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Charge carriers

AP Chemistry Zumdahl 7E Chapter 2 Notes

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AP Chemistry A. Allan Chapter 2 Notes - Atoms, Molecules and Ions 2.1 The Early History Refer to the Chemistry History Timeline for this chapter 2.2 Fundamental Chemical Laws A. Law of Conservation of Mass 1. "Mass is neither created nor destroyed" 2. Translation: In ordinary chemical reactions, the total mass of the reactants is equal to the total mass of the products B. Law of Definite Proportion 1. "A given compound always contains the same proportions of elements by mass" 2. Translation: Compounds have an unchanging chemical formula C. Law of Multiple Proportions 1. "When two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers

The History of the Atom - Notes

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The History of the Atom Chapter 5 Major Discoveries 1806: John Dalton Atomic theory 1896 Henri Becquerel Radioactivity 1897: JJ Thomson Discovered the Electron 1909: Robert Millikan Confirmed existence of Electrons, their mass and their negative charge 1910: Ernst Rutherford Nucleus has the protons and neutrons, rest is mostly empty space 1913: Neils Bohr Planetary model of the atom Dalton?s Atomic Theory Elements are made up of discrete units called atoms Atoms of each element are identical. Atoms of different elements are different. Compounds are formed when atoms combine. Each compound has a specific number and kinds of atom. Chemical reactions are rearrangement of atoms. Atoms are not created or destroyed. Becquerel and Radioactivity Discovered by accident

ap_bio_ch_1_2.ppt

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Introductory Questions #1 Name the seven main properties of life. (Pg. 3) Which of the hierarchial levels of biology is the lowest in regard to carrying on and sustaining all life activities and is the fundamental unit of life? (pg 5) Introductory Questions #1 3. In your own words briefly describe what ?emergent properties? are. 4. How is negative feedback different from positive feedback? (pg. 11) What do these mechanisms do for a living thing? 5. Name the three domains of life. Which domain includes four out of the six kingdoms of life? 6. Why is natural selection considered the ?mechanism? for evolutionary adaptations to occur? 7. How is a hypothesis different from a theory?

Atomic Radius

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Atomic Radius: The atomic radius is the size of the atom of an element. The values decrease. Yes, they both decrease. The atomic radius increases. Yes, but they increase at a slower rate. Ionic Radius: An atom becomes a cation when an atom loses electrons in a reaction. An atom becomes an anion when it gains electrons in a reaction. The cations? values decrease. The anion?s values also decrease. Yes, their trends are the same. The ionic radius value increases. Yes, they also increase. Electronegativity: Electronegativity is the measurement of an element?s tendency to react with electrons in a chemical bond. The values greatly increase. Yes, they both increase. The values slowly decrease. No, because only one number in group 18 is plotted.

cell bi chapter 1/2

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Chapter One Characteristics of living organisms Consist of one or more cells Unicellular organisms (1) A single cell carries out all the functions of life Multicellular organisms Made of many specialized cells Consist of genetic information DNA Info molecule Passed on during cell division Composed of nucleotides Genetic code Gene Specific segment of DNA molecule Contains info to make proteins Proteins Control chemical reactions Cell/organism structure and function Use genetic information to reproduce Use genetic information for growth and development Can extract energy from the environment and use it to do biological work Can convert molecules obtained from their environment into new biological molecules Can respond to environmental changes

General Chemistry Study Exam

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Human behavior
Attachment theory
Evolutionary biology
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[Type text] [Type text] [Type text] May 14, 2014 Chemistry Study Guide Abby & Thomas Chapter 8: 8.1 Vocabulary Covalent bond- a bond formed by the sharing of electrons between atoms Molecule- a neutral group of atoms joined together by covalent bonds Diatomic molecule- a molecule that contains two atoms Example. Oxygen and Hydrogen Molecular compound- a compound composed of molecules Example. Water Molecular formula- the chemical formula of a molecular compound. A molecular formula shows how many atoms of each element a substance contains Important things to know for 8.1 8.2 Vocabulary Single Covalent bond- a bond formed when two atoms share one pair of electrons

Chapter 6- Chemistry in Biology

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Chapter 6-Chemistry in Biology COMPOSITION OF MATTER -Matter-everything in universe is composed of matter. -Matter is anything that occupies space or has mass -Mass-quantity of matter in an object -Weight-pull of gravity on us ELEMENTS -Pure substances that cannot be broken down chemically into simpler kinds of matter -More than 100 elements (92 naturally occuring) -90% of the mass of an organism is composed of 4 elements (oxygen, carbon, hydrogen, and nitrogen) -Each element has a unique chemical symbol -Consists of 1-2 letters -First letter is always captialized ATOMS -The simplest particle of an elemetnt that remains all the properties of that element. -Properties of atoms determine the structure and properties of the matter they compose.

Bob Jones PPT Notes -- Chapter 5b

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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).

Chemistry The central science Summary Chapter

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Lewis Symbols As a pictorial understanding of where the electrons are in an atom, we represent the electrons as dots around the symbol for the element. The number of electrons available for bonding are indicated by unpaired dots. These symbols are called Lewis symbols. Place the electrons on four sides of a square around the element symbol.
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Chemistry

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Chemistry Study Guide Unit 1: Measurement and the Methods of Chemistry Counting significant figures: 1) leading zeros never count 2) Trailing zeros only count if there is a decimal point written 3) All numbers that aren?t leading or trailing zeros count Unit 2: Atomic Structure, Periodicity, and Nuclear Energy Proton: +1 (charge) Neutron: 0 (charge) Electron: -1 (charge) Atomic number= number of protons within an atom Atomic mass= total weight of the atom. P+N If there is a power to the left of the element, that implies the mass. Isotope: same atom with same atomic number, but different number of neutrons. Different weight. Neutrons and protons are INSIDE nucleus. Electrons on orbitals. Valence electrons= electrons on outermost shell. The electrons that do all reactions.

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