reactions are electrons. protons. neutrons. isotopes. Question 2 of 20 The structural unit that retains the properties of an element is the molecule. atom. cell. electron. Question 3 of 20 Which of the following are found in the nucleus of an atom? Protons Neutrons Electrons A and B Question 4 of 20 The component of an atom or molecule that is most important in determining its chemical properties is the isotope. neutron. electron. proton
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objects around you. Atoms are composed of particles called protons‚ electrons and neutrons. Protons carry a positive electrical charge‚ electrons carry a negative electrical charge and neutrons carry no electrical charge at all. The protons and neutrons cluster together in the central part of the atom‚ called the nucleus‚ and the electrons ’orbit’ the nucleus. A particular atom will have the same number of protons and electrons and most atoms have at least as many neutrons as protons. Protons and
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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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are created by the complete transfer of electrons from one atom to another. In this process of electron transfer‚ each atom becomes a ion that is isoelectronic with the nearest noble gas.‚ the substance is held together by electrostatic forces between the ions. The tendency for these ions to be formed by elements is corespondent to the octet rule‚ when atoms react‚‚ they tend to do so in such a way that they attain an outer shell containing eight electrons. The factors that effect the formation of
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these modifications came in 1897 when J.J. Thomson discovered the electron. Based on the work of William Crookes and his "Crookes tube" (Cathode-ray tube)‚ Thomson discovered a negative charged particle was the cause of the light produced by the cathode-ray tube. He also discovered that these particles are present in all elements. These cathode-ray particles are now known as electrons. Soon after the discovery of electrons the proton was discovered. This led Thomson to conclude that ther
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when we get there. Matter is composed of atoms. Atomic nuclei are tightly bound protons and neutrons (1H excepted) with electrons hanging out in the electron clouds around them. Also‚ there are chemical bonds between atoms in a lot of different kinds of matter. These bonds involve the borrowing and loaning of electrons (the so-called ionic bonds) or the sharing of electrons (the so-called covalent bonds). That’s matter‚ and now we’re going to see what happens when we shoot stuff at it. Incoming
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examiner’s report for each question. 1. (i) atoms of the same element with different numbers of neutrons/different masses (1) 1 (ii) 79Br 35 protons‚ 44 neutrons‚ 35 electrons (1) 81Br 35 protons‚ 46 neutrons‚ 35 electrons (1) 2 (iii) (1s2)2s22p63s23p63d104s24p5 (1) 1 [4] 2. (i) iodide has been converted to iodine (1) (with correct use and spelling of iodide and iodine)
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Charging by Induction Purpose: To determine the kind of charge induced on a neutral object when it is approached by a charged object. Materials: • metal-leaf electroscope • ebonite rod • fur • glass rod • silk • human finger (with body) Procedure: 1. The metal-leaf electroscope was approached‚ but not touched‚ by a negatively charged ebonite rod. The rod was moved toward and away from the metal ball on the electroscope several times. Observations were recorded
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some other molecules Influence of the nature of electron pairs on bond angles in molecules of methane‚ ammonia and water Shapes of some polyatomic ions Shapes of molecules with multiple bonds Molecular crystals of buckminsterfullerene (C60) 23.1 – 23.7 Summary 1 Examples of covalent molecules with non-octet structures are as follows: Molecule Electron diagram F BF3 B F F SF4 F Molecule Electron diagram F S F F Cl PCl5 Cl Cl P Cl Cl SF6 F F
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usually formed between a metal and a non-metal‚ Covalent between two non-metals and Metallic between two metals. Ionic Bonding; Ionic bonds tend to form between metals whose atoms need to “loose” electrons to gain the nearest noble gas configuration and non-metals that need to gain electrons. These electrons are transferred from one atom to another. This gives one ion a positive charge and the other a negative one. The Opposite charges in the ion hold them together in a regular three dimensional
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