Chem 121 Introduction to Inorganic Chemistry. What is Matter? Matter is anything that has mass and occupies space. Mass is a measurement of the amount.

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Presentation transcript:

Chem 121 Introduction to Inorganic Chemistry

What is Matter? Matter is anything that has mass and occupies space. Mass is a measurement of the amount of matter present. The mass is constant, no matter where it is …on the moon or on earth. Weight the a measurement of the gravitational force pulling the object toward earth. The weight of an object will be different on the moon that has a different grav. pull.

Properties and Changes Two types of properties: – Physical : Those that can be observed or measured without changing or trying to change the composition of the matter in question * no original substances are destroyed and no new substances are created. Like Color and SIZE. – Chemical: properties that matter demonstrates when attmepts are made to change it into other kinds of matter.

Physical Change VS Chemical Change Physical Change: Cutting a piece of paper, Boiling water, freezing water, heat is added or removed from matter. Chemical Change: burn the paper.,mix the water with an acid.

A Model of Matter Scientific Models are explanations for observed behavior. All matter is made up of particles that are too small to see. (molecules) Molecules: The smallest particle of a pure substance that has the properties of that substance and is capable of a stable independent existence. A molecule is also the limit of physical subdivision for a pure substance.

Example Oxygen: helps a substance burn more rapidly..like wood. – A large amt. or a small amt of Oxygen would behave the same. – The smallest amt. that would still behave the same is known as the molecule.

What’s beyond the Molecule? John Dalton wanted to know. In 1808 he proposed the following: 1. All matter is made up of tiny particles called atoms. 2. Substances called elemenats are made up of atoms that are all identical. 3. Substances called compounds are comginations of atoms or two or more elements.

Cont. 4. Every molecule of a specific compound always contains the same number of atoms of each kind of element found in the compound. 5 In chemical reactions, atoms are rearranged, separated, or combined, but are never created nor destroyed.

Types of Molecules Diatomic Molecule: contains two atoms Homoatomic molecule: contain only one kind of atom. Heteratomic molecule: contain more then one kind of atom Triatomic molecule: 3 non-identical atoms Polyatomic molecule: more then 3

Classification of Matter Pure Substances - not adulterated or mixed with anything else. – They have unique and consistent physical and chemical properties. Physical Properties: Melting Point Temperature, Color, Density. Chemical Properties: a chemicals ability to react with other pure substances. In a chemical reaction, substances lose their identity and form new substances with new chemical and physical properties. – It undergoes physical change without losing its identity... Eg.( melting, freezing, or evaporation)

Mixtures Consists of two or more pure substances in varying proportions. – Heterogeneous – visibly discontinuous..like salt and pepper. – Homogeneous – have a uniform appearance throughout; like sugar and water. The mixture is called a solution, and it is described as homogeneous. Mixtures can be separated back into their pure substance components. Mixtures have properties that are variable and depend on the proportions of the components.

Compounds and Elements Compounds: Some pure substances are found to be able to be decomposed into simpler pure substances. Elements: pure substances that cannot be further decomposed. It cannot be separated chemically in to simpler substances, nor be created by combining simpler substances.

Measurement and the Metric System Measure: - the size, capacity, extent, volume or quantity of anything, especially as determined by comparison with some standard or UNIT. Systeme International d’Unite’s.

Significant Figures Communicating Degrees of Uncertainty 4 1 sig fig sig figs sig figs sig figs

Examples Do not over represent the amt. of precision that you have. Which digits are really giving me info about how precise my measurement is? If you measure the above in km, it could also be 7.00 m (the previous zeros are determining the units to use, the trailing zeros determine precision) …(could be re-written as 52 m) (do not count leading zero’s before the first non-zero digit) 370. (because they wrote a decimal, it is exactly 370) 3 sig figs (go to nearest 10 th ) 3 sig figs ( zero’s are part of measurement..between non zero digits) 37,000 (ambiguous) Maybe you measured to the nearest 1000, or nearest 1…you don’t know. Go with 2 sig figs. (more conservative) ( A trailing Zero as in is significant. (This has 4 sig figs)…

Rules of Thumb A trailing zero, 4.130, is significant. A zero within a number, cm A zero before a digit as in 0.082, is not significant A number ending in zero with no decimal point, 20 is ambiguous.

