Nyb F09 Unit 1 Slides 1 36

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Pertinent Info • Instructor Name: Tom (Tian-Yun) Wang • Email Address: [email protected] • Room #: H-253 • Local Telephone: 5879 • Office Hours: See Handout Primary Method for Contact: Messaging in Omnivox (M

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Transcript of Nyb F09 Unit 1 Slides 1 36

Page 1: Nyb F09   Unit 1 Slides 1 36

Pertinent Info

• Instructor Name: Tom (Tian-Yun) Wang

• Email Address: [email protected]

• Room #: H-253

• Local Telephone: 5879

• Office Hours: See Handout

• Primary Method for Contact: Messaging in Omnivox (MIO)

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Quizzes and Assignments

• Approximately 5 quizzes will be given throughout the semester, each worth 2% of your final grade. Tentative schedule coming shortly.

• Assignments will be given using an internet based system called “LON-CAPA”, all worth 5% of your final grade. More on how to access this system later.

• For more practice with chemistry questions, Problem Sets will be posted online. Completion of these problems are purely optional and do not account for marks

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Lecture Style and Note Access

• Powerpoint slides are used for main facts and diagrams, but often lacks details and explanations

• You do not need to write what is on the slide. It will be much more useful to take notes on what I am saying/explaining

• I will try to get the slides to you in advance of the class online in “Lea”, the Omnivox Classroom.

• Go to “Distributed Documents”, click on file and save to your computer.

• The rest is up to you in terms of organization

• Work will still be done directly on chalkboard

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Finding Motivation As a Student

The amount of motivation you have for school is importantin your success but also important is the kind of motivation that you have.

1. Intrinsic Motivation- Participating in an activity for itself and for the

pleasure derived from the participation

• Obtaining knowledge: “I experience pleasure and satisfaction from learning new things”

• Experiencing stimulation: “I feel intellectually stimulated from the class”

• Sense of accomplishment: “I feel satisfaction from completing difficult academic activities

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2. Extrinsic Motivation- Engaging in an activity as a means to an end, and

not for its own sake

• Identification: “I think that a college education will help me better prepare for the career I am pursuing.”

• Introjection: “To show myself that I am an intelligent person.”

• External regulation: “In order to obtain a more prestigious job later on.”

3. Amotivation- Uninterested and unsure as to why you are

engaging in activities.

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Why Do Some Students Struggle With Chemistry?

• Chemistry is often called “The Central Science”. This is because its main focus is the study of matter, which is essentially anything and everything! Chemistry is connected and related to all other natural sciences.

• In order to understand matter, we must understand what it is made of at the atomic/molecular level.

I believe that some students struggle with chemistry becauseof the visual disconnect they have between what they physically see, and what the matter actually looks like at the atomic/molecular level.

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Granule of table salt

3-D “lattice”of gajillions ofalternatingpositive andnegative ions

An ionic compound

• The ions are stuck together strongly due to attractive electrostatic forces.

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A molecular (covalent)compound

Granules of table sugar (sucrose)

Gajillions of sugar moleculespackedcloselytogether.

C12H22O11

• The atoms of the sugar molecule are held together by covalent bonds. Each sugar molecule “sticks to another through attractive forces.

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Glass of pure water

Gajillions of water moleculestumbling about each other

H2O

OH H

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Solid NaCl Aqueous Na+ and Cl-

ion solution

When ionic compounds are placed in water, the water molecules can pull the ions apart. The ions have dissociated

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=

When most molecular compounds are placed in water, the water molecules pull only the intact sugar molecules apart. No covalent bonds are broken!

Solid sugar Aqueous sugarsolution

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• Solution: A homogeneous (uniform) mixture composed of two or more substances, typically a solvent and a solute

• Solvent: The substance in a solution that does the dissolving

• Solute: The substance in a solution that is being dissolved

Definitions

In this course, we deal primarily with solutions that are aqueous, meaning that the solvent is water.

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Measurement and Significant Figures (Ch. 1.6-1.8)

• In science, it is important to report data with as much certainty as possible. The more significant figures (digits) a number has, the greater its certainty.

