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Chemical elements

Chapter 4 Test Bank AP Bio

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Biology
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Chemistry
Nature
Organic chemistry
Isomerism
Chemical nomenclature
Chemical elements
Reducing agents
Molecule
Isomer
Organic compound
Amino acid
Carbon

Campbell's Biology, 9e (Reece et al.) Chapter 4 Carbon and the Molecular Diversity of Life This chapter focuses on the chemistry of carbon and organic compounds. Students should be able to identify the nature of the bonds between carbon and other elements (nonpolar versus polar), the different types of weak bonds and interactions, the various types of isomers, the basic functional groups of organic molecules, and their relative solubility in water. The abiotic formation of organic molecules from inorganic molecules is important in the origin of life. Multiple-Choice Questions 1) The element present in all organic molecules is A) hydrogen. B) oxygen. C) carbon. D) nitrogen. E) phosphorus. Answer: C Topic: Concept 4.1 Skill: Knowledge/Comprehension

metal alloys worksheet key

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Chemistry
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Chemistry
Alloys
Metallurgy
Chemical elements
Native element minerals
Transition metals
Intermetallic
Aluminium alloy
Metal
Copper
Silver
Heat treating

Metals & Alloys KEY 1. Electrons are stationary in a metallic compound. True or False? 2. Copper is often used to make wires. This is because.... (you may select more than one response) it is ductile it has a high electronegativity it is conductive it is malleable 3. Most metals are _____________at room temperature. gas liquid molten solid 4. Sterling silver is composed of silver & copper. What type of alloy is this? interstitial alloy substitutional alloy substitutional?institial alloy it's not an alloy, its an ionic compound 5. An alloy is formed using a transition metal and carbon. It retains the crystalline structure of the transition metal. What type of alloy is created? A Hetergeneous B Homogeneous substitional C Homogenous interstitial D Intermetallic

metal alloys worksheet

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Chemistry
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Chemistry
Alloys
Metallurgy
Chemical elements
Native element minerals
Transition metals
Aluminium alloy
Intermetallic
Metal
Copper
Silver
Heat treating

Metals & Alloys Name ___________________________ Directions: Circle the best answer for each of the following. 1. Electrons are stationary in a metallic compound. True or False? 2. Copper is often used to make wires. This is because.... (you may select more than one response) it is ductile it has a high electronegativity it is conductive it is malleable 3. Most metals are _____________at room temperature. Gas C. molten Liquid D. solid 4. Sterling silver is composed of silver & copper. What type of alloy is this? interstitial alloy substitutional alloy substitutional?institial alloy it's not an alloy, its an ionic compound

Chapter 7 Chemistry Notes

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Chemistry
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Chemistry
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Chemical nomenclature
Ions
Chemical elements
Periodic table
Polyatomic ion
Chemical compound
Molecule
Oxidation state
Hydrogen
Chemical formula

Chapter 7 7-1 symbol? an abbreviation for the name of the element Chemical formula? a type of notation made with numbers and chem. Symbols To indicate the composition of a compound To indicate the number of atoms in one molecule of an element molecule? a single atom, a group of 2+ atoms of the same element, or a group of atoms of different elements that have combined to form a compound Monoatomic molecules? molecules with one atom Diatomic molecules? two atom molecules Hydrogen, oxygen, nitrogen, chlorine, fluorine, bromine, Iodine When writing the formula for a molecule of an element, write the number of atoms in each molecule as a subscript just after the symbol The formula of a compound tells 2 things: The element making up the compound

alg

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Algebra
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Chemistry
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Universe
Chemical elements
Helium
Chemical substance
Substance theory
Mixture
Gas
Solid
Matter
Chemical reaction

Fundamentals of Chemistry What is Chemistry? What is Matter? How does it change? (How do we organize the types of changes? What categories? How do we categorize the types of matter? We can identify the specific types of matter with its ________ (characteristics). Definition: How many Smallest unit Examples Element: Compound: Mixture: What is the table of elements called? Is a compound considered a pure substance? How is a compound different than a mixture? Is a mixture considered a pure substance? How are mixtures classified? Draw sketches: solid liquid gas Macroscopic Microscopic How do the microscopic models explain the macroscopic properties? Property Solid Liquid Gas Fluidity (fixed shape) Why? Compressibity (fixed volume)

water biofact sheet

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Biology
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Chemistry
Chemical elements
Physical chemistry
Industrial gases
Inorganic solvents
Oxides
Properties of water
Molecule
Hydrogen
Chemical polarity
Water
Chemical reaction

