Chemistry

Unit: Atomic Structure

Name: ______Date: ______MOD: _____

Extra Credit: Atomic Structure (Must be completed individually)

  1. Which atomic theory is the most common?
  2. Quantum Theory
  3. John Dalton
  4. Ernest Rutherford
  1. What do atoms of the same element have in common?
  2. Same number of electrons
  3. Same number of protons
  4. Same number of neutrons
  1. An atom with an atomic number of 12 and a mass of 24 contains how many electrons, protons, and neutrons?
  1. Which of these has 28 protons and 26 electrons?
  2. Fe
  3. Fe2+
  4. Ni
  5. Ni2+

Use the following diagram to answer question 5.

  1. The isotopes of Uranium have different:
  2. Mass numbers
  3. Chemical behaviors
  4. Atomic numbers
  5. Positions on the periodic table
  1. An atom with an atomic number 60 and a mass number 125 contains ______protons, ______neutrons, and ______electrons.
  1. Which part of Dalton’s Atomic Theory is not longer considered to be true?
  1. The smallest part of an element that still has the properties of the element is the ______.
  1. Scientist now believe that the location and movement of an electron is best described as a ______of electrons. This is the ______mechanical model.
  1. Given the isotopic notation Zn64 and Zn66 answer the following question:
  1. The isotopes have different ______
  1. A student tries to identify an element that is in a unmarked bottle. The element is very shiny and is a good conductor of electricity. The element is a
  2. Metal
  3. Non-metal
  4. Metalloid
  1. The same student picks up another unmarked bottle containing another element. This element is yellow, brittle, and conducts heat poorly. This element is a
  2. Metal
  3. Non-metal
  4. Metalloid
  1. Another element has properties of metals and nonmetals. This element is probably a
  2. Metal
  3. Non-metal
  4. Metalloid
  1. The periodic table shows a repeating pattern of elements when the elements are arranged according to increasing ______number.
  1. The third period of elements contains ______energy levels.
  1. The Roman numeral “A” number group number tells you how many ______are in the outermost energy level.
  1. How many unpaired electrons are in each of the following?
  2. C = ______
  3. P = ______
  4. S = ______
  5. Ne = ______
  1. Which orbital(s) are in the first energy level? ______
  1. Which orbital(s) are in the second energy level? ______
  1. Which orbital(s) are in the third energy level? ______
  1. Given the orbital notation 3d7.
  2. The 3 is the ______
  3. The d is the ______
  4. The 7 is the number of ______
  1. The Cl atom has atomic number of 17. How many unpaired electrons does it have? ______
  1. Give the correct electron configuration for each of the following elements below:
  2. Cl ______
  3. C ______
  1. Look at the electron configurations below and identify each element.
  2. 1s22s22p63s23p5 ______
  3. 1s22s22p63s23p6 ______
  1. What general statement can you say about the noble gases? ______
  1. Given the data below, fill in the missing information.

Isotope / Atomic number / Mass number / Protons / Electrons / Neutrons / Charge
G / 17 / 19 / -1
H / 90 / 42 / 40
  1. Arrange the following groups of elements in order of increasing atomic radius.

Al, Mg, Na, S, Si ______

  1. Arrange the following groups of elements in order of increasing first ionization energy. As, Bi, N, P, Sb ______
  1. Arrange the following groups of elements in order of increasing electronegativity.

Al, Cl, Mg, Na, S, Si, ______