Name: The Nature of Chemistry - Lundquist · PDF fileName: _____ The Nature of Chemistry ......

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TheNatureofChemistryUnit 1 (s e ve n c la s s p e r io d s )

Unit 1.1: Lab Safety

1) Key safety protocols

a) DO NOT clean up broken glass – alert your teacher immediately and stand clear

b) Alert your teacher in the event of a spill

c) Wash your hands after every lab

d) DO NOT EAT OR DRINK IN THIS LAB EVER

e) Wear your goggles when working with any fluids

f) Fire extinguishers are to be used on inanimate objects only since they displace oxygen with carbon dioxide

g) Fire blankets are used on living organisms

i) Cover yourself in the fire blanket and tackle a person who is on fire

h) If a reactant makes contact with your skin rinse the area with cool water for 15 minutes

i) A complete run down of safety protocols is available at: https://www.youtube.com/watch?v=0zHev9iM8kU

2) Material Safety Data Sheets

a) Cataloged system for information on chemicals and mixtures

b) Details handling, storage, emergency procedures, and transportation guidelines

c) Sectioned off into segments.

d) Can use various visual systems

Unit 1.2: Introductions

1) Chemistry is the study of matter & energy and the changes between the two

2) Everything is made of chemicals

3) A chemical is any substance that is made of the same stuff no matter where it comes from (the Law of Definite

Proportions)

a) If a chemicals composition changes it is called a chemical reaction

b) Many are reversible

4) The phase of a substance is a representation of how attracted its atoms are for one another.

a) Solid (s) – atoms VERY close together, strongest attraction for themselves; fixed volume and shape.

b) Liquids (l) – atoms close together; strong attraction for themselves; fixed volume.

c) Gas (g) – atoms FAR apart; NO attraction for other atoms; easily compressed.

5) Chemicals can change both physically and chemically

a) Physical changes don’t change the substance

i) Affect the physical properties of a substance

(1) The arrangement, location, and speed of the particles can change

(2) Properties can be:

(a) -Intensive – independent of how much you have

(b) -Extensive- Change with the amount of the substance you have

(c) -Quantitative-a number

(d) -Qualitative-an opinion

b) Chemical changes result in the substance being consumed to produce a new substance

i) Known as chemical reactions

ii) Reactants are what is being used

iii) Products are what is being produced

iv) Signs of a chemical change

(1) Formation of a gas

(2) Formation of a solid (precipitate)

(3) Change in temperature

(4) Change in color

(5) Production of light

6) Matter

a) Any substance with a mass, volume and inertia; everything you see around you except light.

i) How much space an object occupies is its volume

ii) How much of the object there is present its mass

(1) Mass ≠ weight

(2) Mass = amount of matter; taken with a balance

(3) Weight = effect of gravity on that matter; taken with a scale

7) Units

a) Base Units -- Simplest Explanation; 2-D

b) Derived Units --Mathematically altered base units

i) Volume – the amount of space a substance occupies

�� = ��ℎ( �) ×��ℎ( �) × ℎ�ℎ( �)

1cm3 = 1cc = 1mL

ii) Density – amount of stuff in a set space

(1) Denser objects sink below those less dense

(2) �� = 1.00�

��

(3) Measure of how spread out the particles are

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8) The Metric System

a) Prefixes based

on powers of 10

b) You must know

giga- to nano-

Example 1

A gold colored ring has mass of 18.9 grams and a volume of 1.12mL. If the density of gold is 19.3 g/mL is the ring pure

gold?

Example 2

Given the experiment to the right, what is the density of rebar using the water displacement method?

9) Classification of Matter

a) All matter is made up of only about 110 different kinds of atoms.

i) Atoms are incredibly small (largest atom is 564 attometers, that’s 5.64 x 10-16

meters, in diameter

ii) All atoms that have the same properties are called elements

(1) Elements are given an atomic symbol that consist of 1 capital letter and usually a lower case letter

(2) Oxygen = O; Aluminum = Al; Gold = Ag

b) A group of elements bound together chemically is a compound

c) Subscript denotes the numbers of atoms of that element are present in a representative unit of that compound.

(ex: Table salt, NaCl; sugar, C12H22O11)

d) Pure Substance -- one element or one compound; identified by its unique chemical or physical properties.

e) Molecules -- compounds but do not have to be different elements, and can be as few as 1 atom

i) Monoatomic elements – Helium (He)

ii) Diatomic elements – Bromine (Br2), Iodine (I2), Nitrogen (N2), Chlorine(Cl2), Hydrogen (H2),Oxygen (O2),

Fluorine (F2),

iii) Common molecules – Carbon dioxide (CO2), water (H2O)

f) Mixtures are a combination of 2 or more pure substances,

and can be either heterogeneous or homogenous

i) Homogenous mixtures have the same concentration of

pure substances throughout their volume. (air, Kool-

Aid)

ii) Heterogeneous mixtures have area of higher

concentration of pure substances in certain areas

throughout their volume (soil, oil & water)

iii) Mixtures can be separated by the physical properties

of the pure substances that compose them.

