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Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-
- -
1s
2s
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
Na
1s
1s2
+
+
+
+
+
+
+ +
++
+
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron- -
-
- -
1s
2s
2px
-+
+
+
+
+
+
+ +
++
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
Na
1s
1s2
2s
2s2
2p
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-
- --
-
-
- -
1s
2s
2px
2py
2pz
+
+
+
+
+
+
+ +
++
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
Na
1s
1s2
2s
2s2
2p
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
+
+
+
+
+
+
+ +
++
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
Na
1s
1s2
2s
2s2
2p
2p6
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
+
+
+
+
+
+
+ +
++
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
Na
1s
1s2
2s
2s2
2p
2p6
3s
3s
-
3s1
Chemical Bonds
Sodium
Na11
22.990 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-+
+
+
+
+
+
+ +
++
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Na
Na
- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
3s
-
Na
1s
1s2
2s
2s2
2p
2p6
3s
3s1
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
+
+
+
+
+
+
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+- -
1s
2s
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
Cl
1s
1s2
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+ -
-
- -
1s
2s
2px
-
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
Cl
1s
1s2
2s
2s2
2p
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
Cl 1s2 2s2
- --
-
-
- -
1s
2s
2px
2py
2pz
1s 2s2p
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
Cl
1s
1s2
2s
2s2
2p
2p6
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
3s
-
Cl
1s
1s2
2s
2s2
2p
2p6
3s
3s2
-
3p
3px
-
-
3py3pz
-
Chemical Bonds
Chlorine
Cl17
35.453 Atomic Mass
Atomic NumberName
Symbol
+
+
+
+
+
+
+ +
++
++ proton
neutron
electron-+
+
+
+
+
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Cl
Cl
- -
-- --
-
-
- -
1s
2s
2px
2py
2pz
3s
-
Cl
1s
1s2
2s
2s2
2p
2p6
3s
3s2
-
3p
3px
-
-
3py3pz
--
-
3p5
Chemical Bonds
BeAtomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Be
Be
Be
Chemical Bonds
Beryllium
Be4
9.012 Atomic Mass
Atomic NumberName
Symbol
+ proton
neutron
electron-+
+ +
+
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Be
Be
-
-
- -
1s
2s
Be
1s
1s2
2s
2s2
Chemical Bonds
Oxygen
O8
15.999 Atomic Mass
Atomic NumberName
Symbol
+
++
+
++
+
+
+ proton
neutron
electron-
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
O
O
--
--- -
-
1s
2s
2px
2py
2pz
O
1s
1s2
2s
2s2
2p
2p4
-
Draw orbital notations for the following:
C1s 2s
2p
Mg1s 2s
2p3s
Ne1s 2s
2p
P1s 2s
2p3s
3p
Draw electron configurations for the following:
Draw electron-dot (Lewis-Dot)structures for the following:
C 1s2 2s2 2p2
Ca
P
Mg 1s2 2s2 2p6 3s2
Ne 1s2 2s2 2p6
1s2 2s2 2p6 3s2 3p3
1s2 2s2 2p6 3s2 3p6 4s2
C
Mg
Ca
P
Ne
Ca1s 2s
2p3s
3p4s
Draw orbital notations for the following:
Draw electron configurations for the following:
Draw electron-dot (Lewis-Dot)structures for the following:
U U1s 2s
2p
U 1s2 2s2 2p6
3s
3s2
3p
3p6 4s2
4s
3d
3d10
4p5s
4d
4p6 5s2 4d10
5p
5p6
6s
6s2
5d 4f
4f14 5d10
6p7s
6p6 7s2
6d 5f
5f36d1
Na1s 2s
2p3s
Na
Forming an Ionic Bond
Cl1s 2s
2p3s
3p
Cl
-ClNa+
Na+
Cl-
Be1s 2s
O1s 2s
2p
Be
O
+
Be +
O--
Sodium chloride
Beryllium oxide -OBe++ -
Forming an Ionic Bond
CaCa1s 2s
2p3s 4s
3p
F1s 2s
2p
F
Ca2+
F 1-
Ca F2
Calcium fluoride
AlAl1s 2s
2p3s
3p
S
Al 3+
S 2-
Al2 S3
Aluminum sulfide
S1s 2s
2p3s
3p
Forming an Ionic Bond
KK1s 2s
2p3s 4s
3p
N1s 2s
2p
N
K 1+
N3-
K3 N
Potassium nitride
LiLi1s 2s
C
Li1+
C4-
Li4 C
Lithiumcarbide
C1s 2s
2p
Forming an Ionic Bond
MgMg1s 2s
2p 3s
O1s 2s
2p
O
Mg2+
O2-
Mg O
Magnesiumoxide
NaNa1s 2s
2p3s
Se
Na1+
Se 2-
Na2 Se
Sodiumselenide
Se1s 2s
2p3s
3p
4s3d 4p
-ClNa+
-OBe++ -
Chemical Bond -the force that holds two atoms together-formation of chemical bonds allows atoms to form a Noble Gas configuration of valence electrons, allowing them to become more stable and exist at a lower state of potential energy
A. Ionic Bond -chemical bond formed by the exchange of electrons between a very electropositive atom (metal) and a very electronegative atom (nonmetal) which results in the formation of oppositely- charged ions, which are strongly attracted to each- other
Ionic compounds
-electronegativity is the tendency for an atom to attract electrons in order to form a chemical bond
-ionic bonds are those that have a relative electronegativity difference of more than 1.7
A. Ionic Bond
-the electronegativity difference is ______ in Sodium chloride and ______ in Beryllium oxide
2.12.0
NameChemical Formula
1. Na___O___ _______________
2. Be___Cl___ _______________
3. K___Br___ _______________
4. Ca___S___ _______________
5. Li___O___ _______________
6. Mg___F___ _______________
7. Rb___I___ _______________
8. Al___S___ _______________
9. Sr___N___ _______________
2 1
1 2
1 1
1 1
2 1
1 2
1 1
2 3
3 2
Sodium oxide
Beryllium chloride
