Name:Number: Period:Date:

Chemistry Final Review

Review #1: Atomic Structure & Periodic Table

1a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass.

1b. Students know how to use the periodic table to identify metals, semimetals, non-metals, alkali metals, alkaline earth metals and transition metals and halogens.

1c. Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass.

1d. Students know how to use the periodic table to draw atoms and determine the number of electrons available for bonding.

1e. Students know how to use the periodic table to create an ion and can explain the trends of ionization energy for each atom.

THE ATOM

Atomic Structure: label each part of the atom, its charge, and relative mass.

  1. Describe the size and mass of the nucleus compared to the electron cloud:

Atomic mass and number
1. The periodic table is organized according to increasing ______.
Xe
Mass:
Atomic #:
Protons:
Electrons:
Neutrons:
Mass: Atomic #: Protons: Electrons: Neutrons:
Valence Electrons:
What are valence Electrons?
Why are valence electrons important?

PERIODIC TABLE

Identifying Groups: color code each important group and list it’s group number and properties in the space below:

Metals:
Non-metals:
Semi-metals:
Alkali metals:
Alkaline earth metals:
Transition metals:
Halogens:
Noble gases:
Periodic Trends
  1. Electronegativity:
  1. Ionization energy:
  1. Atomic/Ionic Size:

Exit Slip

  1. Which of the following ordered pairs of elements shows an increase in atomic number but a decrease in average atomic mass?
  2. Ag to Pd c. Co to Ni

b. Ge to Snd. Cr to Mo

  1. Chlorine (Cl) is placed after sulfur (S) on the periodic table because:
  2. S has one less electron than Cl
  3. S has one more proton than Cl
  4. S has one more neutron than Cl
  5. S has one less proton than Cl
  1. The neutral element has ____ protons, ____ electrons, and ____ neutrons.
  2. 21 protons, 20 electrons, 20 neutrons
  3. 20 protons, 20 electrons, 21 neutrons
  4. 41 protons, 20 electrons, 20 neutrons
  5. 20 protons, 21 electrons, 20 neutrons
  1. Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons. Which of the following statements best describes the trend in electronegativity seen in the periodic table?
  2. Changes little in a group, but increases as you move across a period.
  3. Decreases as you move down a group and across a period
  4. Decrease as you move down a group, but increases as you move across a period.
  5. Increases as you move down a group and across a period
  1. Which of the following elements is classified as a halogen? (choices b and d in the next column)
  2. Lithium (Li)c. Oxygen (O)
  3. Beryllium (Be)d. Bromine (Br)
  1. As you move down a group on the periodic table, atomic radius
  2. Increases
  3. Decreases
  4. Remains the same
  5. Increases then decreases
  1. As you move down a group on the periodic table, ionization energy
  2. Increases
  3. Decreases
  4. Remains the same
  5. Increases then decreases
  1. Iodine would have properties most like:
  2. Chlorine (Cl)
  3. Xenon (Xe)
  4. Manganese (Mn)
  5. Tellurium (Te)
  1. Calcium (Ca) is a:
  2. Metal
  3. Non-metal
  4. Alkali metal
  5. Semimetal
  1. Which of the following is an alkali metal?
  2. Magnesium (Mg)
  3. Strontium (Sr)
  4. Potassium (K)
  5. Argon (Ar)
  1. Compared to the nucleus, the electron cloud is
  2. Large with most of the mass
  3. Large with very little mass
  4. Small with most of the mass
  5. Small with very little mass

Name:Number: Period:Date:

Take Home Quiz # 1: Atomic Structure, Periodic Table (Justify on back)

  1. How many valence electrons does chlorine have?
  2. 1
  3. 3
  4. 7
  5. 8
  1. As you move down a group on the periodic table, electronegativity
  2. Increases
  3. Decreases
  4. Remains the same
  5. Increases then decreases
  1. Ionization energy is the energy it takes to remove an electron from an neutral atom to make a cation. Which of the following statements best describes the trend in ionization energy seen in the periodic table?
  2. Does not change as you move down a group, but increases as you move across a period.
  3. Decreases as you move down a group and across a period
  4. Decreases as you move down a group, but increases as you move across a period
  5. Increases as you move down a group and across a period.
  1. Place the elements in order of increasing (smallest to largest) atomic size: Cesium (Cs), Potassium (K), Rubidium (Rb)
  2. Cs, K, Rb
  3. Rb, Cs, K
  4. K, Rb, Cs
  5. Cs, Rb, K
  1. Which of the following is a transition metal?
  2. Calcium (Ca)
  3. Magnesium (Mg)
  4. Fluorine (F)
  5. Zinc (Zn)
  1. The neutral element has _____ protons, _____ electrons, and _____ neutrons.
  2. 11 protons, 12 electrons, 11 neutrons
  3. 11 protons, 11 electrons, 23 neutrons
  4. 23 protons, 11 electrons, 12 neutrons
  5. 11 protons, 11 electrons, 12 neutrons
  1. Which of the following could you predict to be true about the chemical behavior of Beryllium (Be) and Strontium (Sr)?
  2. Be and Sr have the exact same chemical properties
  3. Be and Sr have similar chemical properties, but Sr is typically more reactive than Be
  4. Be and Sr have very different chemical properties
  5. Be and Sr have similar chemical properties, but Be is typically more reactive than Sr.
  1. Lithium (Li) is typically classified as:
  2. An alkali metal
  3. An alkaline earth metal
  4. A transition metal
  5. A halogen
  1. Chlorine is a:
  2. Nonmetal
  3. Halogen
  4. Noble gas
  5. Both a and b
  6. Both a and c
  1. Which of the following is a semimetal?
  2. Silicon (Si)
  3. Lithium (Li)
  4. Gallium (Ga)
  5. Cadmium (Cd)