Download Chemistry Mid-term Study Guide A 2016

Name: ____________________________
Chemistry 2016 Mid-term Study Guide
Chemistry Skills
Convert each of the following:
345 mL = ____________ L
2.315 g = ____________ mg
421 cm = ____________ mm
0.0567 km = ____________ m
1.0 x 10-2 L = ______________ L
What is the metric base unit for:
Mass? ________________
Wet Volume? _______________
Distance? _______________
The metric prefixes from largest to smallest are kilo-, hecta-, deca-, deci-, centi- and milli-.
A __________________ has definite volume and definite shape.
A __________________ has definite volume but takes the shape of its container.
A __________________ has neither definite volume nor definite shape.
Label each of the following as a physical or chemical property.
Shape
physical or chemical
Melting Point
physical or chemical
Reactivity with Acid physical or chemical
Density
physical or chemical
Speed
physical or chemical
Boiling Point
physical or chemical
Odor
physical or chemical
Flammability
physical or chemical
In a ________________ change, the physical properties are adjusted (size, shape, density) but
the chemical composition remains the same.
In a ________________ change, the result is the formation of one or more new substances with
different chemical properties.
A change of state is not a _______________ change because the chemical identity of the
substance has not been altered. Water that is frozen has not undergone a chemical change
because it is still ___________________.
Classify the following as a physical or chemical change.
Burning wood
physical or chemical
Dissolving salt
physical or chemical
Cutting paper
physical or chemical
Freezing water
physical or chemical
Melting iron
physical or chemical
An _____________________ is a pure substance that cannot be broken down by ordinary
chemical means into simpler substances.
A ______________________ is a substance consisting of two or more different elements in
definite proportions joined by chemical bonds. The elements cannot be separated by physical
means.
A ______________________ is a substance consisting of two or more elements or compounds
that can be separated by physical means.
A _______________________ mixture is a combination of two or more substances that has
uniform composition and properties throughout.
A _______________________ mixture is a combination of two or more substances that does not
have uniform composition and properties throughout.
Classify the following as element, compound, homogeneous mixture or heterogeneous mixture.
Copper ____________________________
Milk ______________________________
Nitrogen ___________________________
Water _____________________________
Orange juice with pulp ____________________________________
The density of a liquid equals the mass/volume or D = m/V. Solving for mass, m =
__________and solving for volume, V = __________________. Density remains the
__________ when the quantity of a substance changes and its units are _____________.
Precision describes how consistent a set of _________________________ are to each other.
Accuracy describes how close a set of measurements are to the accepted __________.
Atomic Structure
What subatomic particles have significant mass? _________________ and ______________.
Where is the majority of the mass of an atom? ______________________.
Atoms of the same element with different mass numbers are known as ________________.
The atomic number equals the number of _________________ in the nucleus.
In neutral atoms, the number of protons equals the number of ______________________.
The atomic mass equals the number of ________________ and __________________.
The charge on an element is equal to the number of _______________ minus the number of
_____________________.
The average atomic mass is the sum of all of the masses of the different _______________of the
element multiplied by their percent abundance. This causes atomic masses reported in the
periodic table not to be _________ numbers.
Ions are atoms that have an unequal number of __________________ and _________________.
Ions that are negative have _________ electrons than protons and are called ________________.
Ions that are positive have _________ protons than electrons and are called ________________.
In the following, 41Ca2+
What is the charge? __________
What is the mass number? __________
How many protons? __________
How many neutrons? __________
How many electrons? __________
In the following, 33P3What is the charge? __________
What is the mass number? __________
How many protons? __________
How many neutrons? __________
How many electrons? __________
Electron Configuration
The s orbitals are shaped like a _________________.
The p orbitals are shaped like a _____________________.
Most of the d orbitals are shaped like a double ______________________.
When n =1, the total number of electrons can be ______.
When n =2, the total number of electrons can be ______.
When n= 3, the total number of electrons can be ______.
What does “n” stand for? ________________ _________________.
