Ppt on chapter 3 atoms and molecules ppt

LECTURE 5.2. LECTURE OUTLINE Weekly Reading Weekly Reading Prototype Practice Quiz 5: Feedback Prototype Practice Quiz 5: Feedback Molecules, Monomers,

and melting point (both of which were first introduced in Chapter 3). CHAPTER XVI: COVALENT BONDING Oftentimes, the only bond that is ever mentioned in high school is the covalent bond. The covalent bond and the molecule are shown to be inextricably linked, and Chapter 16 defines "the molecule/ matter” consists of “formless” silicon plus The “primal matter” consists of “formless” silicon plus oxygen atoms. The geometric form that is imposed on this matter is a tetrahedron. The geometric form that is imposed/


Chapter 1: An introduction to Anatomy and Physiology.

Integumentary Skeletal Muscular Nervous Endocrine Cardiovascular Lymphatic Respiratory Digestive Urinary Reproductive Organ Level The heart Cardiac muscle tissue Tissue Level (Chapter 4) Cellular Level (Chapter 3) Heart muscle cell Protein filaments Complex protein molecule Atoms in combination Chemical or Molecular Level (Chapter 2) Organ System Level (Chapters 5–20) Figure 1-1 6 of 7 Copyright © 2007 Pearson Education, Inc., publishing as Benjamin Cummings Integumentary Skeletal Muscular/


The Chemistry of Life. E. coli vs. E. coli Atoms Submicroscopic units of matter Smallest unit of all physical material.

from element or compound Oxygen –Strong electron receptor –Most frequent receptor in biological systems Reduction Process where an atom gains an electron Changes charge by -1 Oxidation and reduction occur together Called redox reactions Diatomic Molecules Paired atoms that form a molecule Share electrons with covalent bond H 2 = Hydrogen Gas O 2 = Oxygen Gas Cl 2 = /Indicates concentration of H + ions Neutral is at 7 Determined by taking negative value of exponents of its H + ions concentration End Chapter 3


THE CHEMICAL CONTEXT OF LIFE Campbell and Reece Chapter 2.

very close together  shape of a molecule key to its function in cell  shape of a molecule with >2 atoms determined by positions of atom’s orbitals  determines how biological molecules recognize & respond to each other with specificity  2 molecules temporarily forming weak bond can only happen if their shapes are complimentary to each other  because morphine and endorphins have same shape that fits into endorphin receptors/


Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Define molecule and molecular formula. Explain the relationships.

kind in a chemical compound by using atomic symbols and numerical subscripts. ***A molecular formula shows the types and numbers of atoms combined in a single molecule of a molecular compound. Section 2 Covalent Bonding and Molecular Compounds Chapter 6 Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Comparing Monatomic, Diatomic, and Polyatomic Molecules Chapter 6 Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu/


CHE2201, Chapter 2 Learn, 1 Polar Covalent Bonds: Acids and Bases Chapter 2 Suggested Problems - 1-19,25-6,31,34,36,39- 40,51-2.

Learn, 41 Organic chemistry is 3-D space Molecular shape is critical in determining the chemistry a compound undergoes in the lab, and in living organisms Molecular Models CHE2201, Chapter 2 Learn, 42 Several types: -Dipole-dipole forces -Dispersion forces -Hydrogen bonds Noncovalent Interactions When thinking about chemical reactivity, chemists typically focus on bonds, the covalent interactions between atoms within molecules. Also important are the/


Chapter 3 Biochemistry Pg. 50. Section 1: Carbon Compounds Organic Compounds Contain carbon Come from living things How can you tell whether a compound.

Functional Groups A cluster of atoms that influence the molecules they compose There are 4 functional groups: 1. hydroxyl 2. carboxyl 3. amino 4. phosphate 1. Hydroxyl ( -OH) * can make the molecule it is attached to polar Polar molecules are soluble in water An / acids which make up proteins 4. Phosphate Ex. ATP (adenosine triphosphate) There are 3 phosphate groups in ATP. ATP is a molecule that stores energy AND supplies that energy directly to cells Energy is released from ATP when the bonds between /


Chapter 6. Counting Atoms Subscripts indicate the number of atoms in a COMPOUND.

