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**Chapter 1 Structure Determines Properties**

Dr. Wolf's CHM 201 & 202 5

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**1.1 Atoms, Electrons, and Orbitals**

Dr. Wolf's CHM 201 & 202 5

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**• Atoms are composed of Protons positively charged +**

mass = X kg Neutrons neutral mass = X kg Electrons negatively charged mass = X kg + • – Dr. Wolf's CHM 201 & 202 3

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**Atomic Number and Mass Number**

X Z A Atomic number (Z) = number of protons in nucleus (this must also equal the number of electrons in neutral atom) Mass number (A) = sum of number of protons + neutrons in nucleus Dr. Wolf's CHM 201 & 202 10

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Schrödinger Equation Schrödinger combined the idea that an electron has wave properties with classical equations of wave motion to give a wave equation for the energy of an electron in an atom. Wave equation (Schrödinger equation) gives a series of solutions called wave functions ( ). Dr. Wolf's CHM 201 & 202 5

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**Only certain values of are allowed. **

Wave Functions Only certain values of are allowed. Each corresponds to a certain energy. The probability of finding an electron at a particular point with respect to the nucleus is given by 2. Each energy state corresponds to an orbital. Dr. Wolf's CHM 201 & 202 6

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**Figure 1.1 Probability distribution ( 2) for an electron in a 1s orbital.**

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**Figure 1.2 Boundary surfaces of a 1s orbital and a 2s orbital.**

A boundary surface encloses the region where the probability of finding an electron is high—on the order of 90-95% 1s 2s Figure 1.2 Boundary surfaces of a 1s orbital and a 2s orbital. Dr. Wolf's CHM 201 & 202 7

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**Each orbital is characterized by a unique set of four quantum numbers. **

The principal quantum number (n) is a whole number (integer, 1, 2, etc.) that specifies the shell and is related to the energy of the orbital. The angular momentum quantum number (l) is usually designated by a letter (s, p, d, f, etc) and describes the shape of the orbital. Values for l range from 0 to (n-1) Dr. Wolf's CHM 201 & 202 9

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**Each orbital is characterized by a unique set of four quantum numbers. **

The magnetic quantum number m is a whole number ranging from –l through 0 to +l. This gives the orientation of the orbital. The spin quantum number is either + or - ½ for the electron spin clockwise or counter clockwise Dr. Wolf's CHM 201 & 202 9

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**s Orbitals are spherically symmetric. **

The energy of an s orbital increases with the number of nodal surfaces it has. A nodal surface is a region where the probability of finding an electron is zero. A 1s orbital has no nodes; a 2s orbital has one; a 3s orbital has two, etc. Dr. Wolf's CHM 201 & 202 9

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**The Pauli Exclusion Principle**

No two electrons in the same atom can have the same set of four quantum numbers. Two electrons can occupy the same orbital only when they have opposite spins. There is a maximum of two electrons per orbital. Dr. Wolf's CHM 201 & 202 3

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**Principal quantum number (n) = 1**

First Period Principal quantum number (n) = 1 Hydrogen Helium Z = 1 Z = 2 1s 1 1s 2 1s 2s 2p H He Dr. Wolf's CHM 201 & 202 5

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**p Orbitals are shaped like dumbells. Are not possible for n = 1. **

Are possible for n = 2 and higher. Dr. Wolf's CHM 201 & 202 9

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**p Orbitals are shaped like dumbells. Are not possible for n = 1. **

Are possible for n = 2 and higher. There are three p orbitals for each value of n (when n is greater than 1). Dr. Wolf's CHM 201 & 202 9

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**p Orbitals are shaped like dumbells. Are not possible for n = 1. **

Are possible for n = 2 and higher. There are three p orbitals for each value of n (when n is greater than 1). Dr. Wolf's CHM 201 & 202 9

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**p Orbitals are shaped like dumbells. Are not possible for n = 1. **

Are possible for n = 2 and higher. There are three p orbitals for each value of n (when n is greater than 1). Dr. Wolf's CHM 201 & 202 9

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**Principal quantum number (n) = 2**

Second Period Principal quantum number (n) = 2 1s 2s 2p Be 4 B 5 C 6 Li 3 Z Dr. Wolf's CHM 201 & 202 9

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Second Period 1s 2s 2p O 8 F 9 Ne 10 N 7 Z Dr. Wolf's CHM 201 & 202 10

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1.2 Ionic Bonds Dr. Wolf's CHM 201 & 202 5

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Ionic Bonding An ionic bond is the force of electrostatic attraction between oppositely charged ions Cl– (anion) Na+ (cation) Dr. Wolf's CHM 201 & 202 6

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Ionic Bonding Ionic bonds are common in inorganic chemistry but rare in organic chemistry. Carbon shows less of a tendency to form cations than metals do, and less of a tendency to form anions than nonmetals. Dr. Wolf's CHM 201 & 202 7

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**1.3 Covalent Bonds and the Octet Rule**

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**The Lewis Model of Chemical Bonding**

In 1916 G. N. Lewis proposed that atoms combine in order to achieve a more stable electron configuration. Maximum stability results when an atom is isoelectronic with a noble gas. An electron pair that is shared between two atoms constitutes a covalent bond. Dr. Wolf's CHM 201 & 202 2

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**Two hydrogen atoms, each with 1 electron,**

Covalent Bonding in H2 Two hydrogen atoms, each with 1 electron, H . can share those electrons in a covalent bond. H : Sharing the electron pair gives each hydrogen an electron configuration analogous to helium. Dr. Wolf's CHM 201 & 202 2

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**Two fluorine atoms, each with 7 valence electrons, .. .. F . :**

