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$$$ Quiz $$$ Covalent Bonding and Naming
A bond in which electrons are shared. covalent
A bond in which electrons are exchanged or taken. ionic
How many valence electrons are in an atom of selenium? 6
Does PCl 3 break the octet rule? Part 2: Draw the lewis structure on the board. no
True or False: The pair of electrons in ammonia not involved in bonding is called the “outer pair” ? False, lone pair or unshared pair
What type of bond forms when an “s” orbital overlaps with an s, p, or hybrid orbital? Sigma,
Does the element iodine exist as a monotomic, diatomic, or triatomic molecule? diatomic
What type of orbital and how many of these orbitals are needed to make a pi bond. “p” orbital, 2
Write down the prefixes (from 1-10) used in naming binary molecular compounds. Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
Draw a hydrogen bond on the board.
A triple bond contains how many electrons? 6
CsF, H 2 O, ZnS, Ba I 2 Which one of these compounds is a molecular (covalent) compound? H2OH2O
Give the hybridization of each carbon atom in the following molecule? sp 3 sp 2 sp
What is the shape of AsF 3 ? Trigonal pyramidal
What is the shape of GeCl 4 ? Tetrahedral
What is the shape of SeCl 2 ? Bent or Angle
What is the shape of AlCl 3 ? Trigonal Planar
What is the shape of CS 2 ? Linear
What is the shape of PBr 5 ? Trigonal Bipyramidal
Which one of these is the most polar bond? C-O or C-F or C-Cl or C-N C-F, polar covalent bond
What type of hybrid orbital exists in a methane molecule? sp 3
Name the four intermolecular forces that we recently talked about. Dipole-dipole Ion-dipole Dispersion forces (London) Hydrogen bonding
Which one of these forces is the weakest? Dipole-dipole Ion-dipole Dispersion forces (London) Hydrogen bonding
Write the formula for nitrogen trioxide. NO 3
Write the formula for diphosphorus pentabromide. P 2 Br 5
Write the name of the compound, H 2 O 2. Dihydrogen dioxide, hydrogen peroxide
Write the name of the compound, Si 2 Cl 7. Disilicon heptachloride
What is the chemical formula of tin(IV) carbonate? Sn(CO 3 ) 2
A bond where electrons are shared is known as a _______ bond? covalent
Is there such a thing as S 3- ? No, only S 2-, sulfide
Draw the electron dot structure of silicon?
How many valence electrons does aluminum have? three
Draw the lewis structure for SCl 2
Draw the lewis structure for AsH 3
Draw the lewis structure for HSCN
Is CHCl 3 a polar or nonpolar molecule?
Is BCl 3 a polar or nonpolar molecule?
Is NO 2 a polar or nonpolar molecule? What’s its geometry? Does it have resonance structures? Show on board. Polar, bent
Draw the electron dot structure of antimony ?
What is the chemical formula of ammonium hydroxide? NH 4 OH
Chapter 8 Covalent Bonding. Covalent bonds Atoms share their electrons When atoms share they create a molecule.
Chemistry Chapter 9 Reveiw. Vocab Review Structural Formula Molecule VSEPR Theory Coordinate covalent bonding Hybridization Oxyacids Electronegativity.
TRIVIA Click for Question The strongest intermolecular force…. Hydrogen Bonding Click for: Answer and next Question.
Chapter 9 Covalent Bonding. Section 9.1 Atoms bond together because they want a stable electron arrangement consisting of a full outer energy level. Atoms.
Forming Molecular Bonds. What is a covalent bond? The chemical bond that results from the sharing of electrons Non-metals combine to acquire a full.
Aim: How do chemists use molecular geometry to predict polarity? Metallic bonding Polarity of water and "hydrogen bonding“ Water.
What happens if interacting things do not want to give? They must share…
Jennie L. Borders. Section 8.1 – Molecular Compounds A covalent bond is formed between atoms held together by sharing electrons. A molecule is a group.
Covalent Bonding and Naming. I. Types of Covalent Bonds l. Nonpolar covalent bond-a covalent bond in which the bonding electrons are shared equally 2.
Intermolecular and Intramolecular Forces Review. In the compound PCl 3, how many valence electrons are present?
COVALENT BONDS ELECTRONEGATIVITY 1. Bonds formed by sharing electrons between atoms 2. Group of atoms held together by covalent bond, called molecule OCTET.
