welcome b ack from spring break! week 12: monday do now
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Welcome b ack from spring break! Week 12: Monday Do Now. Name one place that you would like to travel to. Why do you want to go there?. Corrections to PT Trends Quiz. In a different color pen make corrections to your quiz. If you finish early, help a classmate - PowerPoint PPT PresentationTRANSCRIPT
Welcome back from spring break!
Week 12: Monday Do Now
1. Name one place that you would like to travel to.
2. Why do you want to go there?
In a different color pen make corrections to your quiz.
If you finish early, help a classmate
Once you are done, place your quiz in your Test Folder
Corrections to PT Trends Quiz
• Elements are determined by their atomic number
• Atomic number = Number of protons• Atomic number does not change,
therefore the number of protons will not change
Elements
• In a neutral atom…Number of protons = Number of electrons
• However, in an ion, the number of electrons will change
Elements
• An ion is an atom or molecule that has gained or lost at least one electron• If an atom gains an electron, it will have a
negative charge• If an atom loses an electron, it will have a
positive charge• Why?
Ions
• Ions with a positive charge are called cations • Atom will have more protons
Positive ions
+++++++++
• Ions with a negative charge are called anions• Atom will have more electrons
Negative ions
-- -- -- -- --
Lithium with a +1 charge = Li +1
Fluorine with a -1 charge = F -1
Examples of Ions
Normally, Lithium has 3 electrons
3 negative electrons -33 positive protons +3(-3) + (+3) = 0
Example A
Lithium with a +1 charge = Li +1
Li +1 has lost an electron2 negative electrons -23 positive protons +3(-2) + (+3) = +1
Example A
Normally, Fluorine has 9 electrons
9 negative electrons -99 positive protons +9(-9) + (+9) = 0
Example B
Fluorine with a -1 charge = F -1
F -1 has gained an electron10 negative electrons -109 positive protons +9(-10) + (+9) = -1
Example B
Write the number of protons and electrons the element normally has and then determine the new number of protons and electrons given the charge of the ion
*Independent Practice*
Break: ChallengeVery reactive elements are often sealed “under Argon atmosphere” and not in normal air. Why
would they do this?
Valence ElectronsDefinition: the outermost electrons of an atom
Full Valence Electron Shell
What is a full shell?
• A full shell is 8 valence electrons• Elements are more stable with 8
valence electrons• Elements will gain or lose some
valence electrons in order to obtain 8 valence electrons
Elements want a full shell
• An element with less than 4 valence electrons will lose electrons.• This is why Alkali Metals (1 valence
electron) are the most reactive metals. They are very close to a “full” shell.
Elements want a full shell
• An element with more than 4 valence electrons will gain electrons.• This is why Halogens (7 valence
electrons ) are the most reactive non-metals. They are very close to a “full” shell.
“Full” Valence Electron Shell
Noble gases are“inert” or un-reactive
because their outer shell of valence electrons
is full with 8 electrons
Anion formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Chlorine 7 Gain 1 Cl - 1
Sulfur
Nitrogen
Anion formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Chlorine 7 Gain 1 Cl - 1
Sulfur 6 Gain 2 S - 2
Nitrogen
Anion formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Chlorine 7 Gain 1 Cl - 1
Sulfur 6 Gain 2 S - 2
Nitrogen 5 Gain 3 N - 3
Cation formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Sodium 1 Lose 1 Na +1
Calcium
Boron
Cation formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Sodium 1 Lose 1 Na +1
Calcium 2 Lose 2 Ca +2
Boron
Cation formation
Element # Valence Electrons
Gain or lose electrons?
Ion that will form
Sodium 1 Lose 1 Na +1
Calcium 2 Lose 2 Ca +2
Boron 3 Lose 3 B +3
Fill in chart Circle all cations
*Independent Practice*
Week 12: Monday Exit Ticket
Iodine has a negative 1 charge
1. Is Iodine an anion or a cation?2. Write how many electrons and
protons Iodine -1 would have.
*Monday Homework* Copy these elements down on a piece of paper. Make a chart like the independent practice and fill it out.
1. Lithium (Li)2. Beryllium (Be)
3. Iodine (I)4. Arsenic (As)5. Krypton (Kr)
Week 12: Tuesday Do Now
1. What is an ion?2. Classify the following as either
cations or anionsa. Bromine (Br)b. Potassium (K)c. Magnesium (Mg)d. Sulfur (S)
Electrolytes
• All ions carry an electric charge• Electrolytes are substances that become
ions in solution and acquire the ability to conduct electricity.
