Quarter 2 Starters.

Slides:

Advertisements

Similar presentations

III. Ionic Compounds (p. 210 – 224)

Advertisements

The Chemistry Hot Seat Break into groups. I will provide you with a question. Everybody in the group will write down the question and provide an answer.

1 4.6 Covalent Compounds Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings Chapter 4 Forces Between Particles.

Ionic Bonding Review. 1) Octet rule: atoms tend to have.. 2) Electrons in the highest occupied energy level 3) An ionic bond is between a ____ and an.

Ionic and Covalent Bonding 1. Bonding Atoms with unfilled valence shells are considered unstable. Atoms will try to fill their outer shells by bonding.

WRITING FORMULA FOR IONIC COMPOUNDS

Ionic and Covalent bonding. Bonds All atoms are trying to get enough electrons so that their valence shell is full. All atoms are trying to get enough.

Ionic and Covalent Compounds Review. Calcium and Phosphorus Will the compound formed be ionic or covalent? Ionic Write the balanced formula Ca 3 +2 P.

Starter Give the electronic configuration of an atom of: Be Mg Ca Where are these elements found in the periodic table?

Chemistry 103 Lecture 10. EXAM I Survey How did you do on this exam? (Grade range, don’t give your actual score) Did your performance meet your expectations?

Chemistry 103 Lecture 11. Outline I. Ionic Compounds (in review) II. Covalent Compounds  Lewis Dot Diagrams/Lewis structures  Properties predicted 

Complete the worksheet on the structure of the atom

Demonstrate Understanding of Acids and Bases

What do you know about bonding?

Chapter 3 – Elements Combine to Form Compounds. Ion Charge or Combining Capacity Revisited The number of bonds an atom wants to form –Determined by the.

Tech Notes: Why Atoms Combine  Molecule and Compound:  Two or more atoms chemically combined  Have completely different properties than those of the.

Compounds  Atoms are more stable if their outermost (valence) shell is full  most element atoms tend to lose or gain electrons  elements are usually.

How many spherical objects can you think of? Starter.

Write down the formulae for these: a)Iron (II) Sulfate b)Magnesium Oxide c)Silver Carbonate d)Sodium Phosphate e)Copper Hydroxide f)Aluminium Hydroxide.

Ionic Bonds & Ionic Compounds Types of ions – Monatomic ions - ions formed from a single atom. Ca 2+, K +, Al 3+, Cu +, Cu 2+, Fe 2+, Fe 3+, Cl -, O 2-,

Naming Ionic Compounds. Ionic compounds have two components: Ionic compounds have two components: A cation (positive ion) and an anion (the negative ion).

Naming - Ionic Compounds. Charges or Oxidation Numbers Group 1A  ________ Group 2A  ________ Group 3A  ________ Group 4A  ________ Group 5A  ________.

SNC2P Ions and Ionic Compounds. Forming Ions In an atom the number of protons equals the number of electrons. If electrons are added to an atom, the atom.

Naming Ionic Compounds

Balancing Reactions Agenda Quick Quiz Notes on Balancing Reactions Practice, practice and more practice! Homework: More Balancing!

1 CHEMICAL BONDING. 2 Types of Bonds Ionic—transfer of 1 or more electrons from one atom to another (one loses, the other gains) forming oppositely charged.

Chapter 19: Chemical Bonding “Isn’t It Ionic?”. Questions for Review.

Ionic Bonds. How Bonds Form Electrons are transferred from a metal to a nonmetal. Ex: NaCl, CaI 2, Fe 2 O 3 -metals form cations (+) (gives away electrons)

453D-B7EE-4DF53F92A9C4&blnFromSearch=1&productcode=US.

4.1 Ionic Bonding & Structure

Atomic Structure.

Do Now Describe the difference between an ionic bond and a covalent bond.

a. protons b. neutrons c. electrons d. morons a. protons b. neutrons c. electrons d. morons.

Describe how atoms cannot be created or destroyed in a chemical reaction Balance symbol equations Outcomes State a definition of a chemical reaction in.

Top left Write the name for 1 oxygen and 2 fluorine atoms. Top right Identify as ionic or covalent. Bottom left Draw It. Bottom right According to VSEPR,

Unit 6 Ionic Compounds Remember…  The electrons in the outermost level or shell are called… –Valence electrons  You can determine the number of valence.

Ch 2.1 Elements combine to form compounds. Compounds have different properties from elements Elements have individual properties that help us identify.

CHEMISTRY NOTES Polyatomic Ions. What is the formula for….  Iron (III) chloride  FeCl 3  Copper (II) nitride  Cu 3 N 2  Tin (II) Oxide  SnO.