Mulitiplication and Division with Sig Figs Let’s say we are calculating the area of a Rectangle 1.69 m x 2.09m Area = m 2 Use the least precisice number as the basis for the amt. of sig figs.. 3 sig figs.. Area = 3.53 m 2

Another Example Calculate how many tiles I need for a room ft x 10.1 ft. Floor Area = ft 2 ** Do not round yet! *** go to the end with all numbers, then establish sig figs and round** Tiles in bathroom = ft 2 /1.07 ft 2 Tiles = tiles 3 sig figs = 114 tiles

Addition and Subtraction Ex: 1.26 (nearest hundredth, 3 sig figs) (nearest 10 th, 2 sig figs) = 3.56 The least precise number went to the 10 th, therefore 2 sig figs in result. 3.7 Or = (only as precise as the least precise number)… 1.26 has 3 sig figs, has 4 sig figs, however the least precise measurement is as it is measured only to the 10 th, not the 100 th …therefore the answer will be 4 sig figs, 103.6

Another Example One Block: 2.09 m high Another block: m high How tall is it to stack them? = Did I measure the entire stack to the nearst mm? NO! Only report as precise as the least precise measurement. 3.99m

Another example Building: 350 ft tall (ambiguous) Radio Tower : 8 ft tall How tall is building plus the tower: 358 ft We only measured tower to nearest ft. You have to round to the nearest 10 ft. Answer is actually 360 ft. or report it as 3.6 x 10 2

Metric System Units

Using Units in Calculations aka: Dimensional Analysis Step 1: Write Down the known or given quantity. Include both numerical value and units of the quantity. Step 2: Leave some working space and set the known quantity equal to the units of the unknown quantity. Step 3: Multiply the known by one or more factors (conversion factors) to cancel the units of the known and generate the units of the unknown. Step 4: Do the arithmetic.

Example Problems 50 μ L (50 – microliter) sample of blood serum must be expressed as Liters. (1 μ L = 1 x L) Step 1: Step 2: Step 3: Step 4:

Example One of the fastest-moving impulses in the body travels at a speed of 400 ft/per second. (ft/s). What is the speed in miles/hr?

Calculating Percentages Percent = number of specific items x 100 total items in the group % = Part/Total x 100

Non SI units most common

Prefixes for Metric Units

Mass, Volume, & Density Mass is the measure of a quantity of matter. It is measured relative to a standard mass (which is why the devices to weigh an object are called Balances) Mass is not Weight. Volume is the amount of space a sample occupies. 1 mL = 1cm 3 Denisty – a physical property of a substance = mass/volume. Since volume increases with Temperature increase, a density is always reported with a Temperature.

Example A g sample of metal as weighed and put into a graduated cylinder that contained 21.2 mL of water. The water level after the metal was added was 25.2 mL. What is the density of the metal in g/cm 3

How to measure Density Take a substance and weight it. Then add it to a known volume of water in a volumetric flask and notice the volume change in the water as the volume of the substance. Calculate the density. To calculate the mass of a liquid, you add the liquid to a zeroed balance with a volumetric flask and weight the liquid. Then you have the mass and the volume, and you can caluclate the density.

Density Example Problem What is the volume of a 32 g sample of ethanol whose density is 0.789g/cm 3 ? Report volume in cm 3

Hydrometer If something floats on water, it is less dense then water. If something sinks, it is more dense then water. A hydrometer rises or falls to a density that is equal to the density of the liquid. It is calibrated to show the specific gravity of the liquid.

Specific Gravity S.G. = density of test liquid/ density of reference liquid Note that the units cancel. The standard reference liquid for measuring the specific gravity of aqueous solutions is pure water at 4 deg. C. Density is 1.000g/cm 3. S.G. of blood is This means that blood is times the density of pure water.

Temperature Substances can either gain heat or lose it, depending on whether they are cooler or hotter then their environments. To measure heat, we must have an indication of how hot or cold something is…that is the temperature. It indicates how hot something is…not the amount of heat.

Kelvin, C, and F K = C F = 9/5 C + 32 C (F-32)(5/9)

Heat and Calorimetry Heat is a form of energy. Each substance has a different capacity to absorb heat. A unit of heat is defined by its effect (the rise in temperature) on a fixed mass of a reference substance. SI unit = joule, (J) Non-SI commonly used = cal J = 1 cal

Specific Heat : C p The characteristic response of a given mass of a given substance to a given amount of heat is expressed by C p C p = joules/(grams x Δ°C) The specific heat is equal to the heat absorbed or lost per Celsius degree change in temperature per gram of substance.

Specific Heat The higher a substances specific heat, the more slowly it’s temperature rises in repsonse to heating.

Calculating Specific Heat What is the specific heat of a substance if the addition of 334 J of heat to 52 g of that substance causes the temperature to rise from 16 C to 48 C?

Calculating Heat from Cp How much heat must be added to 45.0 g of a substance that has a specific heat of J/gC to cause it’s t to rise from 21 C to 47 C ?

Calorimeter When the heat produced by some physical or chemical process is abosrbed into a given mass of water, the water’s T rise will allow us to calculate the heat produced by the process.

Example What is the Specific Heat (Cp) of an element that takes 50 Joules to heat up 400 grams from 34 deg to 76 deg.?

Calorimeter

Basal Metabolic rate BMR is the minimum metabolic activity of a human at rest and with an empty gi tract. In nutrition and metabolism, heat is more commonly given as calories. The rate means it is the amount of heat over a period of time…expressed in kcal/min.