General Chemistry
description
Transcript of General Chemistry
![Page 1: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/1.jpg)
General Chemistry
1st Semester Review
![Page 2: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/2.jpg)
Chapter 2
• Qualitative observation: describes matter without using numbers– Ex:
• Quantitative observation: describes matter using measurements– Ex:
![Page 3: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/3.jpg)
Classifying Matter by Composition
• A substance is matter with the same fixed composition and properties– Elements & compounds are substances
• A mixture is a combination of two or more substances in which the basic identity of each substance is not changed.– Can be separated by physical processes
![Page 4: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/4.jpg)
Types of Mixtures
• A heterogeneous mixture does not have a uniform composition and its individual substances remain distinct.– Ex:
![Page 5: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/5.jpg)
• A homogeneous mixture, or solution, always has a uniform composition and is the same throughout. – Ex:
– An alloy is a solid solution that contains different metals and sometimes nonmetallic substances.
![Page 6: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/6.jpg)
Substances: Pure Matter
• There are two types of pure substances—compounds and elements.
![Page 7: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/7.jpg)
Elements: the building blocks
• An element is the simplest form of matter– There are 117 elements – only 90 occur naturally
on earth– The periodic table organizes elements and uses
chemical symbols that are universally understood.
![Page 8: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/8.jpg)
Compounds
• A compound is a chemical combination of two or more different elements joined together in a fixed proportion – Compounds have chemical formulas
![Page 9: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/9.jpg)
![Page 10: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/10.jpg)
Physical Properties
• Physical properties are those that do not involve changes in composition.
• Physical properties can be either quantitative or qualitative
When salt is dropped into water, the particles in the salt crystal
separate and are surrounded by water.
![Page 11: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/11.jpg)
• Physical properties are characteristics of a sample of matter that can be observed or measured without any change to its identity.– Ex:
![Page 12: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/12.jpg)
• A physical change is a change in matter that does not involve a change in the identity of the substance– Phase changes are physical changes!– Ex:
![Page 13: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/13.jpg)
• Most matter on Earth exists in one of three physical states: solid, liquid, or gas.
• Changes in state are examples of physical changes because there is no change in the identity of the substance.
• Some substances are volitile, or change to a gas easily at room temperature.
![Page 14: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/14.jpg)
Chemical properties and changes
• A chemical property can be observed only when there is a change in the composition of the substance
• Chemical change, otherwise known as a, is the change of one or more substances into other substances.
![Page 15: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/15.jpg)
• According to the law of conservation of mass, matter is neither created nor destroyed in a chemical change
![Page 16: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/16.jpg)
Energy & Chemical Changes
• Energy, which is the capacity to do work, is either absorbed or released during a chemical change– Energy has many different forms
![Page 17: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/17.jpg)
Exothermic vs. Endothermic
• Exothermic reactions are chemical reactions that give off energy– Combustion
• Endothermic reactions are chemical reactions that absorb energy– photosynthesis
![Page 18: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/18.jpg)
• Density is the amount of matter (mass) contained in a unit of volume.
• Density is a physical property
![Page 19: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/19.jpg)
• Stays the same for a given substance– Doesn’t matter how much of how little you have
• Many possible units– g/m3, g/L, g/cm3, g/mL
• Density formula:
![Page 20: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/20.jpg)
Sample Problem 1
• What is the density of a substance with a mass of 24.3 g and a volume of 32.9 mL?– Answer must have correct unit
![Page 21: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/21.jpg)
Sample Problem 2
• What is the volume of an object with a density of 125 g/mL and a mass of 281 g?
• What is the mass of an object with a density of 4.36 g/mL and a volume of 500 mL?
![Page 22: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/22.jpg)
Chapter 2 Atomic Theory
![Page 23: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/23.jpg)
Dalton
1. all elements are composed of tiny particles called atoms which CANNOT be divided into smaller parts
2. All atoms of the same element have identical properties. Atoms of different elements have different properties
3. Atoms combine in whole-number ratios to form compounds
4. Chemical reactions take place when atoms rearrange. Atoms of one element are NOT changed into atoms of a different element
![Page 24: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/24.jpg)
Thomson
• Discovered 1st subatomic particle!• Experiment
• Discovery
• Model
![Page 25: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/25.jpg)
Rutherford
• Experiment
• Discovery
• Model
![Page 26: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/26.jpg)
Particle Charge Location Mass
Proton
Neutron
Electron
![Page 27: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/27.jpg)
![Page 28: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/28.jpg)
Atomic Number & Mass Number
• Atomic number = number of protons• Differences among elements result from
different numbers of protons in their atoms
![Page 29: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/29.jpg)
• Mass # = Protons + Neutrons• Electrons are so small they have almost no mass
• Atoms are electrically neutral• # of protons = # of electrons
![Page 30: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/30.jpg)
Ions
• Atoms with electrical charge– Cation = • Forms by:
– Anion = • Forms by:
![Page 31: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/31.jpg)
Isotopes
• Atoms with the same number of protons but different number of neutrons– Oxygen – 16, Oxygen – 17, Oxygen – 18– One isotope is more common than the others
![Page 32: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/32.jpg)
Mass Number
• Distinguishes isotopes
• Protons + Neutrons = Mass Number– (Electrons have almost no mass)
![Page 33: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/33.jpg)
Atomic Shorthand
• Beryllium- - -atomic number 4 mass number 9 m# p = 4 # e = 4 # n = 5
• The atomic number is written as a subscript.• The mass number is written as a superscript.