The amount of significant figures you can record froma measurement depends on the accuracy of the device.

1. A digital instrument provides a definite amount of certainty.

- A balance that reads 35.126 g gives 3 decimal places of certainty, and all digits are significant

- If the balance reads 100.000 g, all 6 digits must be reported

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2. An analog device (scaled) is more complicated when it comes to significant figures

- The amount of certainty provided by these types of devices depends on how many incremental markings there are.

You must report all digits that are absolutely certain, PLUSa last digit which is estimated

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10.0

11.0

25.3

25.4

25.5

25.6

3

4

5

6

1.014

1.015

1.016

1.018

1.017

7

A B

C D

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• Counting Significant Figures (sig. figs.)

1) All non-zero digits are significant– 1.5 has 2 sig. figs.

2) Interior zeros are significant– 1.05 has 3 sig. figs.

3) Leading zeros are NOT significant– 0.001050 has 4 sig. figs

4) Trailing zeros may or may not be significant

a) Trailing zeros after a decimal point are significant

- 1.050 has 4 sig. figs.

b) Zeros at the end of a number without a written

decimal point are ambiguous and should be avoided

by using scientific notation

- 150 has 2 sig. figs. then 1.5 x 102

- but if 150 has 3 sig. figs. then 1.50 x 102

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• Adding and Subtracting Sig Figs.

When adding or subtracting measurements with significant figures, the result has the same number of decimal places as the measurement with the fewest number of decimal places

• Multiplying or Dividing Sig Figs.

When multiplying or dividing measurements with significant figures, the result has the same number of significant figures as the measurement with the fewest number of significant figures

• Exact Numbers: they have no uncertainty and thus have no impact on sig fig calculations

Eg. Discrete numbers, defined quantities, and integral parts of an equation

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Classification of Matter (Ch. 1)

• Atom: Atoms are submicroscopic particles that constitute the fundamental building blocks of matter.

The structure of an atom consists of a nucleus of neutral particles called neutrons (no), and positively charged particles called protons (p+), which is surrounded by a cloud of negatively charged particles called electrons (e-).

nucleusElectroncloud

“Realistic” Atom “Cartoony” Atom

An atom that has gained or lost an electron(s) is calledan ion

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• Element: A substance that cannot be broken down into simpler substances. An element consists of only one type of atom.

• Compound: a type of matter composed of two or more different elements (atoms) that are chemically bound together.

There are 7 elements that exists as diatomic molecules

• Molecule: an independent structural unit consisting of two or more atoms that are chemically bound together. The atoms bound together can be the same, or different.

• Substance (pure substance): forms of matter with fixed composition.

All items above have fixed compositions, and therefore are all considered to be substances

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• Mixture: something that consists of two or more substances that are only physically intermingled. The ratio of different substances in a mixture is not fixed

- Homogeneous mixture: a mixture that is uniform in appearance and has the same physical properties throughout.

- Heterogeneous mixture: a mixture that is non-uniform consisting of 2 or more physically distinct phases.

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Physical States of Matter

• Solid: at a molecular level, the particles making up the solid are close together, highly organized and have little motion, giving the solid a physical shape that does not change. Solids have definite volume and have a surface

• Liquid: the particles are close together but have motion, tumbling about each other, and therefore its physical shape can change to fill the shape of its container. It has definite volume, and can create a surface

• Gas: the particles are far apart, disorganized, and moving rapidly, allowing gases to expand to fill its container (diffusion). Gases have no definite shape and volume, and therefore do not create a surface

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Gases are compressible, whereas solids and liquids are not,due to the tight packing of the particles

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Compounds and Chemical Bonding (Ch. 3)

• Ionic Compounds: consist of a positively charged ion (cation) and a negatively charged ion (anion). Ionic compounds are typically formed from the reaction of a metal element with a non-metal element.

All ionic compounds are solids, and consist of 3-Dlattices of alternating ions

The force holding the ions togetheris called an ionic “bond”. (But it’s really more of a force than a bond)

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- During the reaction to form an ionic compound, the metal atoms lose electrons to the non-metal atom to become cations.

