Download Name: Midterm Review (Part II) Fill in the blanks (Chapter 6.1 – 6.3

Name: _______________________
Midterm Review (Part II)
Fill in the blanks (Chapter 6.1 – 6.3):
In the periodic table, each row is called a _______________________________ .
Each column in the periodic table is called a ______________________ .
The elements in each period have the same number of_______________________.
Each of the elements in the same group has the same number of _____________________ in their outer
shells. The electrons in the outer shell are called ___________________ electrons. The group number
equals the number of ______________electrons.
Word Bank: cations, borrow, lend, ion, sign, anions, anions, oxidation, positive, negative, inert (nonreactive),atom, shell,8,plus, minus, gain, lose, positive, cations, negative, anions.
Fill in the blanks (Chapter 7.1 – 7.3):
When an atom lends or borrows electrons it becomes an ______________.
An ionic bond forms between a_________ion with a positive charge and a____________ with a negative
charge. An atom with a plus sign ____________electrons. An atom with a minus sign
___________electrons.
The number of electrons an atom can lend or borrow is called its ___________ (or valence). An oxidation
is a number with a ________or__________in front of it.
Na 1+ : A plus sign meant that the atom _______________1 electron and is called ____________
O 2-: A minus sign means that the atom _______________ 2 electrons and is called ___________
A ________ will borrow enough electrons to complete its _______________. A complete outer shell
usually has _______________ electrons.
Metals lend their valence electrons and become _____________ ions or ______________
Nonmetals borrow valence electrons and become ____________ions or ______________
Noble gases ______________ and do not have an oxidation number.
Complete the following table(Chapter 6.1 – 6.3):
Group #
Family Name
1
2
3
4
5
6
7
8
#Valence Electrons
Charge on the ion
What are elements on the left side of the periodic table called (Periodic Table)?
What are elements on the right side of the periodic table called (Periodic Table)?
Label the following as a metal, nonmetals or a metalloid: Silicon (Si), Argon (Ar), Calcium (Ca), Copper
(Cu)
For Page Two (page 161 – 178 in your book)
Elements in the SAME GROUP have (circle correct) similar properties/different properties because of
(circle correct) valence electrons/inner electrons.
Describe the trends in the atomic size of elements within groups? (Increase/Decrease down a group?)
Describe the trends in the atomic size of elements across periods in the periodic table? (Increase/Decrease
across the period?)
Which element has the largest radius? Lithium, Sodium, Rubidium, Cesium
Which of the following elements is the least reactive metal? Lithium, Sodium, Potassium, Rubidium
Describe the trends in the electronegativity of elements within groups? (Increase/Decrease down a group?)
Explain how size of an atom affects electronegativity? Which element has the greatest electronegativity?
Describe the trends in the electronegativity of elements across periods in the periodic table?
(Increase/Decrease across the period?)
Describe the trends in reactivity of metals within groups?
Describe the trends in ionization of elements within groups? (Increase/Decrease down a group?)
Describe the trends in ionization of elements across periods in the periodic table? (Increase/Decrease
across the period?)
Rank the following elements accordingly to increasing ionization energy
Sodium (Na) Aluminum (Al) Calcium (Ca) Fluorine (F)
Which of the following metals is the LEAST reactive? Lithium (Li), Potassium (K), Rubidium (Rb)
In which group in the periodic table are the most reactive metals?
In which group in the periodic table are the most reactive nonmetals?
Describe the trends in reactivity of nonmetals within groups ((Increase/Decrease down a group?)
Is Bromine is more/less reactive than Chlorine?
List three properties of metals:
List three properties of nonmetals:
Name an element with similar properties to Sodium (Na)
Name an element in the same period with Nitrogen (N)
For page three and four use pages 187 – 203 in your book
How many total electrons in the BOHR diagram? ______________
How many valence electrons in the BOHR diagram? ______________
Use the information provided for each element to draw Bohr Model diagrams:
Sulfur – atomic #: 16, # of n: Sodium – atomic #: 11, # of
16
n: 12
Complete the data table below:
Element
Lewis Dot Total #
Structure electrons
# valence
electrons
Metal or Lends or
nonmetal borrow
Ion
# electrons
Symbol &
(lend/borrow)
charge
one
metal
one
Sodium
lends
Na+1
Chlorine
Cl-1
Magnesium
Oxygen
Aluminum
Neon
Bromine
Calcium
(For the questions below look at chapter 7 and chapter 8)
What is octet rule?
Explains why atoms form chemical bonds with other atoms?
How do metals obey the octet rule when reacting to form compounds?
How do nonmetals obey the octet rule when reacting to form ionic compounds?
How do nonmetals obey the octet rule when reacting to form covalent compounds?
How many valence electrons there are in S-2 ion?
S-2 anion has a larger/smaller radius than a neutral Sulfur (S) atom.
A covalent bond is a bond between two (metals/non-metals) ________________________
An ionic bond is a bond between a (metal/non-metal) ________________________ and a (metal/nonmetal) ________________________
List three properties of ionic compounds:
List three properties of covalent compounds:
A bond in which atoms share a pair of electrons is called?
