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Name ________________________________________ Periods 1 & 6 Final Review Unit 1 The Metric Unit: Chemistry – study of the ______________________________________, and the __________________________________________________________________ Chemistry is the science that __________________________________________ ______________________________________________________________ and engages in the synthesis and analysis of _________________________________. --Webster’s ***OR chemistry is ______________________________________________*** Matter – anything that _________________________________________ ___________________________________________________________ OR ________________________________________________________ ____________________________________________________________ Scientific Notation … making #s __________________. Scientific notation provides an easy way to represent #s that are really really _______________ and really really ___________________ Scientific notation = a ___________________ # in ones place (in front of the decimal) with nothing to the left of it __ . __ __ __ __... ↕ nonzero 400 4.1 33.1 7 0.77 To put numbers into scientific notation: ________________________________________ until there is one nonzero in the ones place with nothing to the left of it. The Final Review – Periods 1 & 6 -1- EXAMPLES: Convert the following #s into sci. not. 7010 = ___________________ 0.041 = ___________________ 7.4 = ___________________ Take the following #s out of sci. not. 1.1 * 10-2 = ___________________ 7 * 101 = ___________________ 2.2 * 103 = ___________________ Unit 2 Matter and Energy: Matter - _________________________________________________________________ ________________________________________________________ … EVERYTHING Matter must have: _________________ and __________________ A. Properties of Matter: • When you look at a particular sample of matter, you observe its ______________. • We classify different types of matter according to _________________________. Physical – observed without changing the chemical _________________. Examples: __________________________________________ Chemical – requires a change in chemical _________________ to be observed – relates to a substances ability to undergo change. Examples: _________________________________________ Qualitative – no observed _____________________ – no # Examples: ________________________________________ Quantitative – includes a numeric measurement Examples: _______________________________________ The Final Review – Periods 1 & 6 -2- Example: My three pennies had a volume of 1.02 ml. Physical or chemical? Qualitative or quantitative? Mass - ____________________________________________________________ Different from weight? ______________________________________________ B. Classifications of Matter: Matter Mixtures (more than 1 ____________________) Pure Substance (always the same – same _________________________ ________________________) Homogeneous (the same throughout) - air = solutions Heterogeneous (physically __________________, not the same throughout) - pizza element compound (2 or more _____________________ chemically bonded together) – A mixture = a _________________________ of two or more components. – Another name for a homogeneous mixture is a solution. Separating the components of a mixture: Differences in ________________________ can be used to separate mixtures. Filtration = the process that ______________________________________ in a heterogeneous mixture is called Distillation = the process of ________________________________________ ________________________________________________________ - during a distillation, a liquid is boiled to produce a vapor that is then condensed into a pure liquid. Which physical property does filtration rely on? ________________________ Which does distillation rely on? ______________________________________ The Final Review – Periods 1 & 6 -3- – Distinguishing Elements and Compounds: Element = the ___________________________________________________ _______________________________________________________________ Oxygen and hydrogen are 2 of the more than 100 known elements. Compound = a substance that contains _______________________________ _____________________________________________ in a fixed proportion. Physical methods that are used to separate mixtures cannot be used to break a compound into simpler substances. To break a compound apart, you must apply _________ (usually heat / electricity) ***The properties of compounds are totally different than the properties of the elements they are made of. C. States of Matter: o Solids – rigid with a _________________________________________________ o Liquid – flowing with a ______________________________________________ o Gas – flowing, compressible – NO definite shape or volume D. Changes in Matter: Lab vocab. A. precipitate – _____________________________________________________ B. exothermic reaction – _____________________________________________ C. endothermic reaction – ____________________________________________ The Final Review – Periods 