The World of Chemistry

The Language of Chemistry CHEMICAL ELEMENTS - pure substances that cannot be decomposed by ordinary means to other substances. Aluminum Bromine Sodium

The Nature of Matter Gold Mercury There are 90 naturally occurring elements.

Aluminum + Bromine

The Language of Chemistry The elements, their names, and symbols are given on the PERIODIC TABLE How many elements are there? 116 elements

The Periodic Table Dmitri Mendeleev (1834 - 1907)

Glenn Seaborg (1912-1999 ) Discovered 8 new elements. Only living person for whom an element was named. Seborgium

Copper atoms on silica surface. An atom is the smallest particle of an element that has the chemical properties of the element. Copper atoms on silica surface. Distance across = 1.8 nanometer (1.8 x 10-9 m)

The Atom nucleus (of protons and neutrons) An atom consists of a nucleus (of protons and neutrons) electrons in space about the nucleus. Electron cloud Nucleus

CHEMICAL COMPOUNDS are composed of atoms and so can be decomposed to those atoms. The red compound is composed of • nickel (Ni) (silver) • carbon (C) (black) • hydrogen (H) (white) • oxygen (O) (red) • nitrogen (N) (blue)

A MOLECULE is the smallest unit of a compound that retains the chemical characteristics of the compound. Composition of molecules is given by a MOLECULAR FORMULA H2O C8H10N4O2 - caffeine

Elements form Compounds

Graphite — layer structure of carbon atoms reflects physical properties.

Kinetic Nature of Matter Matter consists of atoms and molecules in motion.

Physical Properties What are some physical properties? color melting and boiling point odor

Physical Changes Some physical changes would be boiling of a liquid melting of a solid dissolving a solid in a liquid to give a homogeneous mixture — a SOLUTION.

DENSITY - an important and useful physical property Aluminum Platinum Mercury 13.6 g/cm3 21.5 g/cm3 2.7 g/cm3

Relative Densities of the Elements Density of pure water at 25o C is 0.997 g/cm3

Problem A piece of copper has a mass of 57. 54 g. It is 9 Problem A piece of copper has a mass of 57.54 g. It is 9.36 cm long, 7.23 cm wide, and 0.95 mm thick. Calculate density (g/cm3).

Strategy 1. Get dimensions in common units. 2. Calculate volume in cubic centimeters. 3. Calculate the density.

Note only 2 significant figures in the answer! SOLUTION 1. Get dimensions in common units. 2. Calculate volume in cubic centimeters. 3. Calculate the density. (9.36 cm)(7.23 cm)(0.095 cm) = 6.4 cm3 Note only 2 significant figures in the answer!

Problem: Liquid nitromethane is used as a fuel for rockets and race cars. It has a density of 1.13 g/cm3. What is the mass, in grams, of 56L of the fuel? Must convert the liters to cm3

Answer M = 63000 g

DENSITY Density is an INTENSIVE property of matter. does NOT depend on quantity of matter. temperature Contrast with EXTENSIVE depends on quantity of matter. mass and volume. Brick Styrofoam

PROBLEM: Mercury (Hg) has a density of 13. 6 g/cm3 PROBLEM: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg in grams? In pounds? Solve the problem using DIMENSIONAL ANALYSIS.

1. Use density to calc. mass (g) from volume. PROBLEM: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg? First, note that 1 cm3 = 1 mL Strategy 1. Use density to calc. mass (g) from volume. 2. Convert mass (g) to mass (lb) Need to know conversion factor = 454 g / 1 lb

2. Convert mass (g) to mass (lb) PROBLEM: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg? 1. Convert volume to mass ( 95 cm3 )(13.6 g/cm3) = 1.3 x 103 g 2. Convert mass (g) to mass (lb)

Chemical Properties and Chemical Change Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.

Types of Observations and Measurements We make QUALITATIVE observations of reactions — changes in color and physical state. We also make QUANTITATIVE MEASUREMENTS, which involve numbers. Use SI units — based on the metric system

UNITS OF MEASUREMENT Use SI units — based on the metric system Length Mass Time Temperature Volume Meter, m Kilogram, kg Seconds, s Kelvins, K Liter, L

Units of Length 1 kilometer (km) = ? meters (m) 1 meter (m) = ? centimeters (cm) 1 centimeter (cm) = ? millimeter (mm) 1 nanometer (nm) = 1.0 x 10-9 meter O—H distance = 9.58 x 10-11 m 9.58 x 10-9 cm 0.0958 nm

Temperature Scales Fahrenheit Celsius Kelvin Anders Celsius 1701-1744 Lord Kelvin (William Thomson) 1824-1907

Temperature Scales Fahrenheit Celsius Kelvin 32 ˚F 212 ˚F 180˚F 100 ˚C Boiling point of water 32 ˚F 212 ˚F 180˚F 100 ˚C 0 ˚C 100˚C 373 K 273 K 100 K Freezing point of water Notice that 1 kelvin degree = 1 degree Celsius

Temperature Scales 100 oF 38 oC 311 K oF oC K

Calculations Using Temperature Generally require temp’s in kelvins T (K) = t (˚C) + 273.15 Body temp = 37 ˚C + 273 = 310 K Liquid nitrogen = -196 ˚C + 273 = 77 K