CHAPTER 4 VOCABULARY SUBATOMIC PARTICLES BOHR DIAGRAM SHELLS (ORBITS) ATOMIC NUMBER IONIC COMPOUND COVALENT COMPOUND
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1 CHAPTER 4 VOCABULARY VOCABULARY WORD VOCABULARY WORD SUBATOMIC PARTICLES SHELLS (ORBITS) ATOMIC NUMBER ATOMIC MASS (Mass Number) POSITIVE ION NEGATIVE ION IONIC CHARGE BOHR DIAGRAM IONIC COMPOUND COVALENT COMPOUND LEWIS DIAGRAM VALENCE SHELL VALENCE ELECTRONS PDF processed with CutePDF evaluation edition
2 DEVELOPMENT OF ATOMIC THEORY (Quick Summary)
3 John Dalton Proposed first Atomic Theory
4 Michael Faraday showed that atoms could gain electric charges
5 J.J. Thompson The Dalton s atomic theory was revised to include his ideas:
6 Ernest Rutherford In 1911, Rutherford proposed his nuclear model of the atom
7 THE MODERN VIEW OF THE ATOM Nucleus = protons + neutrons
8 THE MODERN VIEW OF THE ATOM It is composed of electrons, protons and neutrons ELECTRONS: Orbit (move around) the nucleus Charge of -1 (negative) Symbol is e They can be shared or transferred between the atoms
9 THE MODERN VIEW OF THE ATOM It is composed of electrons, protons and neutrons PROTONS: In the nucleus Charge of +1 (positive) Symbol is p They CAN T be shared or transferred between the atoms = they are locked in the nucleus
10 THE MODERN VIEW OF THE ATOM It is composed of electrons, protons and neutrons NEUTRONS: In the nucleus Charge of 0 (no charge) Symbol is n They CAN T be shared or transferred between the atoms = they are locked in the nucleus
11 THE MODERN VIEW OF THE ATOM The relative size of the nucleus and atom!
12 Inside the Atom
13 Niels Bohr He studied gaseous samples of atoms, which were made to glow by passing an electric current through them.
14 Niels Bohr He used this property of elements, as well as discoveries by other scientists of the time, to solve the problems with Rutherford s model of the atom.
15 Niels Bohr showed how electrons are arranged in an atom = A BOHR MODEL DIAGRAM
16 Based on his observations, Bohr proposed that electrons surround the nucleus ONLY in specific energy levels or shells. Each energy level or shell has only certain amount of energy!
17 Think of these electron shells as stairs The electrons can only move from shell to shell (stair to stairs)
18 Think of these electron shells as stairs The electrons can only move from shell to shell (stair to stairs)
19 Think of these electron shells as stairs The electrons can only move from shell to shell (stair to stairs)
20 Think of these electron shells as stairs The electrons can only move from shell to shell (stair to stairs)
21 Think of these electron shells as stairs The electrons can only move from shell to shell (stair to stairs) = you can never find them between the shells (between the stairs)
22 Think of these electron shells as stairs The electron in the closest shell to the nucleus have the LOWEST energy = It is on the lowest step of the stairwell
23 Think of these electron shells as stairs The electrons in the furtermost shell to the nucleus have the HIGHEST energy = It is on the highest step of the stairwell
24 So the electrons closer to the nucleus have less energy than the electrons further from the nucleus
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26 1. Which electron has higher energy? 2. If the blue electron wanted to reach the shell in which the red electron is, would the light be given off or not?
27 1. Which electron has higher energy? 2. If the blue electron wanted to reach the shell in which the red electron is, would the light be given off or not?
28 1. Which electron has higher energy? 2. If the blue electron wanted to reach the shell in which the red electron is, would the light be given off or not?
29 The Number of Shells for an Element Each shell can hold ONLY certain number of electrons First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 18 electrons
30 The Number of Shells for an Element The number of shells (orbits) in an atom depends on the number of electrons in that atom First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 18 electrons
31 The Number of Shells for an Element For example, an element with six electrons has two electrons in the first shell and four electrons in the second shell First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 18 electrons
32 Drawing electrons The Bohr Model of the Atom Draw 3 electrons Draw 11 electrons Draw 14 electrons Draw 20 electrons
33 Organization of The Periodic Table of Elements
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35 1. Metals 2.Non-metals 3. Metalloids
36 GROUPS or FAMILIES 1 18
37 PERIODS or ROWS (1 7)
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39 SOME GROUPS OF THE PERIODIC TABLE
40 THE ACTUAL THE PERIODIC TABLE
41 The Periodic Table a chart that organizes the elements according to their physical and chemical properties. gives each element s name, symbol, atomic number, atomic mass, and ion charge(s)
42 Atomic Number the number of protons in the nucleus or the number of electrons (in a neutral atom)of each atom of an element What is the ATOMIC NUMBER of potassium?