Unit 6 Ionic Compounds Remember…  The electrons in the outermost level or shell are called… –Valence electrons  You can determine the number of valence.

Pick Up a Packet & Calculator Write Down EQ Molar Mass EQ: How is molar mass calculated?

How Compounds Form. Compound A pure substance made up of two or more elements that are chemically combined Examples of Compounds 1.Water made up of hydrogen.

Chapter 5 Notes COMPOUNDS AND MOLECULES. Chemical Formulas  A chemical formula contains atomic symbols and subscripts to show the elements and the number.

Balancing Equations Interactive Bonding learner.org.

BELLRINGERS 3rd SEMESTER

Draw a Bohr Model of Chlorine (Cl)

Ionic & Covalent Bonding

Q/ A How would a compound form when Lithium is combined with Phosphorous? How many atoms of each would their be ? How would we write this out at a compound.

1.3 Ions and Octet Rule.

Q 2 Create a list of ways you can quickly predict whether two elements will create an ionic bond. What are chemical formulas and why are they useful? Write.

Naming Ionic Compounds

Chemical Bonding.

What elements form ionic compounds? How is an ionic bond formed?

Ions and Ionic Bonding.

Ions In general, atoms are electrically neutral

Ch. 7 Chemical Bonding.

Naming Ionic Compounds

Links Keywords C2 Elements, Compounds and Mixtures C2.2 Bonding

Knowledge Organiser – Formulae and equations

Naming Ionic Compounds

Naming Ionic Compounds.

Ions & formation of Ionic compounds

Naming - Ionic Compounds

Naming Polyatomic Compounds

Naming Ionic Compounds.

Monday, November 9, 2015 Bell Ringer: Define electronegativity.

! 1. What is an electron in the highest energy level of an atom called? A. Cation B. Anion C. Valence electron D. Core electron.

Naming Ionic Compounds

Practice Problems How many valence electrons are in each of the following molecules O3 C2H6O NO2 Draw a Lewis structure diagram for each.

Do Now Describe the difference between an ionic bond and a covalent bond.

Presentation transcript:

Quarter 2 Starters

October 26th and 27th No starter

Draw an example of the Bohr model. Label the parts October 28th and 29th Draw an example of the Bohr model. Label the parts

October 28th and 29th What is an atomic orbital? How many electrons fit in a p orbital?

November 2nd and 3rd Draw the orbital diagram for magnesium. Write the electron configuration for chlorine.

November 5th and 6th Draw two waves, label one as high frequency and one as low frequency. Label the amplitude and wavelength on one wave.

November 6th and 9th What variable represents frequency? What variable represents wavelength? What equation would you use to find energy if you had the frequency?

November 10th and 11th Place your packet from last class on your desk so I can see # 2 and 3 Convert 8.93 x 10-7 m to nm. Convert 230 nm to m

November 12th and 13th Which wave has a higher frequency? One with a wavelength of 400 nm or one with a wavelength of 800 nm? Which has more energy?

November 16th and 17th Draw the Bohr diagram for carbon. Draw the orbital diagram for carbon Write the electron configuration for carbon

November 18th and 19th What does c stand for in the energy equations? How is light produced by an atom?

November 20th and 23rd Draw the Lewis symbol for oxygen and cesium. Write if each gains electrons or loses electrons, and how many . Eg –Gains 3/ Loses 4\

November 30th & December 1st Write the formula and name for the compound formed from 1. Ca and O 2. Cu+3 and F

December 2nd and 3rd Name the following compounds Zn3N2 Ca(NO3)2

December 4th and 7th What type of elements are in an ionic bond? What type in a metallic bond? What type in a covalent bond?

December 8th and 9th Draw the Lewis structure for PH3 SiO2

December 10th and 11th Name the following Na2CO3 P2O5 NiS NH3

December 14th and 15th Draw the lewis structure, decide the shape, name the compound PCl3 H2S

December 16th and 17th Write the formula Calcium sulfide Triphosporus pentaoxide Iron (II) Phosphate

January 4th and 5th Name the following MgSO4 CuCl2 NO2

January 6th and 7th Write and balance the equation Magnesium chloride reacts with sodium to form sodium chloride and magnesium metal

January 8th and 11th Identify the type of reaction K + S  C2H6 + O2  NaCl + Ca 

January 12th and 13th On the powerpoint slides you picked up today Write as an equation and complete the products Silver (I) nitrate reacts with sodium chloride Get out homework from last class, put predicting products on top on your desk to be checked.