Subscript 2 Ag 1 Cl 2 Molecules: Two Atoms 2x1 = 2 Ag Atoms 2x2= 4 Cl Atoms 2 AgCl 2 4 NaCl Molecules = 4 Atoms: 4 Sodium Atoms 4 Chlorine Atoms 2 Ca(OH) 2 Molecules = 2 Atoms: 2 Calcium Atoms 4 Oxygen Atoms 4 Hydrogen 3 H 2 O Molecules = 3 Atoms: 6 Hydrogen Atoms 3 Oxygen Atoms 4 CO 2 Molecules = 4 Atoms: 4 Carbon Atoms 8 Oxygen Atoms An expression that uses chemical formulas and symbols to describe a reaction Chemical/


CHAPTER 2 CHEMISTRY OF LIFE ATOMS, MOLECULES, WATER AND MACROMOLECULES.

DIFFERENT AMINO ACIDS ARE FOUND IN PROTEINS. Chapter 2 NUCLEIC ACID : LONG CHAIN OF SMALLER MOLECULES CALLED NUCLEOTIDES. NUCLEOTIDE HAS THREE PARTS: A SUGAR, A BASE, AND A PHOSPHATE GROUP CONTAINS PHOSPHORUS AND OXYGEN ATOMS. Chapter 2 NUCLEIC ACIDS EACH TYPE CONTAINS FOUR/ ENZYME’S SHAPE CHANGES SLIGHTLY. STEP 2 AT AN ACTIVE SITE, AN ENZYME AND A SUBSTRATE INTERACT, REDUCING THE REACTION’S ACTIVATION ENERGY. STEP 3 THE REACTION IS COMPLETE WHEN PRODUCTS HAVE FORMED. FACTORS IN ENZYME ACTIVITY ANYTHING THAT/


The Mole Chapter 10. What is a mole? A conversion factor used in chemistry to make it easier to talk about a very large amount of particles of elements.

The Mole Chapter 10 What is a mole? A conversion factor /make up 1.3 moles? Particles to Moles How many moles make up 5.60 x 10 25 atoms of copper? Particles to Moles 25 molecules of carbon tetrahydride= ? moles How does mass relate to the mole? What does an amu (atomic mass unit) / What is the mass of 2.77 x 10 13 molecules of oxygen? Liters to Mole Conversions Liters (L) are a volume unit of measurement STP= standard temperature and pressure conditions (0° and 1 atm) This conversion only may be used when: /


The Mole: A Measurement of Matter

atoms and 1.0 g of hydrogen atoms must have the same number of atoms. Representative Particle Smallest unit in a substance Can be different things One atom (metals, atomic substances) One molecule (molecular compounds) One ion (charged atoms or molecules)/Atoms/Rp= 14.08 X 1024 atoms Clean all results to single digit number!!! 14.08 X 1024 → Atoms = 1.4 x 1025 atoms Practice You have 4.65 x 1024 molecules of NO2? Q: How many atoms? A: RP NO2 has three atoms/molecule 3 atoms/molecule x 4.65 x 1024 molecules/


Chapter Five Molecular Compounds Fundamentals of General, Organic and Biological Chemistry 5th Edition James E. Mayhugh Oklahoma City University  2007.

