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Chemical properties

Basic Chem Review

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Chemistry
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Chemistry
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Chemical properties
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Hydroxide
PH
Chemical bond
Hydrogen
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ion
Proton
Technology
behavior
Human development
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Psychoanalysis
Attachment theory
Ethology
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Atoms: An atom has 7 protons, 7 electrons, and 8 neutrons. Fill in the blanks below for this atom: Atomic Number _______ Mass number: _______ Charge: ________ This atom belongs to which element? Notation Atomic # Mass # # protons # neutrons # electrons Types of Bonds: Determine the Type of Bond. Hydrogen and Oxygen type of bond = __________________ Carbon and Hydrogen type of bond = __________________ Sodium and Chlorine type of bond = __________________ Solutions/Molarity Practice What is the molarity if 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution? What is the molarity if 734 grams of lithium sulfate (Li2SO4) are dissolved to make 2500 mL of solution?

Basic Chemistry Review

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Chemistry
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Chemistry
Bases
Chemical properties
Cations
Physical chemistry
Hydroxide
PH
Chemical bond
Hydrogen
Hydronium
ion
Proton
Technology
behavior
Human development
Interpersonal relationships
Love
Psychoanalysis
Human behavior
Attachment theory
Evolutionary biology
Personal life

Atoms: An atom has 7 protons, 7 electrons, and 8 neutrons. Fill in the blanks below for this atom: Atomic Number _______ Mass number: _______ Charge: ________ This atom belongs to which element? Notation Atomic # Mass # # protons # neutrons # electrons Types of Bonds: Determine the Type of Bond. Hydrogen and Oxygen type of bond = __________________ Carbon and Hydrogen type of bond = __________________ Sodium and Chlorine type of bond = __________________ Solutions/Molarity Practice What is the molarity if 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution? What is the molarity if 734 grams of lithium sulfate (Li2SO4) are dissolved to make 2500 mL of solution?

Semester 1 Final Study Guide

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Chemistry
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Chemistry
Physics
Chemical bonding
Quantum chemistry
Atomic physics
Chemical properties
Molecular physics
Chemical bond
Valence electron
ion
Lewis structure
electron
Technology

Chemistry Final Exam Study Guide, Chapters 1-8 Chapter 1. Matter and Change Chemistry ? the study of matter and its changes Branches of Chemistry ? 1. Organic Chemistry ? substances containing carbon 2. Inorganic Chemistry ? substances not containing carbon 3. Biochemistry ? chemistry of living things DNA, protein, lipids, carbohydrates 4. Physical Chemistry ? properties and changes of matter with respect to energy 5. Analytical Chemistry ? identification of components and composition of matter. 6. Theoretic Chemistry ? creates mathematical models of chemical behavior Chemical ? any substance with a definite composition Mass ? amount of matter Matter ? takes up space and has mass

Chemistry MidTerm Review

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Chemistry
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Chemistry
Physics
Nuclear chemistry
Nuclear physics
Chemical properties
Mass
Baryons
Chemical element
Mass number
Isotope
Atomic mass
Neutron

CP Chemistry Midterm Review List Substance: element & compound ? water, Aluminum, ethanol, carbon dioxide Homogeneous vs. Heterogeneous Physical & Chemical Properties & changes: Freezing/melting, boiling/condensing ;State Change (melting point) Burning/ rusting Metric system: Units, prefixes (kilo-milli), and conversions one milliliter equals 1 cm3 325 mg can be expressed in grams Temperature scales & conversion - Celsius temperature is equivalent to 298K Accuracy vs. precision Scientific Notation & Significant figures 149,000,000 Percent error A molar mass of a compound is 75 g/mol. A student reported an experimental value of 78 g/mol. The percent error is Density

