Experiment 9 Empirical Formula of Zinc Iodide Objectives Upon completion of this experiment‚ students should have learned: 1. The law of conservation of mass. 2. How to calculate an empirical formula. 3. The concept of limiting reagents. Introduction Synthesis and the determination of empirical formulas are two extremely important parts of chemistry. In this experiment‚ you will synthesize zinc iodide and determine its empirical formula. The molecular formula gives the actual
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1. Define the term chemotherapy. Use of chemicals for therapeutic effect is called chemotherapy. 2. Why do we need to classify drugs in different ways ? It is useful for doctors because it provides them the whole range of drugs available for the treatment of a particular type of problem. 3. How are drugs classified? (a) On the basis of pharmacological effect For example‚ analgesics have pain killing effect. (b) On the basis of drug action It is based
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with halogens to produce salts‚ most important NaCl and KCl. Sodium Chloride is used as a preservative for meat and to melt the ice on the roads. KCl is important for plant fertilizers since potassium helps plant growth. The metal halides form white ionic crystalline solids. They are all soluble in water except LiF because of a high lattice enthalpy due to the electrostatic attraction between Li+ and F- ions. All halogens are quite reactive‚ and in the natural world they always occur combined with
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pairs of electrons. A covalent bond involves the sharing of electrons Equal sharing of electrons results in a nonpolar covalent bond Electrons are shared in covalent bonds while ionic bonds involve the attraction between oppositely charged ions. Electrons are shared in covalent bonds‚ whereas ionic bonds involve the loss or gain of electrons. Hydrogen bonds are responsible to the attraction of water molecules to each other. This is what causes cohesion and surface tension of
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ion is simply a regular atom that is charged * It gets charged when electrons are gained or loss * During a reaction‚ atoms prefer to look like their closest Noble Gas atom in their valence shell * The ionic charge is the charge of the atom with a full valence shell Ionic
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covalent bonding of a molecule or ion. Covalent bonds are a type of chemical bonding formed by the sharing of electrons in the valence shells of the atoms. Covalent bonds are stronger than the electrostatic interactions of ionic bonds‚ but keep in mind that we are not considering ionic compounds as we go through this chapter. Most bonding is not purely covalent‚ but is polar covalent (unequal sharing) based on electronegativity differences. The atoms in a Lewis structure tend to share electrons so that
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pass through to lower its energy. This is connected to osmotic pressure because that is the pressure used to stop the molecules from passing through the semi-permeable membrane. Some solutes have different effects on the solutions. For example‚ ionic solutes dissolve and split when placed in a solution. The ions split into positives and negatives and produce multiple ion particles. This makes them affect colligative properties more than molecular
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orders were determined by the way that the top or capital of each column was sculpted. The first order was called the Doric Order. This was the most simple of the three. It was only meant for sturdiness‚ not for beauty. The second order was called the Ionic order. They had capitals sculpted like spiraling scrolls. They too were not that beautiful‚ but very sturdy. The third was the Corinthian Order. Ta the top of each capital of this order were carved Acanthus leaves. They were very beautiful‚ but not
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compound and the water molecules together. The forces of attraction are electrostatic forces resulting from the charged nature of the anhydrous ionic compound and the polar water molecules. Particle size and space limitations dictate the number of water molecules an ionic compound will accommodate and well as the conditions under which the hydrate is formed. Many ionic compounds form multiple hydrates and to remove all of the bound water for some of these can be difficult in ordinary laboratory conditions
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| | Answers are attached Enjoy Biology‚ 8e (Campbell) Chapter 7 Membrane Structure and Function Multiple-Choice Questions 1) Who was/were the first to propose that cell membranes are phospholipid bilayers? A) H. Davson and J. Danielli B) I. Langmuir C) C. Overton D) S. Singer and G. Nicolson E) E. Gorter and F. Grendel 2) Who proposed that membranes are a phospholipid bilayer between two layers of hydrophilic proteins? A) H. Davson and J. Danielli B) I. Langmuir
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