cations)• They can form different ions (variable charge)
eg, Fe2+, Fe3+
39
![Page 40: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/40.jpg)
Examples….
40
![Page 41: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/41.jpg)
Naming variable binary ionic compounds
• Ionic compounds formed between metals with variable charge and non-metals. When naming them, we name the metal first and state the charge in Roman numerals in brackets , then we name the non-metal last- changing the last part of the name of the element to “ide”.
• Roman numerals:• 1 – I 4 – IV 7 – VII 10 – X • 2 – II 5 – V 8 – VIII • 3 – III 6 – VI 9 – IX
41
![Page 42: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/42.jpg)
Ionic compounds with transition metals:
FeCl3 Fe3+ 3Cl1-
Cl Fe Cl
FeCl3
Cl
iron(III) chloride
Cu2SCu S Cu 2Cu1+ S2-
copper(I) sulfide
42
![Page 43: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/43.jpg)
Write the formulas for the following compounds.a) copper(I) oxideb) lead(IV) bromidec) iron(III) sulfided) nickel(III) fluoridee) manganese(IV) sulfideWrite the names of the following compounds.(Use the
anion to calculate the charge of the cation.)a) FeCl2
b) FeOc) Cu2O
d) PbO243
![Page 44: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/44.jpg)
Polyatomic ions…ions made up of 2 or more elements.
44
![Page 45: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/45.jpg)
Ionic compounds with polyatomic ions…
NH41+ and S2-
NH4 1+ S 2- NH4
1+ Charges cancel
2NH41+ S2-
(NH4)2S
ammonium sulfide45
![Page 46: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/46.jpg)
Write the formula for the following ionic compounds
a) Ca2+ & NO31-
b) Na1+ & OH1-
c) K1+ & SO42-
d) Ba2+ & PO43-
e) Li1+ & HCO31-
46
![Page 47: Ionic Bonding Science 10](https://reader035.fdocuments.in/reader035/viewer/2022062221/568134c6550346895d9bebb9/html5/thumbnails/47.jpg)
Naming Ionic Compounds with polyatomic ions
Name the cation: 1) fixed name the element 2) variable element name followed by (roman numeral) 3) name the positive polyatomic (only for NH4
1+) then the anion
Name the negative polyatomic ionWrite the name for the ionic compounds from the previous
slide.
47