42 Chapter Summary Contd. ►Molecular formulas show the numbers and kinds of atoms in a molecule. ►Lewis structures show how atoms are connected in molecules. ►Covalent bonds are indicated as lines between atoms, and valence electron lone pairs are shown as dots. ►Molecules have shapes that can be predicted using the VSEPR model. ►The electronic geometry of atoms with 2 electron charge clouds is linear, with 3 it is planar triangular, and/


Chapter 6 Section 5.

bonding is that which occurs between water molecules. The strong hydrogen bonding between water molecules accounts for many of water’s characteristic properties. Visual Concepts Chapter 6 Hydrogen Bonding Chapter 6 Intermolecular Forces – London Dispersion Forces Section 5 Molecular Geometry Chapter 6 Intermolecular Forces – London Dispersion Forces Even noble gas atoms and nonpolar molecules can experience weak intermolecular attraction. In any atom or molecule—polar or nonpolar—the electrons are/


Chapter 22 Review “Hydrocarbon Compounds”

alkanes all end with the suffix ____. Why are the molecules of hydrocarbons nonpolar? Chapter 22 Review In a cyclic hydrocarbon with only carbon-carbon single bonds and n number of carbon atoms, how many hydrogen atoms are there in terms of n? The name for an / two carbons is __. What is the name of the compound CH3CH(CH3)C(CH3)3? How many more hydrogen atoms does a cyclohexane molecule have than a benzene molecule? Chapter 22 Review What percent of the composition of natural gas is methane? How many forms /


Introductory Chemistry, 3rd Edition Nivaldo Tro

O has 6 e− for a total of 25 e−. Add 1 e − for the negative charge to get a grand total of 26 e− Tros Introductory Chemistry, Chapter 10 Writing Lewis Structures for Covalent Molecules, Continued 3. Attach atoms with pairs of electrons and subtract electrons used from total. Bonding electrons. 4. Add remaining electrons in pairs to complete the octets of all the/


Physics 207: Lecture 25, Pg 1 Lecture 25Goals: Chapters 18, micro-macro connection Chapters 18, micro-macro connection Third test on Thursday at 7:15 pm.

Chapters 18, micro-macro connection Chapters 18, micro-macro connection Third test on Thursday at 7:15 pm. Physics 207: Lecture 25, Pg 2 (m/s) Percentage of molecules 5 10 15 0-100 100-200 200-300300-400 400-500500-600 600-700 700-800 800-900900-1000 1000-1100 1100-1200 Nitrogen molecules/ near room temperature Physics 207: Lecture 25, Pg 3 l What is the typical size of an atom or a small molecule? Atomic /and most random macroscopic state l Thermal energy is spontaneously transferred from a hotter/


Chapter 6 Preview Lesson Starter Objectives Chemical Bond.

one carbon atom, one iodine atom, and three hydrogen atoms. 2. Write the electron-dot notation for each type of atom in the molecule. Carbon is from Group 14 and has four valence electrons. Iodine is from Group 17 and has seven valence electrons. Hydrogen has one valence electron. Lewis Structures, continued Section 2 Covalent Bonding and Molecular Compounds Chapter 6 Lewis Structures, continued Sample Problem C Solution, continued 3. Determine/


SB1- Relationship between Structure and Function in Cells

SB1- Relationship between Structure and Function in Cells 6.1 Atoms, Elements, and Compounds Atomic Mass: the number of protons & neutrons in the nucleus of an element (atom). Find the neutrons only: Atomic mass-atomic number=neutrons Ex: Carbon Picture SB1- Relationship between Structure and Function in Cells Chemical Bonds hold atoms, molecules and compounds together Chapter 6 Chemistry in Biology 6.1 Atoms, Elements, and Compounds Chemical Bonds hold atoms, molecules and compounds together Two types/


Chapter Five Molecular Compounds Fundamentals of General, Organic and Biological Chemistry 6th Edition James E. Mayhugh Copyright © 2010 Pearson Education,

48 Chapter Summary Contd. ►Molecular formulas show the numbers and kinds of atoms in a molecule. ►Lewis structures show how atoms are connected in molecules. ►Covalent bonds are indicated as lines between atoms, and valence electron lone pairs are shown as dots. ►Molecules have shapes that can be predicted using the VSEPR model. ►The electronic geometry of atoms with 2 electron charge clouds is linear, with 3 it is planar triangular, and/