43 What is the pattern of ATOMIC NUMBERS in the Periodic Table? INCREASING
44 Atomic Mass the average mass of an atom of an element Atomic mass # of protons + # of neutrons Always written as a decimal number and measured in amu (atomic mass units) What is the ATOMIC MASS of potassium?
45 What is the pattern of ATOMIC MASSES in the Periodic Table? INCREASING
46 QUICK REVIEW ATOMIC NUMBER = # of protons (or # of electrons) ATOMIC MASS NUMBER = # of protons + # of neutrons # of neutrons = MASS NUMBER ATOMIC NUMBER
47 Standard Atomic Notation Elements are written to show the Atomic Mass Number and the Atomic Number
48 Determine the number of protons, neutrons, and electrons present in potassium 39. Write the symbol for this element using standard atomic notation. potassium - 39 # of protons = Atomic Number = Atomic Mass Number = # of protons + # of neutrons = # of neutrons = Atomic Mass Number Atomic Number = # of electrons (in NEUTRAL ATOM) = # of protons =
49 Determine the number of protons, neutrons, and electrons present in each of the atoms. Write a symbol for each element using Standard Atomic Notation. # of protons: # of protons: # of protons: # of electrons: # of electrons: # of electrons: # of neutrons: # of neutrons: # of neutrons: Standard Atomic Notation: Standard Atomic Notation: Standard Atomic Notation:
50 Determine the number of protons, neutrons, and electrons present in each of the atoms. Write a symbol for each element using Standard Atomic Notation.
51 Determine the number of protons, neutrons, and electrons present in each of the atoms. Write a symbol for each element using Standard Atomic Notation. # of protons: # of protons: # of protons: # of electrons: # of electrons: # of electrons: # of neutrons: # of neutrons: # of neutrons: Standard Atomic Notation: Standard Atomic Notation: Standard Atomic Notation:
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54 A NEUTRAL ATOM Has the same number of protons and electrons Because the electrical charges on protons and electrons cancel each other, the overall charge is zero How many electron(s)? How many protons? OVERAL charge?
55 NEUTRAL ATOMS gain or lose electrons and become IONS A NEUTRAL ATOM Has the same number of protons and electrons Because the electrical charges on protons and electrons cancel each other, the overall charge is zero
56 NEUTRAL ATOMS gain or lose electrons and become IONS A NEUTRAL ATOM Has the same number of protons and electrons Because the electrical charges on protons and electrons cancel each other, the overall charge is zero
57 AN ION when a neutral atom gains or loses electrons The overall charge becomes either POSITIVE or NEGATIVE Potassium NEUTRAL ATOM Potassium ION Oxygen NEUTRAL ATOM Oxygen ION
58 Ion Charge an electric charge that forms on an atom when it gains or loses electrons POSITIVE CHARGE (+, 2+, 3+ ) atom loses electron(s) NEGATIVE CHARGE (-, 2-, 3- ) atom gains electron(s)
59 Ion Charge 1. Would potassium lose or gain electron(s)? 2. How many electron(s)? Potassium NEUTRAL ATOM Potassium ION
60 Ion Charge 1. Would oxygen lose or gain electron(s)? 2. How many electron(s)? Oxygen NEUTRAL ATOM Oxygen ION
61 AN ION - CATION POSITIVELY charged atom Loses an electron or electrons Metals form cations Potassium NEUTRAL ATOM Potassium ION
62 AN ION - ANION Negatively charged atom Gain an electron or electrons Non metals form anions Oxygen NEUTRAL ATOM Oxygen ION
63 Multiple Ion Charges Some elements have a multiple ion charge. These elements can form ions in more than one way.
64 QUICK CHECK 1. What is the atomic mass of this atom? 2. What is the atomic number of this atom? 3. What is (are) the possible ion charge(s) on this atom? 4. Would it gain or lose electrons? How many?
