A) Hydrogen bonds are strong enough to confer structural stability, for example in DNA. B) Hydrogen bonds are weak enough to be easily broken (weaker than covalent bonds). C) They contribute to the water solubility of many macromolecules. D) All of the above Answer: D Page Ref: Section 5 27) London dispersion forces are attractive forces that arise due to A) infinitesimal dipoles generated by the constant random motion of electrons. B) permanent dipoles of molecules containing covalent bonds between atoms of very different electronegativities.
It is known that chlorine is more electronegative than bromine, and thus chlorine is more reactive, and less discriminatory as to what it will react with, thus making bromine more “selective”. Another pertinent piece of information to look at would be stability. The stability of a free radical increases as the number of carbon substituents increases. Therefore, primary is the least stable and tertiary is the most stable. Also, the more stable the free radical that is left behind, the weaker its C-H bond strength will be.
For one mole of gas, the difference between Cp and CV is the constant R (R is the so called universal gas constant) and represents the capacity of the gas to perform expansion work at constant applied pressure. {Cp = CV+R for an ideal gas} Since, for solids and liquids, the constant pressure and constant volume Heat Capacities are the same, the subscript p or V on the 'C' is usually dropped. Q = m C DT This means that the proportionality between the Heat flow into (or out of) an object and the Temperature change of that object is the total Heat Capacity, which can be expressed as a molar property or per mass. if m is moles and C is molar Heat Capacity if m is mass (grams) and C is the Specific Heat Q is positive for a temperature increase because the system has undergone an endothermic change of
When atoms bond together they share or transfer electrons to achieve a more stable electron arrangement, often a full outer main level of electrons, like the noble gases. There are three types of strong chemical bonds: 1.__ionic______, 2.____covalent____ and metallic IONIC bonding • Ionic bonding occurs between metals and non-metals • Metal atoms 3. ___lose___ electrons • Non-metal atoms gain electrons • Positive and negative ions are formed Sodium chloride has ionic bonding. [pic] • The sodium ion is positively charged because it has lost a negative electron
A) double; covalent B) double; ionic C) single; covalent D) single; ionic E) triple; covalent 3. Which property could describe a covalent compound? A) It conducts electricity when melted. B) Has a low boiling point C) It is composed of a non-metal and a metal. D) It conducts electricity when dissolved in water.
With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide. In the reaction the free halogen (X2) oxidizes the other halide ion (Y-) and gets reduced by gaining electron(s). In table 3, chlorine was the strongest oxidizing agent and iodine was the weakest oxidizing agent. Since chlorine was the strongest oxidizing agent it will react more and the weak agent will react less. This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil.
A) gas B) solid C) salts D) ice E) liquid 3. A small amount of salt dissolved in water is an example of a __________. A) compound B) solid C) heterogeneous mixture D) pure substance E) homogeneous mixture 4. Which of the following is an illustration of the law of constant composition? A) Water is 11% hydrogen and 89% oxygen by mass.
When the hydrate is heated, it easily loses water molecules attached and becomes an anhydrous salt. The corresponding chemical reaction for hydrated magnesium sulfate can be written as |MgSO4•7H2O ( MgSO4 + 7H2O |(1) | where MgSO4 is the anhydrous salt. Usually,
Although, Ionic bonding is when an atom gives away elections to another atom, which only happens in a metal and a nonmetal, and they have high melting points and are soluble. By investigating the unknown
11.2 Particulate Model for Solids, Liquids and Gases A block of ice Solid molecules have a restricted motion = Solid A beaker of boiling water Gas molecules are able to move at extremely high speed = Gas A beaker of warm water liquid molecules have greater mobility = Liquid States of Matter Solid * In solids, the molecules are arranged close together in a regular pattern * Strong attractive intermolecular forces hold the molecules in position so they have definite shape and volume * They can only vibrate in their fixed positions Liquid * In liquids, the molecules are not arranged in a regular pattern and are slightly further apart then those in solids * The attractive intermolecular forces are not very strong. Thus, the molecules are able to move among one another, giving liquids its definite volume but not a definite shape. Gases * In gases, the molecules are widely spaced. Intermolecular forces are negligible * The molecules move about randomly with high speeds, colliding with the walls of the container, occupying any available space. Research on *phase changes for water* Heating curve (Please!!!!!!