Download presentation
Presentation is loading. Please wait.
1
SAME AS YESTERDAY = Hints for your lab data:
Question of the Day SAME AS YESTERDAY = Hints for your lab data: every solution should form one precipitate (either with A or B 3 of your solutions should turn pink with the addition of C 6 of your precipitates should dissolve with the addition of D Postlabs (both parts) due by the end of class today!!!
2
Goal for next time = ___% if you made your goal must improve by 1
Goal Setting Day Unit 5 Test = ___% I studied by … Goal for next time = ___% if you made your goal must improve by 1 Next time I will study by…
3
How do you know how many valence electrons an atom has?
Review How do you know how many valence electrons an atom has?
4
How do elements combine to form compounds?
Objective How do elements combine to form compounds?
5
Lewis Dot Structures Notation used to show an abbreviated version of an elements valence electron arrangement H F O
6
H F O Lewis Dot Structures
Notation used to show an abbreviated version of an elements valence electron arrangement H F First determine number of valence electrons. Valence electrons are represented with dots around the element’s symbol. O
7
H F O Lewis Dot Structures
Notation used to show an abbreviated version of an elements valence electron arrangement H F 2 e-s. can fit per side (you can think of each side of the symbol as an orbital) O
8
In order to bond an element must be able to give AND take an electron.
Lewis Dot Structures H In order to bond an element must be able to give AND take an electron. F O
9
Lewis Dot Structures In order for a bond to form an atom must be able to “give” an electron and “take one” F H Both can bond once
10
Na P Al F Lewis Dot Structures Examples: Sodium = can bond ____
Phosphorous = can bond ____ Aluminum = can bond ____ Fluorine = can bond ____ Na P Al F
11
Lewis Dot Structures
12
Lewis Dot Structures
13
Lewis Dot Structures Suggested Steps: 1. Do each individual Lewis dot structure and determine how many times each element can bond 2. Look for ways to make everyone happy 3. Lewis dot structure must match formula!!!
14
Lewis Dot Structures B. Practice: potassium and fluorine bond
magnesium and chlorine bond lithium and oxygen bond hydrogen and oxygen bond
15
Q of the Day The halogens all have __ valence which means they all want to ______________. Day 7 gain one electron
16
How do elements combine to form compounds?
Objective How do elements combine to form compounds?
17
Electrostatic Force – an interaction between charged particles
Ionic Bonding Electrostatic Force – an interaction between charged particles 33 Opposites – Like charges – Attract Repel 17
18
Valence electrons dictate reactivity!
Bonding Introduction What happens when atoms collide? Valence electrons interact. Valence electrons dictate reactivity!
19
Opposites Attract!!! Bonding Introduction Holding it all together
Chemical bond – A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds them together … electrostatic force Nuclei = _______________ charge positive Electrons = _______________ charge negative Opposites Attract!!!
20
Bonding Introduction But Why Bond at all? Atoms want a full set of valence electrons (8) and they can share (bond) to get them!!! ~ octet rule
21
Br Why bonds and ions? Achieving electrical and energetic stability.
Bonding Introduction Why bonds and ions? Achieving electrical and energetic stability. Electron pairs – stable - Good Lone electrons – high potential energy - BAD Br
22
3 main bond types: Ionic Polar covalent Nonpolar covalent
Bonding Introduction 3 main bond types: Ionic Polar covalent Nonpolar covalent
23
Electrostatic Force – an interaction between charged particles
Ionic Bonding Electrostatic Force – an interaction between charged particles 33 Opposites – Like charges – Attract Repel 23
24
Ions – charged particles
Ionic Bonding Ions – charged particles Cation – positive ion Anion – negative ion
25
Ionic Bonding Collision – Ions (-) Br Li BANG Br (+) Li
26
But they don’t separate … WHY?
Ionic Bonding But they don’t separate … WHY? + - Li Br Li Electrostatic Force BANG Br
27
Ionic Bonding Ionic bonds – Chemical bonds that result from the electrical attraction between large numbers of cations and anions Cation – ? Anion – ?
28
Electronegativity – measure of atom’s ability to attract electrons
Ionic Bonding Atoms Only transfer elecs. (form ions) when one atom has a very strong attraction for elecs. (wants them a lot more) Electronegativity Electronegativity – measure of atom’s ability to attract electrons
29
Ionic bonds most commonly form between metals and nonmetals!
Ionic Bonding Electronegativity P. T. (page 181) Ionic bonds most commonly form between metals and nonmetals!
30
Ionic bonds are made up of charged pieces (ions)
Ionic Bonding Ionic bonds are made up of charged pieces (ions) Ions can be made up of one element or a combination of elements (polyatomic ions)
31
high melting points – strong bonds
Ionic Bonding Ionic Compounds: high melting points – strong bonds Brittle dissolve in water to produce mobile ions – good conductors
32
READ section 7.1 and complete #s 1-8 on page 199 Due Monday 3-30
Assignment READ section 7.1 and complete #s 1-8 on page 199 Due Monday 3-30 BINDERS!!! Quarterly Exam = Tuesday 3-31 33 32
33
Draw the Lewis dot structure for chlorine.
Question of the Day Draw the Lewis dot structure for chlorine. Day 2. Draw the Lewis dot structure for oxygen – use your notes packet if needed.
34
2. Is this an ionic compound? Explain!
Question of the Day Day Draw the Lewis dot for the compound that forms when sodium and oxygen bond. 2. Is this an ionic compound? Explain!
35
READ section 7.1 and complete #s 1-8 on page 199 Due Monday 3-30
Assignment READ section 7.1 and complete #s 1-8 on page 199 Due Monday 3-30 BINDERS!!! Quarterly Exam = Tuesday 3-31 33 35
36
Electrostatic Force – an interaction between charged particles
Ionic Bonding Electrostatic Force – an interaction between charged particles 33 Opposites – Like charges – Attract Repel 36
37
L A B Electrostatic Forces 33
Similar presentations
© 2025 SlidePlayer.com. Inc.
All rights reserved.