MOLECULAR GEOMETRY VSEPR ACTIVITY. CARBON DIOXIDE Chemical formula: CO 2 # of atoms bonded to central atom: 2 # of lone pairs on central atom: 0 What.
Molecules. Objectives Write the electron dot structure for an atom. Explain how covalent bonds form molecules.
MOLECULAR COMPOUNDS. Bonding Atoms combine with each other in two general ways: 1. Ionic Compounds: transfer of electrons from one atom to another June.
Tro IC How many dots showing electrons are around the “S” in the Lewis structure of a sulfur atom?
In this chapter you will learn about compounds and their names and formulas.
IIIIII Molecular Geometry (p. 232 – 236) Ch. 8 – Molecular Structure.
Chapter 8: Covalent Bonding Vocabulary: Leave enough space for definition and example 1.Covalent bond 2.Electron dot structure 3.Diatomic Molecules 4.Polar.
Covalent Bonding Covalent Bonding and Covalent Nomenclature.
Covalent compounds Sharing of electrons. Chemical Bonds Ionic Bond – Transfer of electron – Exist in a crystal lattice form Covalent Bond – Pairs of electrons.
CHEMISTRY PART 11 Covalent Compounds. Remember... Metals want to lose electrons and non-metals want to gain them. These are ionic bonds.
Naming with Roman numerals Naming with Greek Prefixes.
Covalent Compound Notes Why do atoms bond? Atoms gain stability when they share electrons and form covalent bonds. Lower energy states make an atom more.
Unit 7 Covalent Bonding. Bonding A metal & a nonmetal transfer electrons –An ionic bond Two metals mix –An alloy (Metallic bond) What do two nonmetals.
Covalent compounds A covalent compound consists of two or more nonmetals. They are able to bond together by sharing their valence electrons.
Molecular Nomenclature and Geometry Chemistry Text Ch 6.1,6.2,6.5,
DE Chemistry – King William High School. Cation – positive charge lose an electron Alkali metals (group 1) take a +1 charge Alkaline earth metals.
Drawing Lewis Structures “ valence dot diagrams” The valence shell holds up to 8 electrons. 0.Determine the number of valence electrons. 1. Write the element’s.
Molecules and Covalent Bonding Substances that are formed by covalent bonding are called molecules. They are characterized by: Bonding formed by two non-metals.
Ch. 12 Notes---Covalent Bonds Covalent Bonds ____________ electrons between two atoms in order to fill the outer energy level (or shell) Each bond involves.
Chemical Bonding b Chapter 6. Chemical bond b The force (electrical attraction) that binds two atoms together.
Chemical Bonds: The Formation of Compounds from Atoms Dr. Bixler-Zalesinsky.
Chapter 15/16 Bonding. Types of Chemical Bonds A. Ionic bond: Results from the electrostatic attraction between positive and negative ions B. Covalent.
Chemical Bonding Shape Lab. 1)One structural isomer only.
Chapter 12 Chemical Bonding Chemistry B2A. 1.Ionic bonds 2. Covalent bonds 3. Metallic bonds 4. Hydrogen bonds 5. Van der Waals forces Chemical Bonds.
Chapter 6 Section 5 Molecular Geometry pages Modern Chemistry Chapter 6 Chemical Bonding Sections 1-5 Introduction to Chemical Bonding Covalent.
Covalent Bonding The joining of two or more elements through the sharing of valance electrons to form a molecule Purpose: To form a stable octet between.
The bond that forms from the sharing of valence electrons.
Ch 6.5 Molecular Geometry. VSEPR Theory Use VSEPR theory Valence-Shell-Electron-Pair Repulsion =the repulsion between electron pairs causes molecular.
1 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) Some examples of molecules with this geometry are: NH 3, NF 3, PH 3,
Section 8-1 Section 8.1 The Covalent Bond Apply the octet rule to atoms that form covalent bonds. chemical bond: the force that holds two atoms together.
Mid-Term Review Ch 7 and 8. Name Me MgSO 4 Name Me PCl 5.
Day 14 – Covalent bonds Sci 10Chemistry. Covalent Bonds Non-metal + non-metal.
Drawing Lewis Dot Structures Covalent compounds 1. Figure valence e- for each atom 2. Draw Lewis Dot Structure 3. Combine atom so each has 8 e- exception.
Review Write the electron configuration for an atom of carbon and chlorine. Determine the empirical and molecular formula for a compound consisting of.
Molecular Compounds. Outline Molecular Compounds Diatomic Molecules Naming Molecular Compounds Combining Capacity.
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