Section One - The Structure of the Atom Atomic Structure 1) Copy and complete the table: Particle Relative Mass Relative Charge Proton 1 +1 Neutron 1 0 Electron 1/840 -1 2) What is the charge on an ion formed when an atom loses two electrons? +2 3) What is the charge on an ion formed when an atom gains two electrons? -2 The Mole 1) Find the molar mass of zinc 65g/mol 2)Find the molar mass of sulfuric acid H2 SO4 98g/mol 3) How many moles of sodium chloride
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specific charge‚ i.e. charge to mass ratio ‚ of an electron using m Thomson’s bar magnet method. Basic methodology: Electrons in a CRT are deflected in the vertical direction by applying a potential between the vertical deflection plates of the CRT. A magnetic field perpendicular to the deflecting electric field is produced using a pair of bar magnets. The position of the magnets is adjusted so as to cancel the deflection of the electrons. The knowledge of the deflecting potential and the magnet
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fixed ratio‚ has characteristics different from those of its elements TRACE ELEMENT- those required by an organism in minute quantities ATOM- smallest unit of matter that still retains the properties of an element NEUTRONS- no electrical charge ELECTRONS- negative charge PROTONS- positive charge ATOMIC NUCLEUS- formed by neutrons and protons ATOMIC NUMBER- number of protons in its nucleus MASS NUMBER- the sum of protons and neutrons in the nucleus ATOMIC MASS- the atom’s total mass‚ can be approximated
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11 I. ABSTRACT The aim of this study is to demonstrate how batteries work. Batteries may seem a little magical‚ but they are not. A battery actually is just a container of chemicals that react together to produce a flow of electrons‚ which is what an electrical current really is. A battery has two terminals‚ one positive and one negative. They are usually marked by plus and minus signs‚ so you can tell which is which. After the battery is assembled‚ a multimeter / voltmeter
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neutrons and electrons. * Define proton number and nucleon number. * Use proton number and the simple structure of atoms to explain the basis of the Periodic Table (Ref. Z=1 to 20) * Define isotopes. * State the two types of isotopes as being radioactive and non-radioactive. * State one medical and one industrial use of radioactive isotopes. * Describe radioactive isotopes as a source of energy. eg. 235U * Describe the build-up of electrons in `shells` and
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and determine the no. of electrons‚ protons and neutrons of the following e- p+ n a.) Oxygen - 8 8 b.) Cesium - 55 55 c.) Argon - 18 18 d.) Uranium - 92 92 e.) Copper - 29 29 2. Calculate the atomic mass of sulfur from its natural isotope. f.) Sulfur-36 g.) Sulfur-32 h.) Sulfur-33 i.) Sulfur-34 3. Complete this table. Symbol of Elements | Atomic Number | Atomic Mass | # of protons | # of Electrons | # of Neutrons | Sc |
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CHEMISTRY 17 1ST LONG EXAM REVIEWER I. ELECTRONIC STRUCTURE OF ATOMS -arrangement of atoms’ electrons -the number of electrons in an atom -distribution of electrons around the nucleus and their energies • ATOMS *Billiard Ball Model (JOHN DALTON) *Plum Pudding Model (JOSEPH J. THOMPSON) *RUTHERFORD’s Model of Atom -atoms are tiny‚ hard‚ indivisible spheres -electrons (negative charge) occupy the atom - Atom is mostly empty space with a dense nucleus • PROBLEMS with Rutherford’s Model
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chemical bond that involves the sharing of pairs of electrons between atoms. A compound is made when two or more atoms form a chemical bond‚ linking them together. The two types of bonds are ionic bonds and covalent bonds. In an ionic bond‚ the atoms are bound together by the attraction between oppositely charged ions. If the electron is shared equally between the atoms forming a covalent bond‚ then the bond is said to be nonpolar. An electron is more attracted to one atom than to another which forming
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emitted due to an atom’s electrons making a transition from a high energy state to a lower energy state. Since each element has different numbers of electrons‚ each element’s emission spectrum is different. This allows elements to be identified by their color during a flame test. For example‚ it is know that a sodium cation burns a yellow-orange color. The normal electron configuration of atoms or ions of an element is known as the ground state. In this energy state‚ all electrons are at their most stable
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protons are not equal to the electrons ion the protons are not equal to the neutrons isotope atomic mass = mass of protons + neutrons changing the number of neutrons does not influece the mass or electrons atom behaviour is because of electrons hydrogen almost always loses its electron‚ leaving it a hydrogen ion taking away a negative charge creates a cation adding a negative charge creates an anion electronegativity is the ability to steal electrons electronegativity is influenced
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