• Electron Transfer

• Valence Electrons of Main Group Elements

- Valence electrons are the electrons of an element/atom in the outermost “shell” of the atom.

- In Main Group elements (1A-8A), the number of valence electrons matches the group number.

During formation of a compound, the atoms gain or lose electrons to look similar in electron structure to the stable, noble gases in the 8th group of the periodic table octet rule

- The non-metal atoms gain electrons becoming anions

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The Periodic Table

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• Molecular (Covalent) Compounds: Formed from non- metal atoms covalently bonded together. Valence electrons between atoms are shared to form the covalent bond

Molecular compounds are extremely varied in their physical nature. A single molecule can be as simple as consisting of 2 atoms, to thousands of atoms in proteins, or millions of atoms in a strand of DNA.

Hemoglobin

Portionof DNA

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Chemical Nomenclature (Ch. 3.5)

• Binary Ionic Compounds:

- If a transition metal is present that can form more than one type of cation charge

- If a polyatomic ion is present, the name of the polyatomic ion is simply stated followed by the name of the cation

• Ionic Compounds Containing Polyatomic Ions:

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• Monatomic Ions: Ion species consisting of 1 atom

• Polyatomic Ions: Ion species consisting of two or more atoms that are covalently bonded together and have net positive or negative charge.

For this course we will require you to memorize thechemical formula and charge of 11 common polyatomic ions

- Nitrate

- Nitrite

- Sulfate

- Sulfite

- Carbonate

- Bicarbonate or hydrogen carbonate

- Hydroxide - Perchlorate

- Phosphate

- Acetate

- Ammonium

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• Hydrated Ionic Compounds:

- Some ionic compounds trap water molecules within their 3-D lattice

- A certain number of water molecules are associated with each formula unit of the ionic compound, and is denoted using a Greek prefix followed by the word hydrate (all in one word)

• Greek prefixes from 1 – 10: mono, di, tri, tetra, penta, hexa, hepta, octa, nona and deca (if ½ of a hydrate “hemi”)

Eg. Magnesium sulfate heptahydrate MgSO4 • 7H2O

Dot after compounddenotes waters of hydration

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• Binary Molecular Compounds:

- 1st element is the one that is most left and down in the periodic table

- Keep in mind that although the 2nd element gets an “ide” ending, it is not an ion.

- If the number of 1st element atoms is 1, the “mono” prefix is left out.

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• Naming Acids (Inorganic Acids)

- Binary Acids: Composed of hydrogen and a non-metal

- Oxyacid (Oxoacid): Contain hydrogen and an oxyanion, which is a polyatomic ion consisting of a non-metal and oxygen

- If oxyanion ends in –ate:

- If oxyanion ends in –ite:

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- Avogadro hypothesized that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. This hypothesis is known as Avogadro’s Law.

1 mole = 6.022 x 1023 entities (atoms, molecules, units, etc)

But Why?

- Carbon is regarded as the most significant element since all life is based on this atom. Scientist standardized the mole to be equal to the number of atoms in exactly 12.00 grams of pure carbon-12 (which is 6.022 x 1023 atoms)

The Mole Concept (Ch. 2)

- This number is called Avogadro’s number to honor the man who first made the connection of equal quantities of particles for a certain quantity of substance

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Formula Mass (Ch. 3)

• The Periodic Table of Elements:

11

NaSodium

22.99

Atomic number

Symbol

Name

Atomic mass

The atomic mass represents the mass of one atom of the element, and is given units called “atomic mass units” or amu.

- A compound’s mass can be approximated by adding together the atomic masses of all atoms in the chemical formula

Ionic Compounds Formula mass or formula weightMolecular Compounds Molecular mass or molecular weight

- Molar mass: the mass of a substance per mole (g/mol)

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Aqueous Solution Chemistry (Ch. 4)

Water is a polar molecule, meaning oneend has more negative charge character,and the other end has more positive chargecharacter.

- Water can create favorable interactions with substances that are also polar or charged, such as ionic compounds.

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- If an ionic compound is soluble in water, it is because the water molecules slowly “take apart” and surround each individual ion.