4-1: ATOMIC STRUCTURE (page 104-110)
à Atoms are made up of 3 types of subatomic particles:
· ______—positively charged, mass of about 1 a.m.u., located in the nucleus.
· ______—have no charge, mass of about 1 a.m.u., located in the nucleus.
· ______—negatively charged, very small mass—about 1/1800 the mass of a proton, located in the electron cloud around the outside of the nucleus.
à The Nucleus
· The small, dense, ______charged center of the atom.
· Contains ______and ______.
· Contains 99.9% of the atom’s mass.
· About 1/100,000 the size of the entire atom. (Think of a ______in the center of a football stadium!)
à Outside the Nucleus
· Danish scientist Niels Bohr said that electrons moved in set paths around the nucleus, similar to the way the ______orbit the ______.
· Later, scientists said that instead of being in definite paths around the nucleus, there were locations where electrons were likely to be found. This region is called the ______.
· Within the electron cloud, electrons with different amounts of energy exist in different ______.
· Within each energy level, electrons are most likely to be found in regions called ______. There are four different kinds of ______: ____, ____, ____, and ____. The simplest kind (“s”) has a shape like a ______.
· An electron in the outermost energy level of an atom is called a ______. These ______electrons determine the chemical properties of the atom.
4-2: A Guided Tour of the Periodic Table (page 111-119)
à Periodic Law—states that the repeating ______and ______properties of elements change periodically with the elements’ ______.
· Examples:
̶ Copper, silver and gold are all in the same vertical column on the periodic table. These elements have similar properties: all are good conductors of heat and electricity, all are malleable.
̶ He, Ne, Ar, Kr, Xe and Rn are all gases at room temperature, they do not react with other substances easily.
à Horizontal rows on the periodic table are called ______. The number of protons and electrons in the elements increases by one as you move from left to right across one of these rows.
· Example: Going from left to right in the 4th period, K has 19 protons and electrons; Ca has 20 protons and electrons, etc.
à Vertical columns on the periodic table are called ______or ______. Atoms of elements in the same vertical column have the same number of ______, and so these elements also have similar ______.
· Example: Going down group 17: F, Cl, Br, I, and At all have 7 ______.
à Atomic Number—the number of ______in an atom’s nucleus.
· The symbol used to represent atomic number is ______.
· All atoms of a particular element have the same atomic number.
· Examples:
- All hydrogen atoms have ______in their nucleus, and thus have an atomic number of 1.
- All ______atoms have 82 protons in their nuclei, and thus have an atomic number of 82.
à Typically, the number of protons in an atom equals the number of electrons in the atom. Therefore, we say that atoms are ______charged.
à Atoms are considered to be chemically stable when they have their valence shell completely full of electrons. Atoms can gain, lose, or share their electrons in order to get a full valence shell. When an atom either gains one or more electrons or loses one or more electrons, the atom is no longer neutrally charged. When an atom or a group of atoms has either a negative or a positive charge it is called an ______.
à Isotopes—atoms of an element that have the same number of protons as another atom of that element, but have a different number of ______.
à Example—isotopes of hydrogen:
Protium Nucleus Deuterium Nucleus Tritium Nucleus
H-1 H-2 H-3
à Mass Number and Average Atomic Mass
· ______(amu)—unit used to measure the masses of subatomic particles.
· Mass Number—the sum of the ______and ______in an atom’s nucleus. Remember: this means ADD them!!
- Mass number is always a whole number!!
· Examples:
- One isotope of carbon has 6 protons and 6 neutrons in the nucleus. Its mass number is 12 (6 + 6 = 12)
- Another isotope of carbon has 8 neutrons in the nucleus. What is its mass number?
- An atom of some element has 11 protons and 13 neutrons in the nucleus. What is the element? ______What is its mass number? ______
· Average Atomic Mass—the weighted ______of the masses of the naturally occurring isotopes for an element. This is the number that appears on the periodic table in each element’s block.
- Average atomic mass is usually not a whole number.
- Example: the average atomic mass for: Mg is _____ amu; B is ______amu
4-3: Families of Elements (page 120- 128)
à Elements are classified into 3 groups:
• Metal (define it)—
§ Where are metals found on the periodic table?
§ List 5 examples of metals.
• Nonmetal (define it)—
§ Where are nonmetals found on the periodic table?
§ List 5 examples of nonmetals.
• Semiconductors also known as ______(define it)—
§ Where are semiconductors found on the periodic table?
§ List the 6 semiconductors your book mentions on pg. 127.
à METALS—there are 3 categories of metals:
• ______—these metals are found in Group 1.
§ List the elements in this category.
§ List a few physical and chemical properties of elements in this category.
§ How many valence electrons do the elements in this category have?
• ______—these metals are found in Group 2.
§ List the elements in this category.
§ List a few physical and chemical properties of elements in this category.
§ How many valence electrons do the elements in this category have?
• ______—one of the elements found in Groups 3-12
§ List 5 of the elements in this category.
• Some elements, such as technetium and promethium are ______.
à Non-Metals
• ______—these non-metals are found in Group 17.
§ List the elements in this category.
§ List some physical and chemical properties of elements in this category.
§ How many valence electrons do the elements in this category have?
• ______—these non-metals are found in Group 18.
§ List the elements in this category.
§ List some physical and chemical properties of elements in this category.
§ Why are elements in this group unreactive?
§ How many valence electrons do most elements in this category have?
à Semi-Conductors
• What is the main use of semi-conductors?
4-4: Using Moles to Count Atoms (pg. 129-134)
à Mole (define it)—
· List some other counting units (other than the mole) that you know of:
· How many individual items are in each of the counting units you listed above?
· How many individual items are in one mole?
· What is this number called?
à Molar Mass (define it)—
· Example: The molar mass of silver is 107.8682 g/mol.
· Use a periodic table to find the molar masses of the following elements:
Ca Cu Xe Be Ba
· An element’s molar mass can be used as a conversion factor to convert moles to grams or grams to moles.
· Example: What is the mass of 2.7 moles of neon gas?
2.7 mol Ne / 20.1797 g1 / 1 mol Ne
· How many moles of mercury are in 150 g of Hg?
150 g Hg / 1 mol Hg1 / 200.59 g Hg