BONDING: GENERAL CONCEPTS

described as forces that hold groups of atoms together and make them function as a unit. Atoms will bond with each other to form molecules if the energy of the aggregate is lower than that of the separated atoms. Atoms bond with each other by either /of an Ionic Solid 1.Sublimation of the solid metal M(s)  M(g) [endothermic] 2. Ionization of the metal atoms M(g)  M+(g) + e [endothermic] 3. Dissociation of the nonmetal 1/2X2(g)  X(g) [endothermic] 8.5 Copyright © Houghton Mifflin Company. All rights /


Chapter 101 Bonding and Molecular Structure Chapter 10.

MO); -One molecular orbital has little electron density between nuclei (  *, antibonding MO). Chapter 1017 Molecular Orbitals The Hydrogen Molecule Chapter 1018 Molecular Orbitals The Hydrogen Molecule Chapter 1019 Molecular Orbitals The Hydrogen Molecule Chapter 1020 Molecular Orbitals The Hydrogen Molecule -MO diagram shows the energies and orbitals in an MO diagram. -The total number of electrons in all atoms are placed in the MO’s starting from lowest energy (  1s/


Chapter 2 Atoms, Molecules, and Ions

with alkane ending “ane” e.g., propane is a 3-carbon alkane EOS Chapter 2: Atoms, Molecules, and Ions Chapter 2: Atoms, Molecules, and Ions Table 20.2 Chapter 2: Atoms, Molecules, and Ions Chapter 2: Atoms, Molecules, and Ions Ethane Propane Second most simple alkane Minor ingredient of natural gas Also known as bottled gas Found in natural gas, but separately for commercial purposes Chapter 2: Atoms, Molecules, and Ions Chapter 2: Atoms, Molecules, and Ions Butane Gas used in Butane lighters Four carbon/


VSEPR Theory As shown at right, diatomic molecules, like those of (a) hydrogen, H 2, and (b) hydrogen chloride, HCl, can only be linear because they consist.

b.Draw the Lewis structure of the chlorate ion. There are three oxygen atoms bonded to the central chlorine atom, which has an unshared electron pair. This is an AB 3 E molecule, which is trigonal-pyramidal. Section 5 Molecular Geometry Chapter 6 VSEPR Theory, continued VSEPR and Hybrid Orbitals VSEPR predicts shapes of molecules very well. How does that fit with orbitals? Let’s use H/


Chapter-2-1 Chemistry 281, Winter 2015, LA Tech CTH 277 10:00-11:15 am Instructor: Dr. Upali Siriwardane Office: 311 Carson.

electron configuration hybridization is sp 3 d 2 Chapter-2-53 Chemistry 281, Winter 2015, LA Tech Molecular Orbital Theory Molecular orbitals are obtained by combining the atomic orbitals on the atoms in the molecule. Molecular orbitals are obtained by combining the atomic orbitals on the atoms in the molecule. Chapter-2-54 Chemistry 281, Winter 2015, LA Tech Bonding and Anti-bobding Molecular Orbital Chapter-2-55 Chemistry 281, Winter/


Chapter 2: Atoms, Molecules, and Ions The Atomic Theory of Matter Democritus (460-371 BC): matter consists of atoms which are solid particles (a-tomos.

2-, S 2 O 8 2- ] Chapter 2: Atoms, Molecules, and Ions Naming Ionic Compounds Common Oxyanions: Sulfate SO 4 2- Phosphate PO 4 3- Chlorate ClO 3 - Bromate BrO 3 - Iodate IO 3 - Nitrate NO 3 - Carbonate CO 3 2- Chapter 2: Atoms, Molecules, and Ions Naming Ionic Compounds Chapter 2: Atoms, Molecules, and Ions Naming Ionic Compounds You must know these! HCO 3 - Hydrogen carbonate ion or Bicarbonate ion Chapter 2: Atoms, Molecules, and Ions Naming Ionic Compounds: chemical formula → name/


Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA Introductory Chemistry, 2 nd Edition Nivaldo Tro Chapter 12 Liquids and Solids 2006,

physical interactions between molecules and the factors that effect and influence them Tros Introductory Chemistry, Chapter 12 3 The Physical States of Matter matter can be classified as solid, liquid or gas based on what properties it exhibits Fixed = keeps shape when placed in a container, Indefinite = takes the shape of the container Tros Introductory Chemistry, Chapter 12 4 Structure Determines Properties the atoms or molecules have different/


Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA Introductory Chemistry, 2 nd Edition Nivaldo Tro Chapter 10 Chemical Bonding 2006,

they do is central to chemistry chemists have an understanding of bonding that allows them to: 1)predict the shapes of molecules and properties of substances based on the bonding within the molecules 2)design and build molecules with particular sets of chemical and physical properties Tros Introductory Chemistry, Chapter 10 3 Lewis Symbols of Atoms also known as electron dot symbols use symbol of element to represent nucleus/


Preview Objectives Molecular Geometry VSEPR Theory Hybridization Intermolecular Forces Chapter 6 Section 5 Molecular Geometry.

therefore be linear: VSEPR Theory Section 5 Molecular Geometry Chapter 6 Representing the central atom in a molecule by A and the atoms bonded to the central atom by B, then according to VSEPR theory, BeF 2 is an example of an AB 2 molecule, which is linear. In an AB 3 molecule, the three A–B bonds stay farthest apart by pointing to the corners of an equilateral/


Chapter 51 Example NO 2 ( ) nitrogen ( ) oxide 2 O’snitrogen dioxide 1 NMononitrogen dioxide often omit “mono” Nitrogen dioxide.

monoxideH 2 O Silicon tetrafluorideSiF 4 dinitrogen tetroxideN 2 O 4 Chapter 56 Lewis Dot Structures Helpful in determining 3-D Shape of molecule Can use 3-D shape to predict properties of molecules Chapter 57 Rules for Lewis structures for molecules 1.Put in the atoms and arrange them to show which atoms are connected to which other atoms. H always on outside 2.Count the total number of outer/


Molecular Geometry Chapter 6.5. VSEPR THEORY Lewis Structures are 2D but we live in a 3D world. molecular geometry: the three-dimensional arrangement.

that electron pairs strongly repel each other. Predicting Molecular Geometry 1.Draw Lewis structure for molecule. 2.Count number of lone pairs on the central atom and number of atoms bonded to the central atom. 3.Use VSEPR to predict the geometry of the molecule. What are the molecular geometries of SO 2 and SF 4 ? SO O AB 2 E bent S F F F F AB/


LIVE INTERACTIVE YOUR DESKTOP May 24, 2012 ACS: Matter – Solids, Liquids, and Gases: Introducing a Free Online Resource for Middle School Chemistry.

Very Small Chapter 1: Matter – Solids, Liquids, and Gases American Chemical Society Welcome Six chapters of activity-based lesson plans that align with state standards and national frameworks in physical science and inquiry. Two main goals: Help students understand and be able/ that apply to liquids also apply to solids? American Chemical Society Heating and Cooling a Solid Ask students: If solids are also made of atoms and molecules, try to explain why this happens on the molecular level. American Chemical/


UNIT A: Cell Biology Chapter 2: The Molecules of Cells: Sections 2.1, 2.2 Chapter 3: Cell Structure and Function Chapter 4: DNA Structure and Gene Expression.

crust would differ from those present in living organisms. 2.Explain how radiation can be both beneficial and harmful to humans. 3.Explain the differences between oxygen 16 and oxygen 18. UNIT A Chapter 2: The Molecules of Cells Section 2.1 TO PREVIOUS SLIDE 2.2 Molecules and Compounds When atoms of two or more different elements bond together, a compound forms. Two types of bonds that/


Chapter Five Molecular Compounds. 10/9/2015 Chapter Five 2 Outline ►5.1 Covalent Bonds ►5.2 Covalent Bonds and the Periodic Table ►5.3 Multiple Covalent.