What is the complete electron configuration for:
Ca ___________________________________________________
P…___________________________________________________
Cu ___________________________________________________
What is the abbreviated (noble gas) configuration for:
Ga ___________________________________________
Na ___________________________________________
Pb ___________________________________________
How many orbitals are available for each of the following:
s? __________
p? __________
d? __________
f? ___________
Each individual orbital can hold _____ electrons.
How many electrons can each of the following sublevels hold:
s? __________
p? __________
d? __________
f? ___________
Each arrow in an orbital diagram represents an __________________.
The direction of the arrow indicates the _________________.
When drawing orbital diagrams, electrons fill orbitals with the ______________ energy first.
For example, 2s is filled before 2p.
When drawing orbital diagrams, electrons fill subshells with multiple orbitals with _____
electron in each orbital spinning in the ________ direction before adding a second
_____________ to the orbital.
When drawing orbital diagrams, no two electrons in the same orbital can have the same
__________.
Please draw orbital diagrams for the following:
Cr
Si
Periodic Table
What is a vertical column in the Periodic Table called? ________________
What is a horizontal row in the Periodic Table called? _________________
The metals are to the _________ of the staircase on the Periodic Table.
What are four properties of all metals?
____________________________
____________________________
____________________________
____________________________
What is the charge of all metal ions (positive or negative)? ___________________
The nonmetals are to the ___________ of the staircase on the Periodic Table. Several nonmetals
are gases.
What are four properties of nonmetals?
____________________________
____________________________
____________________________
____________________________
What is the charge of all nonmetal ions (positive or negative)? ___________________
How many valence electrons do elements in the following groups have?
Group 1? _______
Group 2? _______
Group 13? _______
Group 14? _______
Group 15? _______
Group 16? _______
Group 17? _______
Group 18? _______
What is the charge (number and sign) for ions from each of the following?
Group 1? ________
Group 2? ________
Group 13 metals? ________
Group 15 nonmetals? ________
Group 16 nonmetals? ________
Group 17 nonmetals? ________
What is the name for each of the following sections of the Periodic Table?
Group 1? ________________________________
Group 2? ________________________________
Group 17? _______________________________
Group 18? _______________________________
The noble gases are known to be stable or _______________________.
The metalloids are found along the staircase of the Periodic Table and are also called
_______________________________ or semimetals.
What is the oxidation number (charge) of sodium in NaCl? _________
Periodic Trends
The number of energy levels of a neutral atom is the same as its ___________________.
Moving down a group on the Periodic Table, the atomic radius (size) ____________________.
This is because higher energy orbitals are being added which are _____________ from the
nucleus.
Moving across a period on the Periodic Table, the atomic radius (size) ___________________.
This is because the increase in number of protons creates a stronger pull on the
_______________ electrons.
As atomic radius increases, does the force to remove an electron become higher or lower?
__________________. This happens because electrons that are _______________ from the
nucleus are _________________ to remove. What is the term for the force to remove an
electron? _________________________ ________________.
As atomic radius increases, does the ability of an atom to pull electrons towards itself become
higher or lower? _______________. This happens because electrons that are ____________
from the nucleus are _______________ to remove. What is the term for an atom’s ability to
attract electrons towards itself? __________________________________.
Which of the following has a higher electronegativity?
Rb or Na? _____________
N or P? _______________
S or Cl? _______________
F or K? _______________
Which of the following has a higher ionization energy?
Mg or Ba? _____________
O or S? _______________
Br or Cl? ______________
Fr or F? _______________
In the reactivity lab, Ca was more reactive than Mg because as you go down a group in the
Periodic Table it becomes ___________ for a metal to ________ its valence electrons.
Bonding
Describe the electron sharing (equal, unequal or none) for the following:
Ionic Bonds ____________________
Polar Covalent Bonds _________________
Nonpolar Covalent Bonds __________________
To determine the amount of electron sharing, you determine the electronegativity
___________________ between the two atoms.
If the two atoms have the same _________________________, the difference will be _______
and they will have ____________ sharing of electrons and it will be a __________________
covalent bond.