Example 3

a.) Convert 1.98kg to grams

b.) Convert 300ml to L

c.) Convert 20J to MJ

d.) 634Gbytes to cbytes

iv) Filtration – separation based on phase (solid vs aqueous/liquid)

v) Distillation – separation based on boiling point

vi) Chromatography – separation based on attraction for a solvent (separates dyes)

Unit 1.3 Scientific Investigation

1) Scientific Method

a) Procedure for observing a phenomenon the testing hypothesizes on why it happens.

i) Hypothesis is a prediction based on observation (NO GUESSING). If… then.

ii) Experiments alter only the ONE variable being tested

(1) Independent variable – the variable you are altering; graphed on the X-axis

(2) Dependent variable – the variable that you are observing; graphed on the Y-axis

(3) Control – a group that does not receive the independent variable; shows that the phenomenon doesn’t

happen all on its own.

b) Scientific theories develop in an attempt to explain WHY a phenomenon occurs

c) Scientific Laws are a summation of several observations

2) Accuracy vs Precision

a) Accuracy is how close datum is to an accepted data point

b) Precision is how close data are to other trials.

3) Percent Error

a) Error -- How off you are on a value

b) Percent Error -- what percentage of the

overall experiment were you off by?

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| �'�� − �)'�#�� |

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4) Numbers

a) Whenever reading an analog instrument (graduated cylinder, thermometer) in chemistry you have to produce

an estimated digit.

b) This last digit is where precision runs out, it represents the last known number

c) Significant digits are all known values.

i) Used in rounding an reporting numbers in science

ii) A number is significant if it is:

(1) A Non-Zero (1 – 9)

(2) A Zero “sandwiched” between 2 significant digits (1002)

(3) A Zero to the right of a decimal AND at the end. (0.0010)

d) Where to round

i) ONLY Round your answers, never round during a calculation

ii) Don’t double round (3.48 = 3 not 4)

iii) When multiplying or dividing, round to the least number of sig. figs you’re given.

iv) When adding or subtracting, round to the least number of decimal places

from the numbers you’re given.

Example 4

How many significant digits are in each number

a.) 20

b.) 20.0

c.) 0.810

d.) 100.

e.) 0.00156000

f.) 6.01 x 103

Example 5

Round each expressions product correctly

a.) 4.56 m x 1.4 m =

b.)*++�

,.-.�/=

c.) 12.011 mL + 18.0 mL + 1.013 mL =

d.) 543 g – 4.98 g

Example 9

A student calculates the density of water to be 0.9g/mL, what is their percent error if the density of water is known

to be 1.0g/mL

v) Exceptions to sig. figs. – numbers with INFINITE sig. figs.

(1) Counting numbers -- If you count out something

(2) Known constants – pi (π),Numerals (dozen, pair, mole), Atomic masses

e) Scientific Notation

i) Based on powers of ten

ii) Rules:

(1) Coefficient must be between 1 & 9

(a) USE ONLY SIG FIGS

(2) Exponent

(a) Decimal moves left = +

(b) Decimal moves right

Example 6

Express each number in scientific notation

a.) 0.012

b.) 4201

c.) 0.00740

d.) 100

e.) 0.0000012

f.) 45.07

Example 7

Write out each number

a.) 1.65 x 10-3

b.) 9.4 x 10-1

c.) 5.46 x 107

d.) 6.6 x 100

e.) 7.1012 x 102

f) Dimensional Analysis (Factor Label Method)

i) multiplying by conversion factors to cancel out unwanted units and derive an answer

5) The periodic Table

a) Metals – group 1 to 13ish

i) Shiny, conduct energy, solids (usually)

b) Nonmetals – groups 14ish to 18

i) Dull, insulators, gasses (usually)

c) Metalloids – separate the two

i) Shiny, insulators, solids

d) Group 1 Alkaline metals – explode in water

e) Group 2 alkaline earth metals

f) Group 16 – Chalcogens

g) Group 17 – Halogens – extremely reactive

h) Group 18 – Noble gasses -- inert

i) Groups 3 – 12 are Transition metals

Example 8

a.) How many inches is 0.3miles?

b.) What is 90mph as ft/sec

1 ft = 12 inch 1 mile = 5280 ft 1 hr = 3600 sec

Put each underlined word (group of words) or numbers in the appropriate one of the five category columns below.

SolidSitting on the desk is a heavy 38.1 g solid cube has a small volume of 2.0 ml, has a melting point of 3818¼C and has a high density of 19.05 g/ml. The cube is shiny silver-color and is soft. It currently has a temperature of 24.5¼C. It burns in air and is ductile and malleable. It slowly decomposes in water, and reacts with acids but not bases.