1 & 6 -4- Physical Change – change without change in the ____________________ of the substance – easily reversible. - Are changes of state physical changes? ___________________________ 3 states of matter: -liquid -solid -gas Chemical Change – one or more substances are converted into different (new) substances – cannot go back without another reaction - burning - breaking apart a compound - rusting Law of Conservation of Matter / Law of Conservation of Mass: ____________________ ________________________________________________________________________ Unit 3 Atomic: Before we start (review): __________(_) Nucleus ATOM ___________(_) ___________(_) The Final Review – Periods 1 & 6 -5- I. Atomic Theory (1800s): Make sure you know that Modern Atomic Theory as described below!!! Dalton’s Atomic Theory (1800s): Modern Atomic Theory: 1. All matter is _________________ 1. All matter is composed of extremely small particles called atoms. ___________________________ ___________________________. 2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties. 3. Atoms cannot be subdivided, created, or destroyed. 2. A GIVEN ELEMENT CAN HAVE ATOMS WITH DIFFERENT _____________. 3. ATOMS ARE _____________ INTO EVEN SMALLER PARTICLES. 4. Atoms of different elements combine in simple wholenumbered ratios to form chemical compounds. 4. Atoms of different elements combine in simple wholenumbered ratios to form 5. In chemical reactions, atoms ___________________________. are _____________________ 5. In chemical reactions, atoms are _______________________. ___________________________ ___________________________. - 1897 J. J. Thomson: - Studied ________________________ _______________. - All metals create _____________________________________. - Cathode ray particles are ___________________ and ____________________ _______________________. - Thomson coined the ________________________ as another name for _____________________ ______________ _____________________. - Thomson’s view of the atom = _______________ _________________ with separate parts, negative ____________________ and positive ____________________________ The Final Review – Periods 1 & 6 -6- Representing nuclear decay and other nuclear reactions: ____________________ 4 → 234 92 90 Th + 2He 238U _____________________ Mass # = protons + neutrons Atomic # = protons – find this on the _______________________________ Write the nuclear symbol for Carbon with 6 neutrons _____ Write the nuclear symbol for Carbon with 8 neutrons _____ - 1909-1910 Rutherford: - Gold foil experiments = _______________________________________ ____________________________________________________________ - Atom’s appearance: - _____________________________ - ______________________________________________ - ___________________________________________ - 1912-1913 Bohr: - modified __________________________ model - Electrons are located in ____________________________________________. - Used this model to explain ________________ _________________ … ring model -When an electron becomes excited (____________ ___________) it can jump up to a new energy level. When it falls back down to its _______________________ ______________ (original energy level) it emits energy (light). The Final Review – Periods 1 & 6 -7- -1919 Rutherford: - discovered _________________________ - Carry a _______________ charge and are found in the ________. - The number of ___________ is the atom’s ___________ ____________. - 1926 Bohr: - Neils Bohr’s ____________________model of the atom - ___________________________________________________ - ___________________ is dense center with _____________ _______________ - ______________________ found in specific energy levels - 1932 Chadwick: - discovered ___________________ - no charge, located in the ______________ - What are protons, neutrons, and electrons made of? _______________________ Vocabulary: Isotopes - _______________________________________________________________ ________________________________________________________________________ Ion - ___________________________________________________________________ ________________________________________________________________________ The Final Review – Periods 1 & 6 -8- Fundamental parts of atoms COMPONENT CHARGE electron ______ ________ +1 neutron 0 APPROXIMATE MASS (in amu) LOCATION IN ATOM 0.00055 shells 1.0 nucleus _________ 1.00055 • X = __________ __________ • A = __________ __________ • Z = _________ ____________ • C = ___________________ A Z C X # of neutrons = ________________________ # of electrons = ________________________ What forces act in the atom? - ________________________________ force holds _______________ together - _________________________________ force causes __________________ - Natural radioactivity, radioactive decay, or nuclear disintegration is the _________________________________ of __________________ from an element due to instability of the ___________________. - Problems in nuclear stability occur when there are too few or too many ____________. - All elements with an atomic number greater than _______ are radioactive. The Final Review – Periods 1 & 6 -9-