Chemical element

Atoms

Isotope

Atom

Chemical element

Neutron

Protons, Neutrons, and Electrons Practice Worksheet Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table. Atomic symbol Atomic number Protons Neutrons Electrons Atomic mass B 6 11 24 31 37 39 89 29 35 43 100 Pb 207 102 70 89 225 Mo 53 81 206 100 159 No 261 Yb 172 106 159 Finding Protons, Neutrons, and Electrons of Elements

Campbell Biology Chapter 2 outline

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Baryons

Neutron

Matter

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ion

Proton

SUBATOMIC PARTICLES Proton ? 1 positive charge (P+) Neutron ? no charge (N0) Electron ? 1 negative charge (E+) Nucleus An atom's dense central core, containing protons and neutrons. Electrons move around the nucleus Matter Anything that has mass and takes up space Elements Substance that cannot be broken down by a chemical reaction 92 occur naturally 25 of which are essential for life Bulk elements Required by the body in large amounts C N H O (make up 96% of the body) Trace elements Required by the body in small amounts Ultra trace elements Required by the body in minute amounts Atoms Smallest unit of matter that still retains properties of an element Weight Add proton and neutrons together for weight of nucleus Every proton and neutron weights one Dalton

Basic Biochemistry

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Isotope

Iodine

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AP Biology Biochemistry

Atomic Structures Atoms are basic units of matter Protons (+1) , Neutrons (0), Electrons (-1) Depending on their energy levels, they are in different states. Ground state: At lowest possible potential energy. Excited state: At any state where the system is at higher than the minimum. Isotopes: atoms of one element that vary in neutrons. Are all chemically identical Radioisotopes: decay at a rate known as half-life, often used in medicine. Tracers: used to TRACE certain chemicals in natural pathways Ex: Iodine (radioactive) to give information about thyroid gland metabolism. Bonding In biology, the two main types are Ionic and Covalent Ionic Bonds Transfer of electrons Receiver is called anion (a negative ion) Donor is called the cation Covalent Bonds

Wiley Joeking

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Matter

Odor

Oxygen

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Chemistry: Matter & Properties Matter is anything that has _______________ and occupies ______________. Matter has (Area) (Volume) (Indefinite Structure) What are the 4 building blocks of matter? __________, _________, ___________, and _______________. What is NOT a building block of matter Odor Compounds Amino Acids Both A and C None Of the above The smallest unit of an element that maintains the properties of that element: _________________________ A pure substance made of only one kind of atom is an _________________ An element is made up of ___ kind(s) of atom(s) Which of the following DOESN?T describe a compound? It is a substance It is the smallest unit of an element that maintains the properties of that element Made from atoms Made of 2 or more elements

Chapter 2: Chemical Units and Their Identities

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Ion

Proton

ATOMS: - made of nucleus (protons (positive charge) and neutrons (neutral charge)) and electron cloud (electrons (negative charge) - smallest particle that still retains properties of element - atomic # - # of protons (unique to each element) (also # of electrons in neutral atoms) - mass # - # of protons + neutrons - atomic mass - actual (average) mass of atom (measured in daltons) - about mass # b/c electrons have very small mass compared to protons/neutrons - isotope - atom w/ more/less than usual # of neutrons ELECTRONS: - elemental form of element is when element is by itself - compound - joint of 2+ elements w/ own set of properties diff. from elements - elements in periodic table are arranged in atomic # and are in 18 columns (groups)

Periodic Table

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The periodic table is a very useful device for chemists and students to use. The periodic table is made of all of the elements that exist. For each element, the atomic number, atomic mass,the symbol, and the element name is in the periodic table. The Periodic table is organized in a way for us to easily tell which elements are metals, metalloids, or nonmetals. The state of the element is also sometimes included. The different groups (columns) have similiar characteristics with the other elements within the group. Group 1 is alkali metals, Group 2 is alkaline earth metals, Groups 3-12 are the transitional metals which also include the inner transition metals, Group 17 is the Halogens, and Group 18 is the noble gases.

Periodic Trends

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Periodic table

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Period

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Periodic Table of Elements

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Trend

Three Important Periodic Trends Definition of Periodic Trend: The tendency of a certain characteristic of an element to increase or decrease as they progresses along a period or group on the periodic table of elements Definition of Term Atomic Radius - One half the distance between the nuclei of identical atoms that are bonded together. Picometers (pm) Ionization Energy - The energy required to remove 1 electron from a neutral atom of an element. kiloJoules per Mole (kJ/mol) Electronegativity - The measure of the ability of an atom in a chemical compound to attract the electrons of another atom in the compound. Trend Across the PT The atomic radii decreases as you move across each period, as you add more protons to help pull the electrons closer to the nucleus.

AP Biology Campbell Chapter 2 Objectives

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Matter

Elements and Compounds Distinguish between an element and a compound. Identify the four elements that make up 96% of living matter. Define the term trace element and give an example. Atoms and Molecules Draw and label a simplified model of an atom. Explain how this model simplifies our understanding of atomic structure. Distinguish between each of the following pairs of terms: neutron and proton atomic number and mass number atomic weight and mass number Explain how the atomic number and mass number of an atom can be used to determine the number of neutrons. Explain how two isotopes of an element are similar. Explain how they are different. Describe two biological applications that use radioactive isotopes.

My Biology

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Chemistry Section 5.2 Notes

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