Covalent Bonding in F2 Two fluorine atoms, each with 7 valence electrons, .. .. F . : can share those electrons in a covalent bond. F : .. Sharing the electron pair gives each fluorine an electron configuration analogous to neon. Dr. Wolf's CHM 201 & 202 2

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The Octet Rule In forming compounds, atoms gain, lose, or share electrons to give a stable electron configuration characterized by 8 valence electrons. F : .. The octet rule is the most useful in cases involving covalent bonds to C, N, O, and F. Dr. Wolf's CHM 201 & 202 2

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**to write a Lewis structure for CF4.**

Example Combine carbon (4 valence electrons) and four fluorines (7 valence electrons each) C . F : .. . to write a Lewis structure for CF4. : F .. C The octet rule is satisfied for carbon and each fluorine. Dr. Wolf's CHM 201 & 202 4

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Example It is common practice to represent a covalent bond by a line. We can rewrite : F .. C .. C F .. : as Dr. Wolf's CHM 201 & 202 4

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**1.4 Double Bonds and Triple Bonds**

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**Inorganic Examples C : O .. C : O .. Carbon dioxide : N C H : N C H**

Hydrogen cyanide Dr. Wolf's CHM 201 & 202 10

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**Organic Examples C H C : .. H Ethylene : C H Acetylene C H 10**

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**1.5 Polar Covalent Bonds and Electronegativity**

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**An electronegative element attracts electrons. **

Electronegativity Electronegativity is a measure of the ability of an element to attract electrons toward itself when bonded to another element. An electronegative element attracts electrons. An electropositive element releases electrons. Dr. Wolf's CHM 201 & 202 2

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**Pauling Electronegativity Scale**

Electronegativity increases from left to right in the periodic table. Electronegativity decreases going down a group. Dr. Wolf's CHM 201 & 202 5

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**nonpolar bonds connect atoms of the same electronegativity**

Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. F : .. H—H : N nonpolar bonds connect atoms of the same electronegativity Dr. Wolf's CHM 201 & 202 7

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**polar bonds connect atoms of different electronegativity**

Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. O .. H F : .. H : O C O : .. .. polar bonds connect atoms of different electronegativity Dr. Wolf's CHM 201 & 202 7

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**Electrostatic Potential Maps**

Electrostatic potential maps show the charge distribution within a molecule. F : .. H Solid surface Red is negative charge; blue is positive. Dr. Wolf's CHM 201 & 202 7

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**Electrostatic Potential Maps**

Electrostatic potential maps show the charge distribution within a molecule. F : .. H Transparent surface Red is negative charge; blue is positive. Dr. Wolf's CHM 201 & 202 7

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**Electrostatic Potential Maps**

Electrostatic potential maps show the charge distribution within a molecule. F : .. H - + H Li Red is negative charge; blue is positive. Dr. Wolf's CHM 201 & 202 7

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1.6 Formal Charge Formal charge is the charge calculated for an atom in a Lewis structure on the basis of an equal sharing of bonded electron pairs. Dr. Wolf's CHM 201 & 202 5

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**Nitric acid Formal charge of H : .. H O N ..**

We will calculate the formal charge for each atom in this Lewis structure. Dr. Wolf's CHM 201 & 202 19

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**Hydrogen shares 2 electrons with oxygen. **

Nitric acid Formal charge of H : .. H O N .. Hydrogen shares 2 electrons with oxygen. Assign 1 electron to H and 1 to O. A neutral hydrogen atom has 1 electron. Therefore, the formal charge of H in nitric acid is 0. Dr. Wolf's CHM 201 & 202 19

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**Oxygen has 4 electrons in covalent bonds. **

Nitric acid Formal charge of O : .. H O N .. Oxygen has 4 electrons in covalent bonds. Assign 2 of these 4 electrons to O. Oxygen has 2 unshared pairs. Assign all 4 of these electrons to O. Therefore, the total number of electrons assigned to O is = 6. Dr. Wolf's CHM 201 & 202 19

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**A neutral oxygen has 6 electrons. **

Nitric acid Formal charge of O : .. H O N .. Electron count of O is 6. A neutral oxygen has 6 electrons. Therefore, the formal charge of O is 0. Dr. Wolf's CHM 201 & 202 19

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**A neutral oxygen has 6 electrons. **

Nitric acid Formal charge of O : .. H O N .. Electron count of O is 6 (4 electrons from unshared pairs + half of 4 bonded electrons). A neutral oxygen has 6 electrons. Therefore, the formal charge of O is 0. Dr. Wolf's CHM 201 & 202 19

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**A neutral oxygen has 6 electrons. **

Nitric acid Formal charge of O : .. H O N .. Electron count of O is 7 (6 electrons from unshared pairs + half of 2 bonded electrons). A neutral oxygen has 6 electrons. Therefore, the formal charge of O is -1. Dr. Wolf's CHM 201 & 202 19

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**Electron count of N is 4 (half of 8 electrons in covalent bonds). **

Nitric acid Formal charge of N : .. H O N – .. Electron count of N is 4 (half of 8 electrons in covalent bonds). A neutral nitrogen has 5 electrons. Therefore, the formal charge of N is +1. Dr. Wolf's CHM 201 & 202 19

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**Nitric acid Formal charges : .. H O N + – ..**

A Lewis structure is not complete unless formal charges (if any) are shown. Dr. Wolf's CHM 201 & 202 19

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**An arithmetic formula for calculating formal charge.**

group number in periodic table number of bonds number of unshared electrons – – Dr. Wolf's CHM 201 & 202 16

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**"Electron counts" and formal charges in NH4+ and BF4-**

.. B F : 1 4 N H + 7 – 4 Dr. Wolf's CHM 201 & 202 17

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