LiquidThe beaker holds a large volume of 250.0 ml of a blue-colored liquid which has a boiling point of 112¼C and has a density of 1.15 g/ml. The mass in the beaker is 287.5 g and its temperature is very hot. The liquid is volatile (evaporates easily) and is not flammable.

GasThe instructor is holding a big 35 L balloon filled with a gas less dense than air. The gas is odorless and colorless. It is explosive, and has a current temperature of 25¼C .

chemical

propertiesphysical propertiesphysical properties

intensiveintensive extensiveextensive

qualitative quantitativequantitative qualitative

P 2.1 (pg 1 of 2) Properties: Chemical vs Physical

Extensive vs Intensive Name________________________

Quantitative vs Qualitative Density Worksheet Nam e_________________________Per io d _______

Density is t h e ratio o f t h e mass o f t h e sub st an ce t o t h e volume o f t h e sub st an ce at a

g iven t em p erat ure. D= m ass/vo lum e. Den sit y h as un it s o f g/ cm3 or g/ml , o r an y m ass o ver vo lum e un it .

In science we usually use g/mL f o r liq u id s an d so lid s, an d g/L f o r gases. Den sit y is an intensive physical p ro p er t y. It

rem ain s t h e sam e n o m at t er t h e sam p le size. But it w ill vary w it h ch an ge in temperature. Mo st su b su st an ces w h en

o b ject get h o t t er , t h eir vo lum e get s larger . Wi t h t h e sam e m ass b ein g d ivid ed b y a larger vo lu m e, t h e d en sit y

w ill d ro p . As t h ey co o l, t h e d en sit y w ill r ise.

1. A go ld -co lo red r in g h as a m ass o f 18.9 g ram s an d a vo lu m e o f 1.12 m L. Is t h e r in g p ure go ld ? (Th e d en sit y o f

go ld is 19.3 g/m L.)

2. . Pum ice is vo lcan ic ro ck t h at co n t ain s m an y t rap p ed air b ub b les. A 225gram sam p le o ccu p ied 236.6 m L. Wh at

is t h e d en sit y o f p um ice? Will p u m ice f lo at o n w at er? Th e d en sit y o f w at er is 1.0 g /m L. @ ro o m t em p . Will i t

f lo at in gaso lin e ? Th e d en sit y o f gaso lin e is 0.66 g /m l

3.Wh at vo lum e (in Lit ers) w o uld a 0.871 g ram sam p le o f air o ccup y if t h e d en sit y o f air is 1.29 g/L?

4. A cup o f sugar h as a vo lum e o f 237 m L. Wh at is t h e m ass o f t h e cup o f sugar if t h e d en sit y is 1.59 g /m L?

5. A cru m p et recip e calls f o r 175 gram s o f f lo ur . Acco rd in g t o Ju lia Ch ild 's d at a, t h e d en sit y o f f lo ur is 0.620 g/m L.

Ho w m an y m L o f f lo ur are n eed ed f o r t h is recip e?

6. Fro m t h eir d en sit y values, d ecid e w h et h er each o f t h e f o llo w in g sub st an ces w ill sin k o r f lo at w h en p laced in

sea w at er , w h ich h as a d en sit y o f 1.03 g /m L. (Th e m o re d isso lved p ar t icles in t h e w at er , t h e m o re d en se t h e

w at er b eco m es.)

Gaso lin e 0.66 g /m L

Asp h alt l.2 g /m L

Mercu ry 13.6 g/m L

Co rk 0.26 g/m L

Dist i lled w at er 1.00 g/m l

Rub b in g alco h o l 0.78 g.m l

7. A sam p le o f lead is f o un d t o h ave a m ass o f 32.6 g. A grad uat ed cylin d er co n t ain s 2.8 m L o f w at er . Th e w at er

d isp lacem en t m et h o d allo w s yo u t o f in d t h e vo lum e o f a so lid sam p le. Wh en yo u d ro p t h e so lid in t o t h e w at e r

it w ill d isp lace t h e am o un t o f w at er t h at is eq ual t o t h e vo lum e o f t h e so lid . Af t er t h e lead sam p le is ad d ed t o

t h e cylin d er t h e w at er level read s 5.7 m L. Calcu lat e t h e d en sit y o f t h e lead sam p le in gram s/m l.

8. A p iece o f m agn esium is in t h e sh ap e o f a rect an gle & h as a h eigh t o f 2.62 cm

a w id t h o f 1.34 cm an d a len gt h o f 5.22cm . Wh at is t h e vo lum e o f t h e Mg t o t h e co r rect n um b er o f sign if ican t

d ig it s?

If t h e m agn esium sam p le h as a m ass o f 32.6 g, w h at is t h e d en sit y o f t h e sam p le?

Label each box with the labels:¥ pure substance OR mixture¥ atoms AND/OR molecules¥ element AND/OR compound

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P 2.2 (pg 1 of 2) Using the Vocabulary Name__________________________

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