65 INCREASING REACTIVITY The Periodic Table Where are the following? Atomic number Period Group/Family Metals Non-metals Transition metals Metalloids Alkali metals Alkaline earth metals Halogens Noble gases
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70 BOHR DIAGRAMS
71 Niels Bohr showed how electrons are arranged in an atom = A BOHR MODEL DIAGRAM
72 The Number of Shells for an Element Each shell can hold ONLY certain number of electrons First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 18 electrons
73 Drawing electrons The Bohr Model of the Atom Draw 3 electrons Draw 11 electrons Draw 14 electrons Draw 20 electrons
74 BOHR DIAGRAMS There is a pattern to the arrangements of electrons in atoms Atoms have SHELLS of electrons around the nucleus
75 Drawing electrons The Bohr Model of the Atom Draw 3 electrons Draw 11 electrons Draw 14 electrons Draw 20 electrons
76 BOHR DIAGRAMS Now you know how to FIND the number of electrons in an atom and how to DRAW them
77 A BOHR MODEL DIAGRAM
78 Other BOHR MODEL DIAGRAMs Some diagrams show the electrons as dots. Others just have figures indicating the number of electrons in each shell.
79 BOHR DIAGRAMS Practice (worksheet) First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 8 electrons Draw Bohr Diagrams for: hydrogen sodium phosphorus neon calcium
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81 A Bohr Diagram for An Ion When a neutral atom gains or loses electrons NEUTRAL ATOM How many electron(s)? How many protons? OVERAL charge? ION How many electron(s)? How many protons? OVERAL charge?
82 Bohr Diagrams for Ions When a neutral atom gains or loses electrons NEUTRAL ATOM How many electron(s)? How many protons? OVERAL charge? ION How many electron(s)? How many protons? OVERAL charge?
83 BOHR DIAGRAMS for IONS Practice First shell: 2 electrons Second shell: 8 electrons Third shell: 8 electrons Fourth shell: 8 electrons Draw Bohr Diagrams for: sodium ion phosphorus ion neon ion calcium ion
84 BOHR DIAGRAMS Quick Review NEUTRAL ATOM How many electron(s)? How many protons? OVERAL charge? ION How many electron(s)? How many protons? OVERAL charge?
85 Patterns of Electron Arrangement in Groups If there are 8 electrons in the very last shell = STABLE OCTET 1 exception = HELIUM (2 electrons for STABLE OCTET) Which group has a STABLE OCTET in its outer most shell?
86 ATOMS WANT TO HAVE A STABLE OCTET!!!!!! ALL THE TIME!! If there are 8 electrons in a shell = STABLE OCTET All ATOMS want to be like NOBLE GASES!
87 Valence Shell = OUTERMOST SHELL
88 VALENCE ELECTRONS Electrons in the VALENCE SHELL are called VALENCE ELECTRONS
89 How many VALENCE ELECTRONS in GROUP 1?
90 How many VALENCE ELECTRONS in GROUP 2?
91 How many VALENCE ELECTRONS in GROUP 16?
92 How many VALENCE ELECTRONS in GROUP 18?
93 What Do You Notice about the Number of Valence Electrons for Elements in the Same Group? Elements in the same group have the same number of valence electrons
94 What Do You Notice About the Placement and the Number of Valence Electrons for Elements in the Same Period? Elements in the same period have valence electrons in the same shell AND the number of valence electrons is increasing going left to right within the group by one
95 What Do You Notice About the period number and the number of occupied shells for Elements in the Same Period? The period number indicates the number of shells that have electrons.
96 ATOMS WANT TO HAVE A STABLE OCTET!!!!!! ALL THE TIME!! If there are 8 electrons in a shell = STABLE OCTET All ATOMS want to be like NOBLE GASES!
97 Unreactive because their atoms have filled valence shells = they are stable = NOBLE GAS STABILITY UNREACTIVE = they DO NOT lose or gain electrons NOBLE GASES!
98 Each atom wants to have as many valence electrons as the nearest noble gas. Metals want to LOSE ELECTRONS
99 Why Do Atoms Become Ions? Atoms WILL gain or lose electrons because they want to be as stable as the NEAEREST NOBLE GAS
100 Each atom wants to have as many valence electrons as the nearest noble gas. Non - Metals want to GAIN ELECTRONS
101 Each atom element to have as many of valence electrons as the nearest noble gas. How many electrons does sodium, Na, want to have? 10 electrons
102 Each atom element to have as many of valence electrons as the nearest noble gas. 10 electrons How many electrons does oxygen, O, want to have?
