1. Interim 1 Review KEY
October, 2014

2. Periodic Table How is the periodic table organized?
In order of atomic number, grouped in columns by valence electrons and in rows by energy levels for those electrons.
The atomic number is the same number as ____the number of protons__ and ___electrons in a neutral atom ________
Why are groups in the Periodic Table called families?
Elements in a family have similar chemical properties, because they have the same number of valence electrons.
Name two characteristics of metals and well as two examples.
Good electrical conductors, thermal conductors, high luster (shiny), malleable, ductile.
Examples: gold, silver, iron, copper, nickel, anything to the left of the zig-zag metalloids
Name two characteristics of nonmetals as well as two examples.
Poor conductors of electricity and heat Brittle or gaseous, tend to take electrons in reactions.
Expl: oxygen, nitrogen, carbon (pencil lead, diamond), chlorine, sulfur
Name two characteristics of metalloids as well as two examples.
Somewhat like metals and non-metals. Semiconductors
Expl: silicon (high luster, bonds like carbon) Boron, antimony, germanium

3. Standards of Measurement
What are you measuring
Definition
SI Unit (Symbol)
Volume
How much space a substance fills
mL or cm3
Mass
How much matter is in a substance (based on amu’s)
Gram (g)
Weight
How much gravity pulls on a mass
Newton (N)
Time
Duration of an event
Second (sec)
Temperature
How fast molecules and atoms move (kinetic energy)
Kelvin (K)
Density
How much mass is in a given volume (mass per volume)
g/cm3 or g/mL
How do you calculate the volume of regularly shaped object?
Using displacement, how do you calculate the volume of an irregularly shaped object.
L x W x H
The difference in water level before and after an object is put into the water.
mL of water = cm3 of solid

4. Atoms and Molecules
What is Matter? Anything that takes up space and has mass
What is the law of conservation of matter? Matter is neither created nor destroyed in a chemical reaction
What is an atom? Smallest particle into which an element can be broken and still keep its identity (properties)
What is a molecule? Smallest particle into which a compound can be broken and still keep its identity (properties)
How is an atom different than a molecule? Atom is made of protons, neutrons, electrons … one element.
Atoms bond together to make compounds. They do this by sharing or transferring electrons with other atoms.
State two examples of a pure substance Pure elements: anything listed on the Periodic Table of Elements
Compounds: sugar, baking soda, water, sulfuric acid
What is a mixture? A combination of elements and/or compounds which are not chemically bonded to each other.
Homogeneous = same throughout (iced tea or KoolAid). Heterogeneous = not evenly mixed (tossed salad, salt & pepper)
Why is a mixture not considered a pure substance? Particles are not the same throughout. Can be divided into different components with out changing the identity of those components.
Define Element
All atoms have the same identity and are not chemically bonded with any other element(s)
Define Compound
Atoms of different elements sharing or exchanging electrons to form a substance with its own properties
Define Mixture
Combination of elements, compounds, etc which are not chemically bonded to each other.
What makes an element different than a compound and mixture?
All the same atoms
What makes a compound different than an element and mixture?
Atoms are chemically bonded together
What makes a mixture different than an element and compound?
Substances are mixed without bonding

5. The Atom and States of Matter
Parts of the Atom
Proton: Where is it located and what charge does it have?
In nucleus of atom; positive charge
Electron: Where is it located and what charge does it have?
Outside nucleus of atom, in electron cloud or shells; negative charge
Neutron: Where is it located and what charge does it have?
In nucleus of atom; no charge (neutral)
Name the two structures that make the nucleus.
Protons and neutrons
What part of the atom has the most mass? Nucleus has almost all of the mass of an atom
What part of the atom takes up the most space? Electron cloud takes up the most space
Solid (energy level and how do the particles move) lowest energy state … Atoms/molecules vibrate in place, not changing shape; definite volume
Liquid (energy level and how do the particles move)
Midrange energy state … Atoms/molecules move freely, slide past each other, take the shape of container; but has a definite volume
Gas (energy level and how do the particles move)
High energy state … Atoms/molecules move independently, take the shape and volume of container
Plasma(energy level and how do the particles move)
High energy state … Atoms/molecules move like a gas, but electrons have broken off, making ions – light is emitted

6. Properties of Matter Define Give Examples (as many as possible)
Physical Property
Color, luster, solubility, state of matter, density, mass, malleability, ductility, brittleness, viscosity, melting/freezing point, boiling point
Chemical Property
pH, reactivity (with acid, water, oxygen, etc), flammability, combustibility
How is a physical change different than a chemical change?
Physical: does not change the identity of the substance; it is more likely to be reversible.
Chemical: new substance is formed with new properties, chemical bonds have changed
Explain two physical changes
Explain two chemical changes
Dissolving sugar into water or tea.
Tearing a piece of paper or breaking pencil
Melting butter or metal
Reshaping metal into jewelry
These all have the same substance B4 & after
Caramelizing sugar (changes odor &color)
Burning wood or paper (gas produced, light and heat released, carbon ashes)
Both of these examples involve a substance reacting with oxygen in the air
What clues indicate a chemical change has occurred through your observations.
Included in answers above

7. Properties of Matter Vocabulary
Property
Definition
Chemical or Physical
Density
Amount of mass per unit volume
Physical
Precipitate
Solid forms when mixing 2 liquids
Chemical
Change of State
Changing solid, liquid, gas, plasma with the addition or removal of energy (especially heat)
physical
Melting Point
Temperature at which solid becomes a liquid (usually same temperature as freezing point: liquid  solid)
Boiling Point
Temperature at which liquid boils to rapidly vaporize
Malleability
Ability to be shaped or molded
Ductility
Ability to be drawn/pulled into wires
Reactivity
Likelihood to chemically react with another substance (expl reactive with oxygen, acids, bases, water, etc)
Combustibility
Likelihood to explosively react with oxygen
Conductor
Able to transmit electricity or heat
Vaporization
Liquid (or solid) changing to vapor (gas)

8. Periodic Table Vocabulary
Define the following terms
Atomic Mass Unit
The mass in one proton or neutron
Note: the atomic mass of an element is the weighted average of all naturally occurring isotopes
Mass Number
The number of protons + neutrons in a specific isotope of an element. Note: this is always a whole number
Period
Horizontal row in the periodic table – this represents how many energy shells have electrons in them. (expl,: the third row has electrons in levels 1, 2, and 3)
Group/Family
Vertical column of the periodic table – these elements are grouped together because they have the same number of valence (outer shell) electrons, and therefore have similar chemical properties
Valence Electrons
Electrons in the outermost electron shells. These electrons are the only ones that might interact with other elements to form chemical bonds. Atoms try to have a complete outer shell (usually 8 electrons)