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Isotope

Atomic Structure

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Nuclear chemistry

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Atomic Structure The discovery of atoms began with Democritus, a Greek philosopher, who was the first person to suggest that atoms exist. However Democritus made the false claim that atoms were indestructible which was proven wrong with the development of the atomic bomb (nuclear power), additionally he did not support his idea with scientific evidence or explain the chemical behavior of the atom. Following Democritus was Dalton who took the idea of the atom and explained it and supported it with scientific methods. Atom= The smallest particle of an element that retains its identity within chemical reactions due to maintaining chemical and physical properties. Dalton?s Atomic Theory: All elements are composed of indivisible particles called atoms (later disproved)

Periodic Table - Notes

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Nuclear physics

Chemical element

Relative atomic mass

Extended periodic table

Notes ? Periodic Table Do you know all your elements? http://www.privatehand.com/flash/elements.html Squares on the Periodic Table Each square contains Element Symbol Element Name Atomic Number = Protons Average Atomic Mass = Molar Mass Some contain the physical state at Room Temperature What is the atomic mass? The mass of one atom is VERY small therefore we use a relative scale called the AMU. One AMU is exactly 1/12 the mass of a carbon-12 atom. Protons + Neutrons = AMU = Atomic Mass Unit What is the average atomic mass? In a sample of many atoms, various isotopes exist. The abundance of each isotope impacts the average mass of the sample. To find the average atomic mass, multiply the mass times the abundance of each isotope and add these together.

Atomic Structure Notes

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Chemical properties

Nuclear physics

Nuclear chemistry

Relative atomic mass

Chemical element

Pre-AP Chemistry 1 Chapter ________ Name _____________________________ Period ______ I. Historical Development (3-1) x particle theory of matter first proposed by ________________________ in 400 BC ? named the basic particle the ?_______________?, which means ____________________ in Greek x by 1700?s most scientists accepted definition of an _____________ as a substance that cannot be broken down by ordinary ________________ means x also accepted that _______________ combine to form ________________ x _______________________: the transformation of a substance or substances into 1 or more

Living in the Environment 16th Ed. : Ch.2 Key Terms

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Environmental Science

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Nuclear physics

Nuclear fission

Radioactive decay

Chapter 2 Key Terms acidity Ions are also important for measuring a substance?s acidity in a water solution, a chemical characteristic that helps determine how a substance dissolved in water will interact with and affect its environment. atom The most basic building block of matter is an atom: the smallest unit of matter into which an element can be divided and still retain its chemical properties. atomic number Each element has a unique atomic number, equal to the number of protons in the nucleus of its atom. atomic theory The idea that all elements are made up of atoms is called the atomic theory and is the most widely accepted scientific theory in chemistry. cells

atomic structure

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Atomic Structure Definitions ? Acceleration ? The stage of mass spectrometry during which the movement of the ions of the sample is speeded up using a series of negatively-charged plates. ? Atomic number ? The number of protons in the nucleus of an atom of an element. Represented by the symbol Z. Also called the proton number. ? Deflection ? The stage of mass spectrometry during which the beam of ions is bent by a particular amount, depending on its mass-to-charge ratio. This is achieved using an electromagnet. ? Detection ? The stage of mass spectrometry during which the ions strike a collector plate, producing a mass spectrum for analysis. ? Diatomic ? A molecule consisting of two atoms. ? Electromagnet ? The part of a mass spectrometer responsible for the

Chemistry MidTerm Review

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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

Chapter 6- Chemistry in Biology

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Nuclear chemistry

Quantum chemistry

Charge carriers

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 4c

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Nuclear physics

Chemical bonding

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 2

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Amount of substance

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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

Chemistry Chapter 4,25

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Particle physics

Nuclear physics

Nuclear chemistry

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Lecture 2 (Chapter 4 & 25) Atomic Structure Democritus (400 BC) ? Postulated there must be some basic unit of matter that could not be divided any further. ? Basic unit ? atomos (Greek = indivisible) Dalton Dalton?s Atomic Theory ? All matter is composed of extremely small particles called atoms ? All atoms of a given element are identical having the ame size, mass and chemical properties. Atoms of a specific element are different from those of any other element ? Different atoms combined in simple whole number ratios to form compounds ? Ina chemical reaction, atoms are separated, combined, or rearranged ? Atoms cannot be created, divided into smaller particles or destroyed. Scientist and Experiments Cathode Ray Tube Experiments ? Plum pudding model ?

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