Science history

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Chemical properties
Nuclear physics
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Atomic theory
Atomism
Atomic number
Chemical element
electron
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History of Science ? ? Illusion ? Delusion - Truth I thought this was Science Course Science is the Truth ?. but but ?.. Science seems to change all the time Hmmmm First Quiz From Fire to Atomism Early Greek Atomic Theory Some thought EVERYTHING was made from water in one of the forms (ice, liquid, gas) Democritus ? atoms differed in only shape and size The concept of the ?nocut? atomos was developed ? SMALLEST BUILDING BLOCK Arostotle ? all matter is composed of four elements ? Earth, air, fire, water The philosopher's stone and the rise of alchemy ?convert cheaper metals into gold finding the?elixir of life ?in the air an "ether" which breathed life into living things Problems with Alchemy

Bob Jones PPT Notes -- Chapter 5b

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Chemistry
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Quantum chemistry
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Chemical properties
Atomic physics
Charge carriers
Periodic trends
Chemical bond
Ionization energy
Electronegativity
ion
Technology

Periodic Trends 1 Sizes of Atoms Increase from top to bottom on the periodic table Why? There are higher energy levels, and electrons are farther from the nucleus. Atomic Radii Sizes of Atoms Decrease from left to right on the periodic table Why? There are more protons in the nucleus attracting more electrons (electrostatic attraction). Atomic Radii Atomic Radii 4 p. 113 of Chemistry textbook (BJU Press) Question Why do atoms get larger as you go down the periodic table? They are heavier. They are less dense. Electrons are further from the nucleus. Electrons are bigger. 5 (Comparing the size of an atom to that of its ion, not going across or up the table) Sizes of Atoms Ionic Radii Sizes of Atoms Atoms that lose outer electrons have smaller positive ions (metals).

Bob Jones PPT Notes -- Chapter 4c

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Chemistry
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Chemical properties
Nuclear chemistry
Nuclear physics
Chemical bonding
Mass
Mass number
Atomic mass
Proton
Isotope
Chlorine-37
Technology

Useful Element Notations The number of protons in the nucleus Determines the identity of the atom (which element it is) Atomic Number (Z) If you change the number of protons, the atom changes to another element. The total number of particles in the nucleus?protons and neutrons The total number of particles that make up the mass of the atom Mass Number (A) Atoms of an element which have various amounts of neutrons but the same number of protons Isotopes: Since the number of neutrons changes, the mass of the isotopes is different. Count Those Neutrons It shows the mass number, atomic number, and symbol for the element. Isotopic Notation X A Z Isotopic Notation Example: Be 9 9 protons and neutrons 9 4 4 4 protons Therefore, there must be 5 neutrons. 18 40 22 58 Question

Chapter 3

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Chemistry
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Chemistry
SI base units
Mass
Chemical properties
Analytical chemistry
Molar mass
Mass fraction
Mass spectrometry
Mole
Kilogram
Molecular mass
Molar volume

Chapter 3.1 Average mass= total mass/ number of objects massed 3.2 Mass spectrometer- most accurate method currently availbe for comparing masses of atoms 3.3 Avogadro?s number- 6.022X 10^23 = one mole of something Molar mass- mass in grams of one mole of the compound g/mol Find on periodic table 3.5 Percent comp: Mass/ weight percent= (Mass of element in compound/ mass of compound)X100 3.6 Molecular formula= (empirical formula)n N is an integer To find molec formula take molar mass/ empirical formula mass and that is n SEE PAGE 96 IF CONFUSED
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Chapter 2

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Chemistry
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Chemistry
Science
Physics
Chemical properties
Mass
Stoichiometry
Amount of substance
Atomic mass
Atomic theory
Isotope
Chemical element
Chemical bond

Chapter 2.1- 2.3 (pages 41-48) Law of conservation of mass- Mass is neither created nor destroyed Law of definite proportion- a given compound always contains exactly the same proportion of elements by mass. Law of multiple proportions- When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers Dalton?s Atomic Theory- -Each element is made up of atoms -The atoms of a given element are identical -Chemical compounds are formed when atoms of diff elements combine with each other -Chemical reactions involve reorganization of the atoms Dalton prepared first table of atomic masses

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