48 Chapter Summary Contd. ►Molecular formulas show the numbers and kinds of atoms in a molecule. ►Lewis structures show how atoms are connected in molecules. ►Covalent bonds are indicated as lines between atoms, and valence electron lone pairs are shown as dots. ►Molecules have shapes that can be predicted using the VSEPR model. ►The electronic geometry of atoms with 2 electron charge clouds is linear, with 3 it is planar triangular, and/


1 All Roads Lead to Mole City. 2 What Have We Learned Thus Far (10.1) How to convert from molecules to moles/moles to molecules.

1 mole CuHAsO 3 = 288.596 g CuHAsO 3 = 289 g CuHAsO 3 (only 3 sig figs) Moles x Molar Mass = Grams 10 Delayed Objective (10.2) Learn how to convert between moles and volume (L, gas) We will learn this when we derive the Ideal Gas Law in Chapter 14.3, but …… /3.45 x 10 25 molecules NH 3 17.0 g NH 3 N = 1(14.0) = 14.0 g/mol H = 3(1.0) = 3.0 g/mol molar mass NH 3 = 17.0 g/mol 1 mol NH 3 = 974.252 g NH 3 = 974 g NH 3 6.02 x 10 23 molecules NH 3 1 mol NH 3 13 Sample mixed mole problem: Grams to Molecules/Atoms/


Chapter 1: Crystal Structure. The Nobel “Booby” Prize! See the “Ig Nobel” Prize discussed at: Chapter 1: Crystal Structure.

Data Objectives At the end of this Chapter, you should: 1. Be able to identify a unit cell in a symmetrical pattern. 2. Know that (in 3 dimensions) there are 7 (& ONLY 7!!) Possible unit cell shapes. 3. Be able to define cubic, tetragonal/ All Solids! All solids have “resistance” to changes in both shape and volume Solids can be Crystalline or Amorphous Crystals are solids that consist of a periodic array of atoms, ions, or molecules –If this periodicity is preserved over “large” (macroscopic) distances the /


Chapter Five Molecular Compounds Fundamentals of General, Organic & Biological Chemistry 4th Edition Mohammed Hashmat Ali Southeast Missouri State University.

the periodic table reach an electron octet by sharing an appropriate number of electrons. Prentice Hall © 2003 Chapter Five 3  Water molecule results when two hydrogen atoms and one oxygen atom are covalently bonded in a way shown in the following picture: Prentice Hall © 2003 Chapter Five 4  When two atoms come together, electrical interactions occur.  Some of these interactions are repulsive – positively charged nuclei repel each other/


Bonding is the way atoms attach to make molecules an understanding of how and why atoms attach together in the manner they do is central to chemistry chemists.

oxyacids, the acid hydrogens are attached to an oxygen 2)Calculate the total number of valence electrons available for bonding – use group number of periodic table Tros Introductory Chemistry, Chapter 1017 Writing Lewis Structures for Covalent Molecules 3)Attach atoms with pairs of electrons and subtract electrons used from total – bonding electrons 4)Add remaining electrons in pairs to complete the octets of all the/


AP Biology 2005-2006 Chapter 9. Cellular Respiration Harvesting Chemical Energy.

energy-rich hydrogen is harvested as NADH, and two ATP molecules are formed. 3-carbon sugar phosphate 3-carbon sugar phosphate 3-carbon sugar phosphate 3-carbon pyruvate MCC BP Based on work/is to Make ATP! ATP What’s the point? AP Biology 2005-2006 Chapter 9. Cellular Respiration Oxidation of Pyruvate Krebs Cycle MCC BP Based on work/ passes electrons to ETC  H cleaved off NADH & FADH 2  electrons stripped from H atoms  H + (H ions)  electrons passed from one electron carrier to next in mitochondrial /


Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 6 Chemical Bonding Section 1 Introduction.

