relative atomic mass from isotopic composition data‚ or from a mass spectrum of an atom d) deduce relative molecular mass from the mass spectrum of a molecule e) Give the electronic configuration of atoms with atomic number 1-36 and of the common ions of elements 1 - 18 f) Define 1st‚2nd ionisation energy g) Explain trends in 1st IE across period (general increase‚ decrease from Be to B‚ decrease from N to O) and down group h) Explain trends in successive ionisation energies i) Explain
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material. On the other hand‚ the atoms (ions) in ionic materials show strong attractions to other ions in their vicinity. This generally leads to low melting points for covalent solids‚ and high melting points for ionic solids. For example‚ the molecule carbon tetrachloride is a non-polar covalent molecule‚ CCl4. It’s melting point is -23°C. By contrast‚ the ionic solid NaCl has a melting point of 800°C. Ionic Compounds Crystalline solids (made of ions) High melting and boiling points Conduct
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Covalent 4. Metallic Classification of Crystalline solids: S.No. Types of solid Constituent Particles Nature of forces Examples 1 Ionic solids Positive and Negative ions Strong electrostatic forces of attraction LiF‚ KCl‚ KNO3‚ BaSO4 2 Molecular solids Molecules Van der Waal’s forces. Dipole interactions. Hydrogen bonding I2‚ CO2 (solid)‚ HCl‚ Ice 3 Covalent solids Atoms Covalent bonds Diamond‚ Silicon 4 Metallic solids Positive metal ions (Kernels) and
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UTAR FHSC1134 Inorganic Chemistry Trimester 3 Experiment 1 ________________________________________________________________________ Title: Investigating the Properties of Period 3 Oxides Aim: To examine the oxides of Period 3 elements and describe their structure and bonding. Introduction: Generally‚ there are oxides of metals and non-metals. Metals burn in oxygen to form basic oxides while non-metals form acidic oxides. Structurally‚ they are covalent or ionic compounds. You are to
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Chapters 7&8 Gauge Sheet 7.1- Ions To find the number of valence electrons in an atom of a representative element‚ simply look at its group number. Atoms of metals tend to lose their valence electrons‚ leaving a complete octet in the next-lowest energy level. Atoms of some non-metals tend to gain electrons or to share with another non-metal to achieve a complete octet. The gain of negatively charged electrons by a neutral atom produces an anion. 7.2- Ionic Bonds and Ionic Compounds Although
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PAHANG TRIAL 2009 EXAMINATION CHEMISTRY PAPER 2 MARKING SCHEMES SECTION A - Structural Questions: Question 1. (a) (i) The presence of isotopes 1M (ii) Let the abundance of 63X be a %. The % abundance of 65X. = ( 100 – a ) 1M Relative atomic mass = ( 62.93 x a) + ( 64.93 x ( 100 -a) ) 1M
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Bharati Bhawan) (Chapter 1 and 2) 3. A New Approach to ICSE Chemistry(Part-I) Goyal Brothers Prakashan (Chapter 1 and 3) 2. Atoms and Molecules/ Mole concept Dalton’s atomic theory‚ atoms‚ molecules‚ ions‚ atomic mass‚ molecular mass‚ atomic scale units(CU)‚ symbol‚ valency of ions‚ formula of ions and compounds‚ Writing ionic equations‚ solubilty rules‚ balancing simple equations by hit and trial method‚ Mole concept‚ percentage composition of elements in compounds‚ empirical and molecular formula
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What is water purification? Water purification generally means freeing water from any kind of impurity it contains‚ such as contaminants or micro organisms. Water purification is not a very one-sided process; the purification process contains many steps. The steps that need to be progressed depend on the kind of impurities that are found in the water. This can differ very much for different types of water. In which ways is polluted water treated? Settling Before the purification process begins some
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mass of metallic oxide: 80.763 g Mass of metal is 74 % of the total mass (It was later discovered the new metal held 11 protons‚ 12 neutrons & 11 electrons) 4. Mr. Collins went home and wanted to know about the following: a. The number of moles of chlorine atoms in 3.08g of tetrachloromethane (CCl4) b. The number of moles of fluorine atoms in 204 g of boron trifluoride BF3; c. The number of moles of chloride in 5.55 g of calcium chloride‚ CaCl 2 d. The number of moles of sulphate ions in 144g
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unequal‚ with the electrons spending more time around the more non-metallic atom‚ are called polar covalent bonds. In such a bond there is a charge separation with one atom being slightly more positive and the other more negative‚ i.e.‚ the bond will produce a dipole moment. On the other hand‚ Ionic bonds are bonds in which one or more electrons from one atom are removed and attached to another atom‚ resulting in positive and negative ions which attract each other. In the extreme case where one or more
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