Be
![Page 34: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/34.jpg)
• P =
• N =
• Electron =
– + ion– - ion
![Page 35: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/35.jpg)
Element Atomic Number
# of Protons
# of Electrons
# of Neutrons
Mass #
2713 Al
2713 Al3+
Oxygen – 16
148O
9 10
20884 Po
53 54 74
![Page 36: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/36.jpg)
Atomic Mass
• Different from Mass Number• Average of the masses of all the isotopes of
the element• Measured in Atomic Mass Units (amu)– Proton = 1 amu– Neutron = 1 amu– Electron = 0 amu
![Page 37: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/37.jpg)
• Nitrogen has 2 naturally occurring isotopes, 14
7N has an abundance of 99.63%. 157N has an
abundance of 0.37%. What is the atomic mass of Nitrogen?
![Page 38: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/38.jpg)
Chapter 3
![Page 39: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/39.jpg)
Energy Levels
• Areas of space where electrons can move
• Closer to nucleus = lower energy• Further from nucleus = high
energy• ELECTRONS CANNOT EXIST
BETWEEN ENERGY LEVELS!!!• Numbered: level closest to
nucleus = 1
![Page 40: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/40.jpg)
• S sublevel = 1 orbital• p sublevel = 3 orbitals• d sublevel = 5 orbitals• f sublevel = 7 orbitals• Each orbital can be filled: (2 e-), half filled: (1
e-), or empty: (0 e-)
![Page 41: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/41.jpg)
Put it all together
• Energy level 1 = closest to nucleus– One sublevel = s– One orbital = 1s
• Energy level 2 – 2 sublevels = s and p– 4 orbitals = 2s, 2px, 2py, 2pz
![Page 42: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/42.jpg)
• Energy level 3– Three sublevels = s, p, and d– Nine orbitals = 3s, 3px, 3py, 3pz, five 3d orbitals
• Energy level 4– Four sublevels = s, p, d, and f– 16 orbitals
• Higher energy levels have all four sublevels
![Page 43: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/43.jpg)
![Page 44: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/44.jpg)
Sample Problems
• What are the electron configurations of the following elements?
• Li
• O
• Cl
![Page 45: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/45.jpg)
Sample Problems
• Co
• Kr
• Ba
![Page 46: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/46.jpg)
Valence Electrons
• Electrons in the s & p orbitals of highest energy level
• Boron: 1s22s22p1
– Highest energy level– Valence electrons
• Scandium: 1s22s22p63s23p64s23d1
– Highest energy level– Valence Electrons
![Page 47: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/47.jpg)
Dot Diagrams
• Valence electrons are the only ones that are involved in chemical reactions
• Dot diagrams show the valence electrons
![Page 48: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/48.jpg)
1.Figure out how many valence electrons element has
2.Write the element symbol3.Add dots to top, right, bottom, and left of
symbol one at a time until all valence electrons are used
4.Remember: each orbital can only hold 2 dots
![Page 49: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/49.jpg)
Element Electron Configuration
# of Valence Electrons
Dot Diagram
Phosphorus
Bromine
Oxygen
![Page 50: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/50.jpg)
Chapter 4
![Page 51: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/51.jpg)
Henry Moseley
• Rearranged the elements according to increasing atomic number– Atomic # =
• Resulted in the structure of the modern periodic table
![Page 52: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/52.jpg)
• Periodic Law – the physical and chemical properties of the elements repeat in a regular pattern when they are arranged in order of increasing atomic number.
![Page 53: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/53.jpg)
Periods and Groups
• 7 horizontal rows = periods– Correspond to outermost energy level
• Vertical columns = groups/families– Correspond to the number of outermost electrons– Have similar properties– Some have special names
![Page 54: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/54.jpg)
Group/Family Names
• Group 1 = Alkali metals• Group 2 = Alkaline earth metals• Group 3 – 12 = Transition metals• Inner Transition metals• Group 17 (VII A) = Halogens• Group 18 (VIII A) = Nobel gases
![Page 55: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/55.jpg)
![Page 56: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/56.jpg)
Physical States and Classes of Elements
• Most elements are solid at room temperature
• Br & Hg are liquid
• N, O, F, Cl, and Noble gases are gas
![Page 57: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/57.jpg)
• Elements are classified as metals, metalloids, or nonmetals based on their properties
![Page 58: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/58.jpg)
• Metals– Located to the left of the stairs– Have luster– Conduct heat and electricity– Usually bend without breaking– Solid at room temperature– Very high melting points
![Page 59: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/59.jpg)
• Nonmetals – located to the right of the stairs– Brittle– Dull looking– Poor conductors of heat and electricity– Usually gases
![Page 60: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/60.jpg)
• Metalloids – have properties of both metals and nonmetals– B, Si, Ge, As, Sb, Te, Po, At– Some are semiconductors – conducts electricity
better than a nonmetal but not as good as a metal
![Page 61: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/61.jpg)
Patterns in Valence Electrons
• Valence electron =
• All elements of a family have the same number of valence electrons
• Increase across a period
![Page 62: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/62.jpg)
Why do atoms form ions?