The Biological Importance of Water B io F actsheet September 1998 Number 30 1 Water is a polar molecule i.e. it has both positively charged and negatively charged areas. Water is made up of two positively charged hydrogen atoms and one negatively charged oxygen atom (Fig 1). Water (H2O) is the most abundant molecule in cells, whole organisms and on earth. This is a consequence of the unique physical and chemical properties of water. This Factsheet will briefly explain the significance of these physical and chemical properties, then discuss the primary roles of water in animals and plants. As a result of this polarity (the uneven distribution of charges), adjacent water molecules are attracted to and become bonded to each other. The

Chapter 1.2 Outline

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Chemistry
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Condensed matter physics
Chemical substance
General chemistry
Chemical compound
Homogeneous and heterogeneous mixtures
Mixture
Solution
Gas
Liquid

Matter Classified by? Physical State (Gas/ Liquid/ Solid) Composition (Element/ Compound/ Mixture) States of Matter Gas (vapor) No fixed volume or shape Uniformly fills its container Can be compressed to occupy a smaller volume Can be expanded to occupy a larger volume Molecules are far apart, move quickly, and often collide with the surrounding container Liquid Distinct volume (independent of container) No fixed shape (assumes shape of occupied container) Can't be compressed Molecules are packed closely but can still move (they flow over each other, reducing viscosity Solid Definite shape and definite volume Can't be compressed Molecules have fixed positions an wiggle only slightly *Temperature and pressure changes lead to phase changes of the substance

Campbell Biology 9th Edition Chapter 4 Outline

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Biology
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Chemistry
Chemical elements
Nonmetals
Carbon
Photosynthesis
Organic chemistry
Oxygen
Organic
Organic compound
Carbon cycle
Environment
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Chemistry
organic chemistry
Chemical elements
Nonmetals
Reducing agents
Carbon
Isomer
Structural isomer
Organic compound
molecule
Inorganic compound
Hydrogen
Environment
Carbon and the Molecular Diversity of Life

Chapter 4 Carbon and the Molecular Diversity of Life Outline Carbon: The Backbone of Life Organisms are made up of chemicals based mostly on carbon Carbon comes into the atmosphere through the action of plants: plants use solar energy to transform CO2 Carbon forms molecules that are large, complex, and varied Organic Chemistry is the Study of Carbon Compounds Organic Chemistry: The branch of chemistry that specializes in the study of carbon compounds Overall percentages of the major elements of life are quite uniform from one organism to the next Chemists learned to make many simple compounds in the lab by combining elements under the right conditions by the 1800s Vitalism: The belief in a life force outside the jurisdiction of physical and chemical laws

Ch. 2: The Chemical Context of Life

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Biology
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Chemical elements
Dietary minerals
Nonmetals
Reducing agents
Chalcogens
Sulfur
Chemical substance
Phosphorus
Oxygen
Potassium
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Chapter 2 The Chemical Context of Life Camobell Bio 9th Edition

2.1 An element is a substance that cannot be broken down to other substances by chemical reactions. A compound is a substance consisting of two or more different elements combined in a fixed ratio. Essential elements are needed for a healthy life and to reproduce. Humans need 25, plants need 17 Oxygen (O), Carbon (C), Hydrogen (H) and Nitrogen (N)?make up 96% of living matter Calcium (Ca), Phosphorus (P), potassium (K), sulfur (S), and a few other elements accounting for most of the remaining 4% of an organism's mass. Trace elements are required by an organism in only minute quantities. ? 2.2 Protons and neutrons are electrically charged. Proton= positive, electron=negative, neutron=neutral

Chapter 3 Notes

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Biology
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Chemical elements
Periodic table
Nonmetals
Chalcogens
Oxygen
Period
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Hydrogen
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biochemistry

BIOL 1020 - CHAPTER 2 LECTURE NOTES Chapter 2: The Chemical Context of Life You must understand chemistry to understand life (and to pass this course)! Elements and Atoms Elements ? substances that cannot be further broken down into other substances (at least by ordinary chemical reactions) every element has a chemical symbol (H for hydrogen, O for oxygen, etc.); this is most familiar from the periodic table Essential elements: elements that an organism needs to live. They are similar along different organism but there is some variation Trace element: elements that are required by an organism in only minute quantities E.g.: Iron (Trace) Oxygen, Hydrogen, Nitrogen, and Carbon(Essential elements)

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