103 Why Do Atoms Become Ions? Atoms WILL gain or lose electrons because they want to be as stable as the NEAEREST NOBLE GAS Ions have the same electron arrangement as the nearest noble gas
104 Bohr Diagrams Worksheet 1. How many protons does this element have? 2. How many electrons does this element have? 3. How many valence shells does this element have? 4. How many valence electrons does this element have? 5. How many occupied shells does this element have? 6. What is the identity of this element?
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111 LEWIS DIAGRAMS
112 LEWIS DIAGRAMS Show only an atom s valence electrons and the chemical symbol.
113 Rules for Drawing Lewis Diagrams Dots representing valence electrons are placed around the element symbols
114 Rules for Drawing Lewis Diagrams Electron dots are placed singly ( o clock) until the fifth electron is reached. Then they are paired up.
115 LEWIS DIAGRAMS Show only an atom s valence electrons and the chemical symbol. How many VALENCE ELECTRONS for chlorine?
116 LEWIS DIAGRAMS How many VALENCE ELECTRONS for potassium?
117 LEWIS DIAGRAMS How many VALENCE ELECTRONS for sodium?
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120 LEWIS DIAGRAMS Show only an atom s valence electrons and the chemical symbol.
121 MOLECULES and IONIC COMPOUNDS Atoms combine with different atoms to form compounds (thanks to electrons) SHARING ELECTRONS Covalent Compounds DONATING/ACCEPTING ELECTRONS Ionic Compounds Molecules
122 MOLECULES and IONIC COMPOUNDS Forces that hold atoms together are called CHEMICAL BONDS These bonds arise when VALENCE ELECTRONS interact Each atom attempts to have as many of valence electrons as the nearest noble gas.
123 IONS Atom or a group of atoms with net negative or positive charge POSITIVELY CHARGED ION = CATION NEGATIVELY CHARGED ION = ANION
124 IONIC COMPOUNDS Formed by an attraction of positively charged ion (cation) and negatively charged ion (anion) Chemical formula
125 IONIC COMPOUNDS Formed when an electron(s) are transferred from a metal to a non - metal Chemical formula
126 IONIC COMPOUNDS Cations and Anions are attracted to each other IONIC BONDING
127 Draw the BOHR MODEL DIAGRAM for NaCl
128 Draw the BOHR MODEL DIAGRAM for NaCl
129 Draw the BOHR MODEL DIAGRAM for NaCl
130 Draw the BOHR MODEL DIAGRAM for KF
131 Draw the BOHR MODEL DIAGRAM for CaF
132 Lewis Diagrams of IONS and IONIC BONDS For positive ions, one electron dot is removed from the valence shell for each positive charge. For negative ions, one electron dot is added to each valence shell for each negative charge. Square brackets are placed around each ion to indicate transfer of electrons.
133 Draw the LEWIS DIAGRAM for MgO
134 Covalent Compounds - MOLECULES Valence Electrons are shared between atoms
135 Covalent Compounds - MOLECULES Valence Electrons are shared between atoms + hydrogen fluorine electrons are shared hydrogen fluoride
136 Lewis Diagrams of COVALENT COMPOUNDS Like Bohr diagrams, valence electrons are drawn to show sharing of electrons. The shared pairs of electrons are usually drawn as a straight lineare placed around each ion to indicate sharing of electrons.
137 Lewis Diagrams of COVALENT COMPOUNDS LONE pair of electrons BONDING pair of electrons
138 Lewis Diagrams of COVALENT COMPOUNDS Draw Lewis diagram for compounds of Water (2H and O) Ammonia (N and 3H) Methane (C and 4H)
139 Lewis Diagrams of COVALENT COMPOUNDS
140 Lewis Diagrams of COVALENT COMPOUNDS Draw Lewis diagram for diatomic molecules of F 2, O 2, N 2 Valence electrons are shared Several non-metals join to form diatomic molecules.
141 Lewis Diagrams of COVALENT COMPOUNDS Draw LEWIS STRUCTURE of O 2 O O O O O O DOUBLE BOND
142 Lewis Diagrams of COVALENT COMPOUNDS Draw LEWIS STRUCTURE of N 2 N N N N N N TRIPLE BOND
143 Lewis Diagrams of COVALENT COMPOUNDS Draw LEWIS STRUCTURE of CO 2 C O O O O C C O O
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