Chapter 6 Section 3: Naming compounds and writing formulas Key Concepts: What information do the name and formula of an ionic compound provide? What information.

Chapter 6Section 3:

Naming compounds and writing formulasKey Concepts:

• What information do the name and formula of an ionic compound provide?

• What information do the name and formula of a molecular compound provide?

Question 1:

What does the formula of an ionic compound describe?.

Answer: The formula of an ionic compound describes the ratio of the ions in the compound.

Question 2:

How did the discovery of new elements such as gallium demonstrate the usefulness of Mendeleev’s table?

Answer: The close match between Mendeleev’s predictions and the actual properties of new elements showed how useful his periodic table could be.

Question 3:

Scientists before Mendeleev had proposed ways to organize the elements. Why were Mendeleev’s efforts more successful?

Answer: Mendeleev provided an organizing principle that worked for all off the known elements.

Question 4:

What characteristic of solitaire did Mendeleev use as a model for his periodic table?

Answer: In solitaire, cards are arranged into categories called suits and ordered by value.

Question 5:

Why did Mendeleev leave spaces in his table?

Answer: In order to place elements with similar properties in the same column, Mendeleev needed to leave spaces for undiscovered elements.

Question 6:

In general, how can a scientist test the correctness of a scientific model?

Answer: The scientist tests weather the model can be used to make accurate predictions.

Question 7:

Explain why it would not have been possible for a scientist in 1750 to develop a table like Mendeleev’s.

Answer: With only 17 known elements to work with, the scientist would not have had enough data.

Question 8:

How was Mendeleev able to predict the properties of elements that had not yet been discovered?

Answer: Mendeleev based his predictions on the properties of nearby elements and other elements in the same column.

Chapter 5Section 2:

The Modern Periodic TableKey Concepts:

• How is the modern periodic table organized?• What does the atomic mass of an element depend on?

• What categories are used to classify elements on the periodic table?• How do properties vary across a period in the periodic table?

Question 1:

What determines the order of the elements in the modern periodic table?

Answer: In the modern periodic table, elements are arranged by increasing atomic number.

Question 2:

Describe the periodic law.

Answer: Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups.

Question 3:

What two factors determine the atomic mass of an element?

Answer: Atomic mass is a value that depends on the distribution of an element’s isotopes in nature and the masses of those isotopes.

Question 4:

Name three categories that are used to classify the elements in the periodic table.

Answer: Metals, nonmetals, and metalloids.

Question 5:

What major change occurs as your move from left to right across the periodic table?

Answer: The elements become less metallic and more nonmetallic in their properties.

Question 6:

The atomic mass of iodine (I) is less than the atomic mass of tellurium (Te). But an iodine atom has one more proton than a tellurium atom. Explain how this situation is possible.

Answer: Answers may include that the tellurium isotopes that are most abundant have many neutrons in their nuclei or that all tellurium atoms have more neutrons than iodine atoms.

Question 7:

Explain how you know that no new element with an atomic number less than 100 will be discovered.

Answer: The atomic number of an element corresponds to the number of protons in the element’s atoms. The atomic number must be a whole number. All the places between 1 and 100 are already filled with existing elements.

Question 8:

Compare the reactions with water of the elements sodium and magnesium.

Answer: Sodium reacts quickly and violently with water at room temperature. Magnesium will not react unless the water is hot.

Chapter 5Section 3:

Representative GroupsKey Concepts:

• Why do the elements in a group have similar properties?• What are some properties of the A groups in the periodic table?

Question 1:

Explain why elements in a group have similar properties.

Answer: They have similar properties because they have the same number of valence electrons.

Question 2:

What is the relationship between an alkali metal’s location in Group 1A and its reactivity?

Answer: The reactivity of alkali metals increases from the top of Group 1A to the bottom.

Question 3:

What element exists in almost every compound in your body?

Answer: Carbon

Question 4:

Which Group 5A elements are found in fertilizer?

Answer: Nitrogen and phosphorus.

Question 5:

Which group of elements are found in fertilizer?

Answer: The noble gases (Group 8A)

Question 6:

Why is hydrogen located in a group with reactive metals?

Answer: Hydrogen is placed with other elements that have a single valence electron.

Question 7:

What biological function requires magnesium?

Answer: The process that uses sunlight to produce sugar in plants.

Question 8:

Why is aluminum recycled?

Answer: The energy needed to purify recycled aluminum is only about 5% of the energy needed to extract aluminum from bauxite.

Question 9:

What is the main use of sulfur?

Answer: To produce sulfuric acid.

Question 10:

Why is chlorine added to drinking water?

Answer: Chlorine is added to drinking water to kill bacteria.

Question 11:

In which class of elements is there a greater range of properties, the metals or the nonmetals? Give an example to support your answer.

Answer: Accept all answers that are supported by reasonable arguments. Students may choose nonmetals and say that they display a greater range of physical properties and reactivity.

Question 12:

What happens to the reactivity of nonmetals within a group from the top of the group to the bottom?

Answer: The reactivity of nonmetals decrease from the top to the bottom of a group.