JQ Eighth

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MrsTabor

journal questions for 8th graders 3rd quarter 2009.

Educación Desarrollo personal Tecnología

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Moje presentace z konference Devel.cz 2013. Najdete tu mikroúvod do problematiky Big Data a pak praktické užití v české energetice - smart grid. Povšimněte si dvou problémů: 1) presentace byla dělána na Macku, pak konvertována do PowerPointu, tím se ztratila část fontů. 2) presentace byla dělána pro sdělení publiku a bez mého komentáře vám asi nebude dávat valný smysl. Nu, měli jste přijít na Devel :)

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Chapter 2 Lecture Participation Assignment 5 points To complete this assignment, you can either print out this worksheet and fill in your answers or you can fill them in electronically in this word document. When you are done, you will upload your assignment to the ‘chapter 2 participation assignment’ folder found in D2L under assessments à assignments. 1. How many protons in 12C , 13C, 14C, 12C - ? In 16O , 17O, 18O,? 2. How many electrons in 12C , 13C, 14C, 12C - ? In 16O , 17O, 18O,? 3. How many neutrons in 12C , 13C, 14C, 12C -? In 16O , 17O, 18O,? 4. What do all forms of the element carbon have in common (besides the C)? All forms of O? 5. How are the isotopes of carbon ( 12C , 13C, 14C) different from each other? The isotopes of O( 16O , 17O, 18O) ? 6. What determines the mass number (12, 13,14 or 16, 17, 18 ) in the different isotopes? Part II: Atomic Structure and Bonding Atoms do not exist all alone. Much of the time, atoms bond to other atoms to form molecules. These molecules can be very large (consisting of hundreds or thousands of atoms). For example, the major biological macromolecules (carbohydrates, lipids, proteins, and nucleic acids) are large molecules made up of many C, H, O, and N or P atoms bonded together. How can we predict if an atom will form bonds with another atom? Examine the model below. Reactive (form bonds) Not reactive (first 7 columns) (last column) Critical Thinking Questions: 7. Based on the model, what is the maximum number of electrons that can be in the first electron shell?8. Based on the model, what is the maximum number that can be found in the 2nd shell? The 3rd?9. What do you notice about the outer shells of all the nonreactive atoms?10. Can you draw the electron distribution diagram for potassium (K)? Part III: Types of Bonds There are 3 major types of bonds: ionic , covalent , and hydrogen bonds . There are two types of covalent bonds: polar covalent and nonpolar covalent. Model: Ionic bond : electrons are transferred from one atom to another in order to fill the atoms’ outer shells. The resulting ions are attracted to each other due to their opposite charges. Covalent bond : electrons are shared by two atoms in order to the fill atoms’ outer shells. H2 O2 H20 1. In the ionic bond model, why does the sodium have a positive charge? 2. In the ionic bond model, why does the chlorine have a negative charge? 3. In the covalent bond model, why don’t any of the atoms have a charge?4. For each of the covalently bonded molecules, circle the shared electrons.5. Look at all of the bonds. If you c.

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ELEMENTARY PARTICLES OF MATTER Matter is made up of discrete particles, the main ones are:- 1. Atoms 2. Ions 3. Molecules - (AIM) DEFINITION OF ATOMS An atom is the smallest particle of an element which can take part in a chemical reaction THE CONSTITUENTS OF ATOMS Rutherford in 1911 threw more light on the nature of the atom. He demonstrated that atom is made up of sub-particles which are called: 1. Proton 2. Neutron 3. Electron. He discovered that the protons and neutrons are concentrated in the nucleus of an atom, while the electrons are revolving round the nucleus. J.J THOMPSON’S MODEL J.J Thompson described the atom as being made up of a mixture of positive (Protons) and negative (Electrons) charges. LORD RUTHERFORD’S MODEL Lord Rutherford described the atom as being made up of Positive (Protons) and Neutral (Neutrons) charges in its centre (nucleus) while the negative charges (electrons) rotates around its orbit. He used the planetary bodies rotating around the sun to describe the structure of atoms. CHARACTERISTICS OF PROTON, ELECTRON AND NEUTRON DALTON’S ATOMIC THEORY In 1808, John Dalton proposed the Atomic Theory which can be summarised as follows: All elements are made up of small, indivisible particles called atoms. Atoms can neither be created nor destroyed. Atoms of the same elements are alike in every aspect, and differ from atoms of all other elements. When atoms combine with other atoms, they do so in simple ratios. All chemical changes result from the combination or the separation of atoms. The Atomic Theory was partially supported by experimental evidences deduced from the Law of Conservation of Mass, the Law of Definite Proportions, the Law of Multiple Proportions and so on. It could not explain electrolysis and certain other phenomena. As a result of new discoveries, Dalton’s original Atomic Theory has undergone several modifications but the principal aspects as outlined above are still useful in the study of chemistry. MODIFICATIONS OF DALTON’S ATOMIC THEORY All Elements Are Made Up Of Small Indivisible Particles Called Atoms: This statement has been proven wrong by Rutherford’s discovery – the atom is built up of three main types of sub-particles: the proton, the electron, the neutron. It is not an indivisible solid piece. The Atom Can Neither Be Created Nor Destroyed: This statement still holds good for ordinary chemical reactions and is embodied in the basic Law of Conservation of Mass. During a nuclear reaction, such as the fission of Uranium – 235, the nucleus is broken up into smaller units which form simpler atoms while a tremendous amount of heat energy is released. These changes that occur during nuclear fission destroy the atoms of the element involved. The Atoms Of The Same Elements Are Alike In Every Aspect And Differ From Atoms Of All Other Elements: The discovery of isotopes makes this statement unacceptable. Chlorine, for example has two different atom

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JQ Eighth

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JQ Eighth

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JQ Eighth