• They are present in the human body in a specific balance that is necessary for the function of our cells and organs
Electrolytes
Electrolytes
NaCl(s) → Na+(aq) + Cl−
(aq)
(Na+), (K+), (Ca2+), (Mg2+), (Cl−), (HPO4
2−), (HCO3−)
Page R5 in appendix ARead Electrolyte Balance in the Body and answer the following 5 questions
If you finish early, check out the Sodium-Potassium Pump on page R6
• Using the information you have just read, you will act as a doctor and answer several questions about your patients’ electrolyte balances
• Leave your book open to page R5, you will need to refer to Table 1B
Doctor Activity
• A patient comes in with a Na+ level of 180 mmol/L. What should you be worried about?
• Hypernatremia • Increased urine excretion (peeing too much).• What happens if you lose too much water?• Dehydration
You are the doctor
• A patient comes in with a K+ level of 2.0 What should you be worried about?
• Hypokalemia. Gastrointestinal conditions• What do you think gastrointestinal issues
are?• Gastro = stomach, Intestine = intestines.• Stomach and intestine problems: stomach
upset
You are the doctor
• A patient comes in with a Na+ level of 120. What should you be worried about?
• Hyponatremia. Vomiting, diarrhea• What do you think is a problem that
could come from vomiting and diarrhea?• Dehydration from water loss
You are the doctor
• A patient comes in with a K+ level of 6.0. What should you be worried about?
• Renal failure• What organ are we talking about when
we say “renal failure”• Kidneys
You are the doctor
Kidneys
Normal kidney Renal failure kidney
• A patient comes in with a Cl- level of 90. What should you be worried about?
• Hypochloremia: acute infection, burns.• What does the word acute mean?• Temporary
You are the doctor
• Record your answers in your notes
Take the sodium IQ quiz on page R7
Challenge Question:High pressure lamps (used along highways and in parking lots) contain the elements _____________ and ____________ in addition to sodium.
Break
Lewis Dot Diagrams
X Draw the chemical symbol Treat each side as a box that can
hold up to two electronsCount the valence electronsStart filling the boxes - don’t make
pairs unless you need to
Lewis Dot Diagram
O Oxygen has 6 electronsin its valence shell
Start putting them in the boxes.
Lewis Dot Diagram
This is the Lewissymbol for oxygen.
O
Lewis Dot Diagram
Li Be B C
Lewis diagrams of second period elements
Lewis Dot Diagram
Li Be B C
Lewis diagrams of second period elements
Draw Lewis Dot Diagrams for all elements givenYou should notice a pattern
*Independent Practice*
Week 12: Tuesday Exit Ticket
1. Define the term electrolyte2. Draw the Lewis Dot Diagram for
Sodium3. What do the dots in #2
represent?
Week 12: Wednesday Do Now
1. Draw the Lewis Dot Diagram for Fluorine (F)
2. Draw the Lewis Dot Diagram for Potassium (K)
White Board ActivityReview of Lewis Dot Diagrams
Boron (B)
Draw the Lewis Dot Diagram for…
Nitrogen (N)
Draw the Lewis Dot Diagram for…
Chlorine (Cl)
Draw the Lewis Dot Diagram for…
Magnesium
Draw the Lewis Dot Diagram for…
Neon
Draw the Lewis Dot Diagram for…
Bromine
Draw the Lewis Dot Diagram for…
Bromine -1
Draw the Lewis Dot Diagram for…
Lithium +1
Draw the Lewis Dot Diagram for…
Arsenic -3
Draw the Lewis Dot Diagram for…
The ion of Sodium
Draw the Lewis Dot Diagram for…
The ion of Iodine
Draw the Lewis Dot Diagram for…
The ion of Phosphorous
Draw the Lewis Dot Diagram for…
Please return all white boards & markers
Lewis Dot Structure & Bonding
Na + Cl
Which element is more electronegative?
Na + Cl Na Cl
Cl is more electronegative.
Therefore, Cl will steal an electron from Na.
Formation of NaCl
Na + Cl Na+ Cl -
Na becomes Na+1 the cationCl becomes Cl-1 the anionThe + and - charges attract each otherand form a bond
F + Li
Which element is more electronegative?
Which element is more electronegative?F is more electronegative.
Therefore, F will steal an electron from Li
F + Li F Li
F becomes F-1 the anionLi becomes Li+1 the cationThe + and - charges attract each otherand form a bond
F + Li F - Li+
Formation of LiF
Mg + O
Which element is more electronegative?
Mg + O Mg O
O is more electronegative.
Therefore, O will steal 2 electrons from Mg
Mg + O Mg+2 O -2
Mg becomes Mg+2 the cationCl becomes O-2 the anionThe + and - charges attract each other and form a bond
Break Challenge Question
Write out the electron configuration for the bromine ion Br -1
Independent Practice
Questions?Ask 3 other students before you ask Ms. McCullough
Week 12: Wednesday Exit Ticket
Draw the Lewis Dot Diagram for Sulfur (S) and Barium (Ba)
individually and then show how an ionic bond will form.