• Representative elements lose or gain electrons in order to obtain the same electron configuration as a noble gas
![Page 63: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/63.jpg)
Before
• Na– 1s22s22p63s1
• B– 1s22s22p1
• P– 1s22s22p63s23p5
• F– 1s22s22p5
![Page 64: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/64.jpg)
After
• Na1+
– 1s22s22p6 (Ne)
• B3+
– 1s2 (He)
• P3-
– 1s22s22p63s23p6 (Ar)
• F1-
– 1s22s22p6 (Ne)
![Page 65: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/65.jpg)
Bond Types
• Differences in electronegativity determine bond type
• 0 – 0.4 = nonpolar covalent• 0.4 – 1.7 = polar covalent• 1.7 – 3.3 = ionic
![Page 66: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/66.jpg)
Nonpolar Covalent 0 – 0.4
• Electrons equally shared– Directly in the middle of the two atoms
• H2
• O2
![Page 67: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/67.jpg)
Polar Covalent 0.4 – 1.7
• Electrons are shared by not equally– More electronegative atom pulls electrons closer
• HCl
• CCl4
![Page 68: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/68.jpg)
Ionic >1.7
• Electrons not shared at all– Atom with higher electronegativity takes electrons
from atom with lower electronegativity• NaCl
• K2O
![Page 69: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/69.jpg)
Molecule Electronegativity of 1st atom
Electronegativity of 2nd atom
Electronegativity difference
Bond Type
O2
HCl
NaCl
NO3
NH4
![Page 70: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/70.jpg)
Rules for writing dot diagrams of molecules
1. Atoms want 8 electrons in their outer energy levels (octet rule)
2. Number of dots in the molecule = sum of dots in individual atoms
![Page 71: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/71.jpg)
Examples
• CH4
• NH3
• CO2
![Page 72: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/72.jpg)
VSEPR Theory
• V alence• S hell• E lectron• P air• R epulsion
• The shape of a molecule is determined by minimizing repulsion between lone pairs
![Page 73: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/73.jpg)
Linear
• Atoms are in a line• CO2
![Page 74: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/74.jpg)
Trigonal Planar
• Atoms make a flat triangle• CO3
2-
![Page 75: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/75.jpg)
Tetrahedral
• Pyramid shaped• CH4
![Page 76: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/76.jpg)
Trigonal Pyramidal
• A triangle that is not flat• NH3
![Page 77: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/77.jpg)
Bent
• H2O
![Page 78: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/78.jpg)
Naming Flow Chart
![Page 79: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/79.jpg)
• Name the following:– KOH
– Ca(NO3)2
– (NH4)3PO4
![Page 80: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/80.jpg)
– CuCl2
– CoN
– CCl4
– Hg3P2
![Page 81: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/81.jpg)
Formula Writing Flow Chart
![Page 82: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/82.jpg)
• Aluminum Sulfide
• Sodium Phosphate
• Calcium Nitrite
• Barium Oxide
![Page 83: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/83.jpg)
• Carbon Tetrachloride
• Sulfur Hexaflouride
• Tetraphosphorus Decoxide
• Dinitrogen Monoxide
![Page 84: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/84.jpg)
• Iron (III) Sulfate
• Titanium (III) Oxide
• Chromium (III) Carbonate
• Copper (I) Chloride
![Page 85: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/85.jpg)
1000 m = 1km 1000 L = 1 kL 1000 g = 1 kg1 m = 10 dm 1 L = 10 dL 1 g = 10 dg1 m = 100 cm 1 L = 100 cL 1 g = 100 cg1 m = 1000 mm
1 L = 1000 mL 1 g = 1000 mg
1 m = 1000000 µm
1 L = 1000000 µL
1 g = 1000000 µg
![Page 86: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/86.jpg)
Conversions – 1 step
Ex 1: A roll of wire is 15m long, what is the length in cm?
Ex 2: convert 8.96L to milliliters
![Page 87: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/87.jpg)
1 step cont.
• Convert 100 yards to feet
• Convert 5 kilometers to miles
![Page 88: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/88.jpg)
Conversions – 2 step
• The front board is 500 mm long, how long is it in km?
• A football field is 120 yards long, how long is it in miles?
![Page 89: General Chemistry](https://reader035.fdocuments.net/reader035/viewer/2022062501/56816938550346895de0a061/html5/thumbnails/89.jpg)
2 step cont.
• Convert 525 km to cm
• Convert 10000 in to miles