, continued Sample Problem C Draw the Lewis structure of iodomethane, CH 3 I. Section 2 Covalent Bonding and Molecular Compounds Chapter 6 Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Sample Problem C Solution 1.Determine the type and number of atoms in the molecule. The formula shows one carbon atom, one iodine atom, and three hydrogen atoms. 2.Write the electron-dot notation for each type of/


Organic Chemistry Chapter 24 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

molecules have at least one asymmetric carbon atom – a carbon atom bonded to four different atoms or groups of atoms Are the following molecules chiral or achiral? a) Cl | H-C-CH 2 -CH 3 | CH 3 b) Br | I-C-CH 2 -CH 3 | Br 24.2 Cycloalkanes Alkanes whose carbon atoms/ Group Chemistry Ethers have the general formula R-O-R’. CH 3 OH + HOCH 3 CH 3 OCH 3 + H 2 O H 2 SO 4 catalyst Condensation Reaction 24.4 Functional Group Chemistry Aldehydes and ketones contain the carbonyl ( ) functional group. O C R C/


Air Pressure Chapter 1, Section 2, p10-14. Properties of Air Air has mass – Air is made of atoms & moleculesAtoms & molecules have mass How can you.

Chapter 1, Section 2, p10-14 Properties of Air Air has mass – Air is made of atoms & moleculesAtoms & molecules have mass How can you test this? Because air has mass, it also has other properties, including density & pressure Density Density: the amount of mass in a given volume of air – Density = mass ÷ volume Increase molecules in volume of air = increase density Decrease molecules/end and partially / of mercury Altitude and the Properties of Air/molecules farther apart at high altitudes – Become quickly out of/


Chapter 11 : Matter Notes. Mole (mol) is equal to 6.02x10 23 The mole was named in honor of Amedeo Avogadro. He determined the volume of one mole of gas.

atomic mass for an element. Unit is g/mol. Converting moles to Mass: Number of moles number of grams = mass(g) 1 mole Converting moles to particles. Number of moles_ 6.02x10 23 _ particles = particle 1 mole Example: How many molecules are in 3.50 moles of sucrose? 3/Compounds: 1. Convert grams to formula units: 35.6 g AlCl 3 1 mol AlCl 3 6.02 x 10 23 formula units 133.33g AlCl 3 1 mol AlCl 3 = 1.61 x10 23 formula units AlCl 3 Chapter 11 Matter Notes Section 11.4 Percent Composition: Percent composition is /


Chapter 2 STRUCTURE AND PROPERTIES OF ORGANIC MOLECULES Chapter 2: Structure and Properties of Organic Molecules Helpful web site:

formation of  -orbitals. 2.The first bond between any pair of atoms is ALWAYS a  -bond. 3. Only ONE  -bond can be formed between any pair of two atoms. The rest (if any) are  -bonds. Chapter 2: Structure and Properties of Organic Molecules PREDICTIONS BASED ON ELECTRONIC STRUCTURE OF CARBON 1.There is one 2s and three 2p orbitals, to form four bonds total. It would be/


1 Macromolecules Chapter 6-3. 2 Organic Compounds Compounds organicCompounds that contain _________ are called organic. Derived from _________________.