Potassium bromide
Calcium sulfide
Lithium oxide
Magnesium fluoride
Rubidium iodide
Aluminum sulfide
Strontium nitride
Properties of Ionic Compounds -when ionic compounds form, they form a _____________, a _________________________ arrangement of _______ and ________ ionsNa
Cl
Na
Na
NaNa
Cl Cl
Cl
Cl
Na
Na
NaNa Na
NaNa
Na Na
Na Na
-the energy required to separate _______ (6.02 x 1023) of ions from each other is called the ________________, the more ________ the lattice energy, the ______ the attraction between ions
-the strength of the attraction between ions affects the compound’s __________ _________
geometricthree-dimensionalcrystal lattice
negativepositive
one mole
lattice energynegative stronger
physicalproperties
Na
Properties of Ionic Compounds Compound Lattice Energy
LiF
LiCl
LiBr
LiI
NaF
NaCl
NaBr
NaI
KI
KBr
KCl
KF
-1032
-852
-815
-761
-926
-786
-752
-702
-813
-717
-689
-649
A. Lattice Energy
-gather data
Properties of Ionic Compounds
A. Lattice Energy
-1200
-1000
-800
-600
-400
-200
0
Li Na K
F
Cl
Br
I
-analyze data
Properties of Ionic Compounds
A. Lattice Energy -draw conclusions-the lattice energy is more negative in ionic compounds that have ____________________, because the ions are ___________________ to each other
smaller ionic radiimore strongly attracted
Compound Melting Point (°C) Boiling Point (°C)B. Melting and Boiling Points
Cal2
NaCl
CaCl2
NaBr
KBr
NaI
MgO
660
734
747
782
784
801
2852 3600
1413
1100
1600
1390
1435
1304-gather data
Properties of Ionic Compounds
B. Melting and Boiling Points -draw conclusions
-ionic compounds with higher lattice energies have _________melting and boiling points temps.
-smaller ions are more ________ attracted to each other, because the _______ is closer to the _______ _________, while ions with larger positive and negative charges are more ________ attracted to each other
higher
strongly
valencenucleus
electrons
strongly
C. Electrical Conductivity -to conduct electricity, charged particles must be _________________, so ionic compounds generally do not conduct electricity as a _____, but generally do as a ______ or when ______________ _______________
free to move
solidliquid dissolved in water
(electrolyte)
Properties of Ionic Compounds
D. Hardness -the ions in ionic compounds with _______________ lattice energies are more _________ attracted to each other, so they tend to be ________
more negativestronglyharder
For Review
1. Rank the following ionic compounds, in order, from most negative to least negative lattice energy: RbCl, RbF, RbBr, RbI
2. Rank the following ionic compounds, in order, from highest to lowest melting point temperature: NaCl, MgCl2, MgO
3. Rank the following ionic compounds, in order, from softest to hardest: Li2O, Li2S, Li2Te, Li2Se
4. Rank the following ionic compounds, in order, from ions most strongly to ions least strongly attracted to each other: MgF2, RbCl, CaF2, CaCl2, MgO
2. RbCl 3. RbBr 4. RbI1. RbF
1. MgO 2. MgCl2 3. NaCl
1. Li2Te 2. Li2Se 3. Li2S 4. Li2O
1. MgO 2. MgF2 3. CaF2 4. CaCl2 5. RbCl
Naming Ionic Compounds
1. MgF2 ___________________Magnesium fluoride
2. Rb2S ___________________
3. Ba(NO3)2 ___________________
4. (NH4)2Te ___________________
Rubidium sulfide
Ammonium telluride
Barium nitrate
5. (NH4)3PO4 ___________________
6. Na2SO4 ___________________
7. Cu3P ___________________________________
Ammonium phosphate
Sodium sulfate
Copper(I) phosphide or Cuprous phosphide
Iron(III) hydroxide or Ferric hydroxide
10. Sn(HCO3)4 __________________________________________
9. Cr2(CO3)3 _______________________________________
8. Fe(OH)3 ________________________________
Tin(IV) Hydrogen carbonate or Stannic bicarbonate
Chromium(III) carbonate or Chromic carbonate
Metallic Bonds -like ionic compounds, metals in their ______ state form ________ structures
-each metal atom contributes its _______ _________ to a ___________ _____ of electrons, which move freely throughout the solid
-without its ________ _________, each metal atom forms a _________ _______
-the attraction between the ________ _________ and the _____________ ___________ is called a _________ _____
solidlattice
valence electronsdelocalized sea
valence electronsmetal cation
metallic cationdelocalized electrons metallic
bond
Properties of Metals -influenced strongly by the strength of attraction between the _______ ________ and the number of ____________ ___________
metallic cationdelocalized electrons
A. Melting Point
Properties of Metals
-since it doesn’t matter where the _________ _______ are within the _______ __________ of the metal, the cations _______ _________ easily, while still remaining in ______ _______ with each other, so ________ _______ temperatures are relatively ____
-the _________ the attraction between ________ ________ and the ____ of ______________ __________, the ________ the melting point temperature, so ________ atoms tend to have _______ melting point temperatures.