Week 12: Thursday Do Now
Draw the Lewis Dot Diagram for Sodium (Na) and Bromine (Br)
individually and then show how an ionic bond will form.
BondingKey Points
1. There are 3 types of bonds
• Ionic• Polar Covalent• Non-polar Covalent
2. The difference betweenionic and covalent bonds
• Ionic bonds:–One atom steals electrons from the
other atom• Covalent bonds:–Two atoms share electrons
3. The difference in electronegativity between the two atoms will determine the type of bond that forms
• Difference of 3.3 to 1.7 Ionic• Difference of 1.7 to 0.3 Polar Covalent• Difference of 0.3 to 0.0 Non-polar Covalent
Chemical Bonding Notes
• Read the 3 sections & complete notes– Introduction to Chemical Bonding (Pg 165)– Covalent Bonding and Molecular Compounds (Pg
168)– Ionic Bonding and Ionic Compounds (Pg 180)
• Not all of the blanks are for bolded vocabulary words. You will have to read thoroughly.
What type of bond will form?
Practice Problem A
• What type of bond will form between Lithium and Fluorine?
• Hint: you need to look up the electronegativity value of both elements on page 153
• What type of bond will form between Lithium and Fluorine?
• What is the difference in electronegativity?• Lithium: 1.0• Fluorine: 4.0• 4.0 – 1.0 = 3.0 • Ionic Bond!
Practice Problem A
Practice Problem B
• What type of bond will form between Oxygen and Hydrogen?
• Hint: you need to look up the electronegativity value of both elements on page 153
• What type of bond will form between Oxygen and Hydrogen?
• What is the difference in electronegativity?• Oxygen: 3.5• Hydrogen: 2.1• 3.5 – 2.1 = 1.4• Polar Covalent Bond!
Practice Problem B
Index Card Activity
• Every person will receive 3 index cards labeled:– I (Ionic)– PC (Polar Covalent)– NPC (Nonpolar Covalent)
• I will put up 2 elements on the board and based on their electronegativities, you will decide what type of bond will form
Sodium and Chlorine
3.0 – 0.9 = 2.1 Ionic Bond
Sulfur and Oxygen
3.5 – 2.5 = 1.0 Polar Covalent Bond
Calcium and Oxygen
3.5 – 1.0 = 2.5Ionic Bond
Carbon and Hydrogen
2.5 – 2.1 = 0.4Polar Covalent Bond
Hydrogen and Hydrogen
2.1 – 2.1 = 0Non-polar Covalent Bond
Nitrogen and Oxygen
3.5 – 3.0 = 0.5Polar Covalent Bond
Potassium and Bromine
2.8 – 0.8 = 2.0Ionic Bond
Fluorine and Fluorine
4.0 – 4.0 = 0.0Non-polar Covalent Bond
Potassium and Iodine
2.5 – 0.8 = 1.750% Ionic
50% Polar Covalent Bond
Week 12: Thursday Exit Ticket
1. What are the 3 types of bonds?2. What type of bond would form between Hydrogen and Sulfur?3. What type of bond would form between 2 atoms of Nitrogen?
Week 12: Friday Do Now
1. Ionic bonds _____ electrons2. Covalent bonds _____ electrons3. What type of bond would form between an atom of Nitrogen and Oxygen?
Covalent Bonds
Types of Covalent BondingSingle bond- one pair of
electrons is shared between two atoms
Chlorine-ChlorineCl-Cl
Types of Covalent BondingDouble bond- two pairs of electrons are shared between two atoms
Oxygen-OxygenO-O
Types of Covalent BondingTriple bond- three pairs of
electrons are shared between two atoms
Nitrogen-NitrogenN-N
Examples A, B, and C
Drawing Covalent Bonds in Molecules
Steps to draw a covalent bond
1. Write out all atoms in the molecule2. Draw Lewis Dot Diagrams for each atom in the molecule3. Count the total number of valence electrons to be shared
among the atoms 4. Arrange the atoms to form a skeleton structure for the
moleculeEach atom should now have an octet Circle the electron pair bonds. (Each atom wants a full shell of 8) (Exception: hydrogen wants only 2)
5. Draw the electron pairs as lines. These are the covalent bonds.
3. )
Drawing Covalent Bonds in Molecules
Silane: SiH4
Ammonia: NH3
Hydrogen sulfide: H2S
Carbon Dioxide: CO2
• https://www.youtube.com/watch?v=YHxHjnS5y5E
Week 12: Friday Exit Ticket
Using Lewis Dot Diagrams…1. Draw the bond between Lithium
and Sodium2. Draw the bond between two
atoms of Bromine