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Atomic mass

Mass Relationships in Chemical Reactions Practice QuestionsG

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Atomic mass mass of an atom in atomic mass units An atomic mass unit is equal to? One twelth the mass of one carbon-12 atom The average atomic mass is equal to? atomic mass on the periodic table Isotopes are atoms of the same element with a different number of ___ and so they have different ___ 1) neutron 2) masses Mole Is a counter and relates to mass.* It is similar to a dozen. *It can count the number atoms/molecules/particles. Molar Mass *is the mass of one mole of the substance. *g/mol = atomic mass of the element *molar mass of an element contains mols of atoms Avogadro's number particles/atoms/molecueles > moles *6.022x10^23 Percent Composition Mass of element/ mass of compound x 100 Tell how much an element contributes to the mass of the compound

AP Chemistry Zumdahl 7E Chapter 3 Notes

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Chemistry

AP Chemistry A. Allan Chapter 3 Notes - Stoichiometry 3.1 Atomic Masses A. C-12, the Relative Standard 1. C-12 is assigned a mass of exactly 12 atomic mass units (amu) 2. Masses of all elements are determined in comparison to the carbon - 12 atom (12C) the most common isotope of carbon 3. Comparisons are made using a mass spectrometer B. Atomic Mass (Average atomic mass, atomic weight) 1. Atomic masses are the average of the naturally occurring isotopes of an element 2. Atomic mass does not represent the mass of any actual atom 3. Atomic mass can be used to "weigh out" large numbers of atoms 3.2 The Mole A. Avogadro's number 1. 6.022 x 1023 units = 1 mole 2. Named in honor of Avogadro (he did NOT discover it) B. Measuring moles

Periodic Table - Notes

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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.

Mole conversions - Notes

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Chemical Quantities The MOLE CHAPTER 7 THE MOLE: A MEASUREMENT OF MATTER A mole (mol) is a unit of measurement Types of measurement include Counting/weighing/volume/ number of units Examples of other Quantitative measurement units Pair/Dozen/Ream Mole The term representative particles is a generic term that can refer to Atoms (single element), or Diatomic molecules (two of one type of element), or Formula units (what makes up an ionic compound) or Molecules (what makes up a molecular compound), or electrons or protons, or ions, etc Mole It is typically referred to as a mole of atoms or a mole of molecules A mole is also called Avogadro?s number For example: One mole would be 6.022 x 1023 representative particles Why use moles?

Atomic Structure Notes

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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

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

Chapter 4

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Chemistry 1210: General Chemistry Dr. Gina M. Florio 13 September 2012 Jespersen, Brady, Hyslop, Chapter 4 The Mole and Stoichiometry CHE 1210 Lecture Slides G.M. Florio 1 Conversion Factors Conversion Factor ? relates one quantity to another ? used to convert between two units in chemistry What is my height in centimeters (cm) if I am 5 feet 4 inches tall? 1. How many inches are in a foot? 2. How many inches are in a centimeter? 12 inches = 1 foot 1 inch = 2.54 cm Factor Label Method The factor-label method, or dimensional analysis lets us treat a numerical problem as one involving a conversion from one kind of units to another using conversion factors.

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

Bob Jones PPT Notes -- Chapter 4c

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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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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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