Atomic Concepts
Periodic Table
Moles/Stoichiometry
Chemical Bonding
Physical Behavior of Matter
100

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.

100
Which Group 14 element is classified as a metal
What is lead, Pb
100

Describe a laboratory procedure that can be used to recover the solid solute from the aqueous solution.

What is evaporation, boiling, or distillation

100

Which type of bonding is found in all molecular substances?

What is covalent bonding

100

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

200

Which subatomic particles are located in the nucleus of an He-4 atom?

What is protons and neutrons

200

The elements on the Periodic Table are arranged in order of increasing ...

What is atomic number

200

What is the total mass in grams of 0.75 mole of SO2?

What is 48 grams

200

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

200

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

300
An atom in an excited state has an electron configuration of 2-7-2. Write the electron configuration of this atom in the ground state.
What is 2-8-1
300

An atom of which element has the greatest attraction for electrons in a chemical bond?

What is Fluorine, because it has the highest electronegativity

300

Glycine, NH2CH2COOH, is an organic compound found in proteins. Calculate the gram-formula mass of glycine.

What is 75 g/mole

300

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 

300

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.

400

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

400

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

400

2NaHCO3(s) + heat → Na2CO3(s) + H2O(g) + CO2(g) Identify the type of chemical reaction represented by the equation.

What is decomposition

400

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

400

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

500
The light emitted from a flame is produced when electrons in an excited state
What is fall back to the ground state and release energy
500

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

500

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)

500

Oxygen, nitrogen, and fluorine bond with hydrogen to form molecules. These molecules are attracted to each other by ...

What is hydrogen bonds

500

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)

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