Triple Bond: atom shares 3 electrons, three bars. 9 Macromolecules Large ____________ molecules.Large ____________ molecules. Polymers: a large molecule formed when many smaller molecules bond togetherPolymers: a large molecule formed when many smaller molecules bond together Made up of smaller “building blocks” called MONOMERS.Made up of smaller “building blocks” called MONOMERS. organic 10 Macromolecules Examples:Examples: 1. Carbohydrates 2. Lipids 3. Proteins 4. Nucleic acids (DNA and RNA)


Chapter 23 Review “Functional Groups”. Chapter 23 Review What is the name of the functional group in the following compound? What is the name of the functional.

between: CH 3 COH(CH 3 ) 2 and (CH 3 ) 3 COH CH 3 COH(CH 3 ) 2 and (CH 3 ) 3 COH  What is true about the boiling point of isopropyl alcohol?  What alcohol is used in antifreeze? Chapter 23 Review What substance is added to an organic molecule to test for/carbon skeleton of an ester look like? When an oxygen atom is attached to a carbon atom, the carbon atom becomes more ____. When an oxygen atom is attached to a carbon atom, the carbon atom becomes more ____. What is the test for aldehydes? What/


Introduction to Anatomy & Physiology Chapter 1 Introduction to Anatomy & Physiology Chapter 1.

heart Cardiac muscle tissue Tissue Level (Chapter 4) Cellular Level (Chapter 3) Heart muscle cell Protein filaments Complex protein molecule Atoms in combination Chemical or Molecular Level (Chapter 2) Organ System Level (Chapters 5–20) Figure 1-1 6/Diaphragm subdivides ventral cavity into: Thoracic cavity Abdominopelvic cavity Ventral Body Cavity Thoracic cavity Pleural cavities (R and L) Mediastinum Pericardial cavity Membranes of the Ventral Cavity Pleura Pericardium Double layered “serous membranes”: -/


Chapter 4 Notes The Structure Of Matter. Chapter 4.1 Notes Chemical Bond is the attractive force that holds atoms or ions together Chemical structure:

metal ions and the electrons around them (metals) Covalent bond : bond formed when atoms share one or more pairs of electrons (2 nonmetals) Polyatomic ion : an ion made of two or more atoms that are covalently bonded and that act like a single ion Chapter 4.3 Notes Naming /-vdW.png http://content.answers.com/main/content/wp/en- commons/thumb/a/ae/180px-Lithium-hydride- 3D-vdW.png “Gas molecules”. Jan. 24, 2008. http://www.phy.cuhk.edu.hk/contextual/heat/tep/t rans/kinetic_theory.gif http://www.phy.cuhk.edu/


CMH 121 Luca Preziati Chapter 3: Chemical Bonds Molecule = A group of at least two atoms, linked together by chemical bonds DEF Chemical Bond = An interaction.

by the electromagnetic force between opposing charges. DEF 1)predict the shapes of molecules and properties of substances based on the bonding within the molecules 2)design and build molecules with particular sets of chemical and physical properties Understanding Chemical bonding is used to: CMH 121 Luca Preziati Chapter 3: Chemical Bonds An atom and its relative ion have completely different properties. Na e-e- e-e- e-e- e/


Modern Chemistry Chapter 6 Chemical Bonding Part V Molecular Geometry and Intermolecular Forces.

than one bond depends on … bond polarity and molecule geometry. Chapter 6 Section 5 Molecular Geometry pages 197-207 24 Molecule Polarity 1.Draw the Lewis Structure true to shape. Example NH 3 N H H H : Chapter 6 Section 5 Molecular Geometry pages 197-207 25 Molecule Polarity 2.Find all the partial positive and negatives for each atom in the molecule H H H Look at each bond/


Chapter 2: Chemical Basis of Life Part I: Structure of Matter.

elements- Trace elements- Ultratrace elements- Atomic Structure Atoms Nucleus Electrons Protons Neutrons Fig. 2.1 Atomic Structure ●Atomic Number ● Atomic Mass (Weight) Isotopes –Stable Isotopes –Unstable Isotopes O, I, Fe, P, Co Radiation (α,β,γ) Molecules and Compounds Molecule Molecular Formula Compound Fig. 2.2 Bonding of Atoms Bonds Electron Shells Fig. 2.3 Bonding of Atoms All atoms want to be stable, meaning… –Octet Rule –Inert atoms Bonding of Atoms Ions Cation Anion Ionic Bonds/


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