Matter Test - Review
Name:________________________
November 2011
I. Vocabulary
A.
All blocks
1. matter – Anything that has mass and takes up space.
2. atom - An extremely small particle that is the basic unit of matter and is composed
mainly of protons, neutrons, and electrons.
3. proton – Positively charged particle located in the nucleus of an atom.
4. neutron – A particle without a charge that is found in the nucleus of an atom.
5. electrons- Negatively charged particles that are the lightest of the three main particles
found in an atom and that form a cloud around the atom’s nucleus.
6. nucleus – The extremely dense central core of an atom. Almost the entire mass of the
atom is concentrated in the nucleus, which occupies only a tiny fraction of the atom's
volume. The nucleus of an atom consists of neutrons and protons.
7. element - Natural or synthetic (man-made) matter that is made up of only one type of
atom.
8. periodic table - A chart that organizes all known elements by the number of protons in the
nucleus of each element.
9. electron cloud (shell) - Region of space around the nucleus that have electrons with about
the same energy and are about the same distance from the nucleus.
10. atomic number – Number of protons in the nucleus of an atom.
11. atomic mass (weight) - Mass of the whole atom.
12. mass number – Sum of number of protons and number of neutrons in the nucleus of the
atom. It is found by rounding the atomic mass.
13. volume – The amount of space taken up by matter.
14. mass – Amount of matter in an object.
15. density – A physical property of matter that can be found by dividing the mass of a
material by its volume.
16. molecule – A group of two or more atoms that function as a unit because the atoms are
tightly bound together. It can be atoms of the same element or atoms of different
elements.
17. compound - A form of matter made by chemically combining two or more different
elements.
18. mixture- A combination of two or more substances that are not chemically combined and
can be separated by physical means.
19. chemical formula- Notation made up of the symbols of the elements and number of
elements in a compound.
B. Blocks 1, 3, and 5
1. electron subshell – Region of space within a shell that contains electrons with the same
energy.
2. orbitals – Region of space within a subshell where an electron is most likely to be found.
3. homogeneous mixture – A mixture that contains only one visibly distinct phase (part),
which has uniform properties throughout.
4. heterogeneous mixture – A mixture that contains visibly different phases (parts), each of
which has different properties.
5. solution – A homogeneous mixture of two or more substances in which each substance
retains its own chemical identity.
6. solute - The substance that is dissolved to form a solution.
7. solvent - The substance that dissolves a solute to form a solution.
8. solubility - Amount of a solute that will dissolve in a specific solvent under given
conditions. The dissolved substance is called the solute and the dissolving fluid (usually
present in excess) is called the solvent, which together form a solution. The process of
dissolving is called solvation, or hydration if the solvent is water.
9. miscibility - The property of various substances, particularly liquids, that allows them to
be mixed together and form a single homogeneous phase. For example, water and ethanol
are miscible in all proportions. By contrast, substances are said to be immiscible if they
cannot be mixed together, for example, oil and water.
II. Drawing an Atom
A. Calculating protons, neutrons, and electrons
1.
2.
3.
4.
Number of Protons = Atomic Number
Number of Electrons = Atomic Number
Mass Number = Rounded (Atomic Mass)
Number of Neutrons = Mass Number – Atomic Number
B. Protons and Neutrons in the Nucleus
C. Electrons on the Shells (2n2) (2, 8, 18, 32, 50)
III. Compounds and Mixtures
A. How are they alike?
1. Compounds and mixtures are alike because they both are made of 2 or more different
elements.
B. How are they different?
1. Compounds are made of 2 or more different elements chemically combined. (ex. H2O)
2. Mixtures are made of compounds and/or elements that are not chemically combined. (ex.
NaCl combined with H2O is salt water)
C. Draw an element, compound, and mixture.
1. Refer to the gumdrop drawings we did in class.
IV. Physical and Chemical Properties and Changes
A. Definitions
1. physical property – A characteristic of matter that can be observed by the senses – for
example, shape, size, taste, texture, color, and form.
2. physical change – A change in the shape, size, form, or state of matter that can be
observed without changing the identity of the matter.
3. chemical property – A characteristic of a substance that permits its change to a new
substance – for example, the ability to burn and the ability to react with oxygen.
4. chemical change – The change of materials into other, new materials with different
properties.
B. Recognize physical and chemical properties and changes. Review labs.
V. Element Symbols And Chemical Formulas
A. Element Names and Symbols
C = Carbon
O = Oxygen
Ag = Silver
He = Helium
Mg = Magnesium
Ca = Calcium
B = Boron
Sn = Tin
H = Hydrogen
Cl = Chlorine
Au = Gold
N = Nitrogen
Hg = Mercury
P = Phosphorus
Al = Aluminum
I = Iodine
Fe = Iron
Zn = Zinc
Na = Sodium
K = Potassium
S = Sulfur
F = Fluorine
Pb = Lead
Cu = Copper
Si = Silicon
B. Chemical Formulas
1. Counting Atoms
a) H2O = Hydrogen 2, Oxygen 1
b) 2NaCl = Sodium 2, Chlorine 2
c) Mg(OH)2 = Magnesium 1, Oxygen 2, Hydrogen 2
2. Determine the Reactants and Products
a) Ex. Cu + 2AgNO3 => 2Ag + Cu(NO3)2
Reactants = Cu + 2AgNO3
Products = 2Ag + Cu(NO3)2
3. Balancing Equations (Blocks 1, 3, and 5)
a) Unbalanced Equation
Balanced Equation
NaCl + BeF2 => NaF + BeCl2
2NaCl + BeF2 => 2NaF + BeCl2
VI. Scientists
A. Democritus
Greek philosopher who believed that everything in the universe was made up of tiny
indestructible particles called atoms.
B. Lavoisier, Antoine
A French chemist that showed that matter cannot be created or destroyed which is the
Law of Conservation of Mass.
C. Joseph Louis Proust
A French chemist that stated substances are always put together in the same way. For
example water is always 2 hydrogen and 1 oxygen. (Law of Constant Composition)
D. John Dalton
An English chemist who introduced a model to describe matter and atoms.
E. Dmitri Mendeleev
Russian chemist who created a compact graphical method for representing elements in
order of increasing atomic number. His work resulted in the Periodic Table we use
today.