Atomic Concepts
State two conclusions about the atom that resulted from Ernest Rutherford's gold foil experiment.
What is (1) the atom is mostly empty space, and (2) atoms have a small, dense, positive nucleus.
Describe a laboratory procedure that can be used to recover the solid solute from the aqueous solution.
What is evaporation, boiling, or distillation
Which type of bonding is found in all molecular substances?
What is covalent bonding
Heat is added to a 200.-gram sample of H2O(s) to melt the sample at 0°C. Determine the total amount of heat required to completely melt the sample.
What is q=mHf, so 66,800J
Which subatomic particles are located in the nucleus of an He-4 atom?
What is protons and neutrons
The elements on the Periodic Table are arranged in order of increasing ...
What is atomic number
What is the total mass in grams of 0.75 mole of SO2?
What is 48 grams
Which type of bonding is characteristic of a substance that has a high melting point and electrical conductivity only in the liquid phase?
What is ionic bonding
A 200-gram sample of H2O(ℓ) is heated from 0°C to a final temperature of 65°C. Calculate the total amount of heat required to raise the temperature of the H2O(ℓ) from 0°C to its final temperature.
What is q=mdCT, or 54,340 J
An atom of which element has the greatest attraction for electrons in a chemical bond?
What is Fluorine, because it has the highest electronegativity
Glycine, NH2CH2COOH, is an organic compound found in proteins. Calculate the gram-formula mass of glycine.
What is 75 g/mole
Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar?
What is the shape of the CO2 molecule is symmetrical
Compare the amount of heat required to vaporize a 200.-gram sample of H2O(ℓ) at its boiling point to the amount of heat required to melt a 200.-gram sample of H2O(s) at its melting point.
The heat of vaporization is higher, so it takes more heat to vaporize than it does to melt.
Explain, in terms of subatomic particles, why the radius of a chloride ion is larger than the radius of a chlorine atom.
What is the ion has gained an electron
Describe the trend in ionization energy as elements in Period 3 are considered in order of increasing atomic number.
What is the ionization energy increases
2NaHCO3(s) + heat → Na2CO3(s) + H2O(g) + CO2(g) Identify the type of chemical reaction represented by the equation.
What is decomposition
What is the total number of electron pairs shared between the carbon atom and one of the oxygen atoms in a carbon dioxide molecule?
What is 2
In a laboratory, a student makes a solution by completely dissolving 80.0 grams of KNO3(s) in 100.0 grams of hot water. The resulting solution has a temperature of 60.°C. Classify, in terms of saturation, the type of solution made by the student.
What is unsaturated
Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found?
What is group 16
2NaHCO3(s) + heat → Na2CO3(s) + H2O(g) + CO2(g) State evidence that indicates the entropy of the products is greater than the entropy of the reactant.
What is phase change from solid to gas and 1 reactant to several products (increase in disorder)
Oxygen, nitrogen, and fluorine bond with hydrogen to form molecules. These molecules are attracted to each other by ...
What is hydrogen bonds
Compare the boiling point of a NaCl(aq) solution at standard pressure to the boiling point of pure water at standard pressure.
What is boiling point of a solution is always higher than that of water (colligative properties)