metalliccations lattice structure
change positionclose contact
melting pointlow
stronger metalliccations sea delocalizedelectrons higher
smallerhigher
A. Melting Point
Properties of Metals Metallic Element Melting Point (°C)
Lithium
Sodium
Potassium
Rubidium
Cesium
Francium
Beryllium
Aluminum
Calcium
Strontium
Barium
Radium
180
98
64
39
29
27
1278
660
839
764
725
700
A. Melting Point
Properties of Metals
-________ _______ temperatures are _________ by increasing the number of ________ ________ contributed to the _____ of ______________ __________. ___________ __________ like _______ and _________ contribute their ______ ________ electrons as well as their __________ __________ to the ____ of ________________ __________, __________ the melting point temperature dramatically.
melting point increasedvalence electrons
sea delocalizedelectrons Transition elements
Copper Tungsten dorbital valenceelectrons sea delocalizedelectrons increasing
Metallic Element Melting Point (°C)
Copper
Tungsten
Iron
Chromium
Silver
1083
3410
1535
1857
962
Properties of Metals
B. Malleability & Ductility -because particles in a metal can easily change position, they are __________, or can be __________ _____ _______ or other shapes easily
-because particles in a metal can easily change position, they are __________, or can be __________ _____ _______
malleablehammered into sheets
ductiledrawn into wires
C. Durability& Boiling Point -even though particles in a metal can easily change
position, they are __________ ____________, to the ____ of __________ surrounding them, and are __________ to _______ from the metal, giving them a high ___________ and a high ________ ______ temperature as well
strongly attractedsea electrons
difficult removedurability boiling
point
Properties of Metals
D. Conductivity -because __________ __________ in a metal are _____ ___ _____ while keeping _________ ______ intact, the __________ move _____ from place to place easily, so metal are _____ ___________ of _____
delocalized electronsfree to move metallicbonds electrons heat
goodconductors heat
-because __________ __________ in a metal are _____ ___ _____, they move easily as a part of an ________ ________ when an __________ __________ or ________ is applied to the metal, and the ________ ________ structure of the __________ ________ allows the __________ to flow without _________ with the ________, which allows for little __________
delocalized electronsfree to move
electrical current electricalpotential voltage
crystal latticemetallic cations electrons
colliding cationsresistance
Properties of Metals
E. Luster -because ____________ ___________ are free to move, they can interact with ______, __________ and __________ ________ of _______, giving metals their _______ ________
delocalized electronslight absorbing
releasing photons lightluster (shine)
F. Hardness& Strength -as the number of ___________ __________
contributed to the ____ of _________ increases, the strength of the _________ _____ increases, so metals such as _______, which contribute ____ ________, are relatively _____ and _____, while metals that contribute their outer __ electrons plus their inner __ electrons such as _________, _____, or _______ are relatively _____ and _______
delocalized electronssea electrons
metallic bondsSodium one electron
soft weaks d
Chromium NickelIronhard strong
Metal Alloys -because it doesn’t matter what _________ the _________ ________ are in in a metal, it is easy to introduce other _________ __________ into the ________ structure of a metal, creating an ______, or ________ of metals
position metalliccationsmetallic cations lattice
alloy mixture
-in ______________ _______, atoms of one kind of metal, like _______, are replaced with atoms of another kind of metal, like _______, to form an ______ like ________ _______, which has the properties of both metals. Pure _____ is beautiful, rare, and almost completely _________, and so is highly valuable, but it is too _____ to be of much use by itself, so it is ________ with ________ and ______ to make _________ or _________ _____, which is still beautiful, but much _______ and _________
substitutional alloysSilver
Copper alloy SterlingSilverGold unreactive
softalloyed Silver Copper
10 carat 14 carat Goldharder durable
-in ______________ _______, atoms of another kind of element, like _______, are inserted into the spaces in between the cations of a metal like _____ to form _______ ______, which is _______, ________, and less ________ than _____
interstitial alloysCarbon
Iron Carbonsteel harder stronger ductile
Iron
