Transcript Exam Review - Manistique Area Schools

Chemistry
Semester One
EXAM REVIEW
Chapter 3 Vocab
 Atom
 Pure Substance
 Element
 Compound
 Mixture
 Heterogeneous
(colloid/suspension)
 Homogeneous
(solution)
 Law of Conservation of
Mass
 Physical Property
 Intensive
 Extensive
 Physical Change
 Chemical Property
 Chemical Change
 States of Matter
Chapter 3
 What type of property is observed when
milk sours?
 a. an intensive property
 b. an extensive property
 c. a chemical property
 d. a physical property
Chapter 3
 Which of the following is a compound?
 a. steel
 b. water
 c. neon
 d. crude oil
Chapter 3
 Seaweed is not a substance because ______.
 A. It is salty
 B. It is a liquid
 C. Its composition may be different from
sample to sample
 D. It has hydrogen as part of its composition.
Chapter 4 vocab
 Atom
 Nucleus
 Electron cloud
 Subatomic Particles
 Proton
 Neutron
 Electron
 Isotope + Symbols
 Mass Number
 Atomic Number
 Dalton
 Thompson –
 Plum Pudding Model
 Rutherford
 Nuclear Model
 Gold Foil
Experiments
Chapter 4
 Atoms with the same number of protons, but
different numbers of neutrons
 A. radioactive
 B. atomic mass unit
 C. Dalton’s elements
 D. isotopes
Chapter 4
 For the Copper Isotope, Copper-65, please
write the symbolic notation and identify the
number of protons, neutrons and electrons in
the atom. Also list the atomic number and
the mass number.
Chapter 4
 Briefly describe the structure of the atom
according to modern atomic theory. Include
the two main areas of the atom, all of the
subatomic particles, along with the
subatomic particles’ charges, location and
relative size.
Chapter 5 - vocab
 Electron cloud
 Principal Energy
Level
 Sublevel
 Atomic Orbital
 Filling Order
 Atomic Emission
Spectra
 Waves





Ground State
Quantum
Photon
Valance Electrons
Electron
Configuration
Notation
 Noble Gas Notation
 Electron Dot
Structure
Chapter 5
 Write the electron configuration notation and
nobles gas notation for the following:
 Magnesium
 Bromine
 Germanium
 Iodine
 Aluminum
Chapter 5
 What causes an atomic emission spectrum?
What does each line in a atomic emission
spectrum represent? Why are there spaces
between the lines of color? Why do we see
one color?
Chapter 6-7
 Antoine LaVoisier
 John Newlands
 1864
 “Law of octaves”
 Dmitri Mendeleev (Russian)
 1869
 Mendeleev was able to predict the properties of
undiscovered elements
 Henry Moseley
 1913
 Atomic #
Chapter 6-7
Representative
Transition
Inner
Lanthanide
Transition
Actinide
Chapter 6-7
Electronegativity, ionization energy increases
Atomic and ion size (radius) increases
Electronegativity/ionization NRG decreases
Atomic and ion size (radius) decreases
Chapter 8
 Would you expect a positively charged ion to
be larger or smaller than the “parent” atom?
Explain your reasoning.
 Would you expect a negatively charged ion to
be bigger or smaller than the “parent” atom?
Chapter 8-9
 For the following compounds, write formulas:
 Iron (III) oxide
 Carbon tetrafluoride
 Potassium Oxide
 Sulfuric Acid
 Hydrosulfuric Acid
 Manganese (III) hydroxide
 Dinitrogen Tetrahydride
Chapter 8-9
 Compare the melting points, conductivity
and malleability fro ionic, covalent and
metallic compounds.