9 week exam Review

History Periodic Trends

Metals, nonmetals, metalloids

Electrons Bonding

10 10 10 10 10

20 20 20 20 20

30 30 30 30 30

40 40 40 40 40

50 50 50 50 50

Question 1 - 10

• The modern periodic table lists elements in order of increasing atomic________.

Answer 1 – 10

Number

Question 1 - 20

• Describe Mendeleev’s periodic table.

Answer 1 – 20

He arranged elements in order of increasing atomic mass.

Question 1 - 30

Why is Mendeleev the “Father of the Modern Periodic Table” and not Meyer or both?

Answer 1 – 30

• Mendeleev correctly predicted physical properties of three unknown elements.

Question 1 - 40

How did Moseley update the Periodic Table?

Answer 1 – 40

After calculating the atomic number of elements, he rearranged the PT by increasing atomic number.

Question 1 - 50

• Assess the contributions of Mendeleev and Moseley to our modern understanding of the relationship between atomic structure and atomic behavior.

Answer 1 – 50

• Mendeleev’s PT was able to show that groups/families of elements have similar properties depending on the size of the nucleus. (able to predict properties of atomic behavior based on guessed atomic mass)

• Moseley expanded upon Mendeleev’s ideas with atomic number (number of protons) defining an atom and its properties.

Question 2 - 10

What is the trend for metallic reactivity across a period? (for example from sodium, to magnesium, then aluminum?)

Answer 2 – 10

• Chemical reactivity of metals generally decreases across a period.

Question 2 - 20

• What is ionization energy?

Answer 2 – 20

• Amount of energy needed to remove an electron to form a cation.

Question 2 - 30

• Describe the trend across a period and down a group for electronegativity.

Answer 2 – 30

• The trend across a period for electronegativity increases. It decreases as it goes down a group.

Question 2 - 40

• What is the trend for atomic radius on the periodic table?

Answer 2 – 40

• It decreases across a period and increases down a group.

Question 2 - 50

What is the most electronegative element, and what is its value?

Answer 2 – 50

Fluorine, 4.0

Question 3 - 10

• Where are the metals located on the periodic table?

Answer 3 – 10

• To the left and cover most of the periodic table.

Question 3 - 20

• What type of element is Tungsten?

Answer 3 – 20

• Transition metal

Question 3 - 30

What is a metalloid?

Answer 3 – 30

Solids that are semi-conductors that have properties in between metals and non-metals.

Located on the staircase.

Question 3 - 40

• Give 3 characteristics of a nonmetal

Answer 3 – 40

Gases at room temp/brittle if solidLow melting/boiling pointsNon-conductors

Question 3 - 50

• Describe metals’ role in bonding. (how do they bond?)

Answer 3 – 50

• They form cations (positive ions) by losing electrons (transfer to nonmetals). Therefore, they participate in ionic bonding.

Question 4 - 10

The main energy levels of an atom are indicated by the_________.

Answer 4 – 10

• Principal quantum numbers.

Question 4 - 20

At n=2, the total number of electrons that could be found is____.

Answer 4 – 20

8 electrons.

Question 4 - 30

• Which principle states that no two electrons in the same atom can have the same set of quantum numbers?

Answer 4 – 30

• Pauli exclusion

Question 4 - 40

• What is the electron configuration for aluminum?

Answer 4 – 40

1s22s22p63s23p1

Question 4 - 50

• What are the 4 quantum numbers for Sulfur?

Answer 4 – 50

3, 1, -1, -1/2

Question 5 - 10

What are three properties of a covalent compound?

Answer 5 – 10

1. Low melting/boiling points2. Non-conductors3. Wide variety of textures4. Do not form crystals

Question 5 - 20

• What shape will NH3 exhibit?

Answer 5 – 20

• Trigonal pyramidal

Question 5 - 30

The model used to describe and explain the bonding and arrangement of atoms in a solid metal is the_______

Answer 5 – 30

• Electron sea/sea of electrons model

Question 5 - 40

• What type of bonding exists between nitrogen and hydrogen?

Answer 5 – 40

• Polar-covalent bond

Question 5 - 50

Describe polar bonds and what leads to a polar covalent bond.

Answer 5 – 50

• Difference in electronegativity leads to an UNEQUAL sharing of electrons. One atom will pull the electron pair closer to it leaving a partial positive on the other atom while gaining a partial negative charge.