Classify the following bonds as either ionic, polar covalent or nonpolar covalent
1. NaCl
2. Br2
Name the following compounds:
3. HCl
1. N2H4
2. CO2
3. MgO
Write formulas of the following compounds:
1. Sodium Carbonate
2. Calcium Carbonate
3. Aluminum Sulfate
For the following questions use Chapter 8.1 – 8.3
Describe how the bonding electrons are shared in a nonpolar covalent bond.
Describe how the bonding electrons are shared in a polar covalent bond.
Label the more electronegative atom in HF molecule.
Draw the Lewis structures of each atom, draw lines to show the electrons that are shared and determine
the shape of a molecule:
Example 1: Oxygen and 2 hydrogen
Example 2: Carbon and 2 oxygen
What is a coordinate covalent bond?
Count the number of atoms in Cr2(CO3)3
For the following questions use Chapter 10 in your book
Calculate the molar mass of Na2(SO4)
Calculate % mass of Calcium in Ca(OH)2
Chapter 11 – See your chapter packet and you need to be able to;
Balancing chemical reactions
Label Reactants and Products
Balancing Chemical Reactions
Types of Chemical Reactions
Name: _______________________
Midterm Review (Part I)
Fill in the blank:
(mass, volume, density) (p. 89 – 90, 39 – 40)
___________ amount of matter
___________ amount of space an object takes up
____________matter per volume
How many significant figures are in the measurement 811.40 grams?(p. 66 – 72)
How many significant figures are in the measurement 0.003 4 kg?
A train travels at a speed of 30 miles per hour. If 1 mile = 1.6 kilometers, how fast is the train traveling in
kilometers per hour? (p. 80 – 88)
What is the volume of 80.0 g of ether if the density of ether is 0.70 g/mL?
(p. 63 – 65)
Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a
reading of 7.32 g for the mass of the standard. These results imply that the balance that was used is ____.
1. Accurate 2. Accurate and precise
3. Precise
4.neither neither accurate nor precise
.3
Classify the following properties as either physical or chemical properties (p 49 – 50):
1. Dissolve in water
2. Reacts with acid
3. Melts at 200®C
Classify the following changes as either chemical or physical changes (p. 42 – 48):
1. Burning a candle
2. Cutting an apple
3. Melting/Freezing butter 4. Metal is glowing when
it is placed into a flame.
Fill in the blank: (p. 44-48)
(element, compound, mixture)
What is the smallest particle of an element that maintains the properties of the element?
What is the material that cannot be broken down further by chemical means?
How can you separate a mixture of sand and water? (Circle all that apply) (p. 44)
1. Filter
2. Heat with water
3. Add more water
How can you separate a mixture of sugar and water? (Circle all that apply) (p. 44)
1.
Filter
2. Heat with water
3. Add more water
Compounds are elements that are chemically bonded, mixtures are not chemically bonded.
Circle the correct answer below (p. 44 – 47)
How do you separate a mixture: physical methods chemical methods
How do you separate a compound: physical methods chemical methods
(p. 45)
A solution is a mixture that has a uniform composition. The composition of a heterogeneous mixture is not
uniform throughout. Classify the following solutions as either homogenous or heterogeneous mixtures
1. Salt dissolved in water
2. Oil is mixed with water
3. Air
4. Soil
State the law of conservation of mass. What would be the total mass of the products of a reaction in which
10 grams of water decomposes into the elements hydrogen and oxygen? (p. 55)
Label the following parts of the atom:
(p. 104-105)
Word Bank: Neutrons, Electrons, Protons, Nucleus, Orbitals
A. _______________________
B. _______________________
C. _______________________
D. _______________________
E. _______________________
Label the following:
(p. 163-164)
Complete the chart below:
A. Atomic number _______________________
B. Chemical Symbol _______________________
C. Atomic Mass _______________________
D. Element Name _______________________
E. Number of Protons____________________
Fill in the blanks (p. 104):
The smallest particle of an element that retains the properties
of that
element is a(n) ____.
F. Number
of Neutrons___________________
The particles that found in the nucleus of an atom are ___________________________
G. Number of Electrons____________________
The atomic number of an element is the total number of which particles in the nucleus?
The sum of the protons and neutrons in an atom equals the ____.
How many different elements are represented by the nuclei in the table below?
atoms
A
B
C
D
Number of protons
6
6
7
7
Number of neutrons
6
7
7
8
Which of the following sets of symbols represents isotopes of the same element (p. 112 – 113)?
a.
J
J
J
c.
M
M
M
b.
L
L
L
d.
Q
Q
Q
What does the number 84 in the name krypton-84 represent (p. 111)?
Which of the following isotopes has the same number of neutrons as phosphorus-31 (p 112-116)?
Which of the following isotopes has the same number of neutrons as phosphorus-31 (p. 116)?
a.
P
b.
Si
c.
S
d.
Si
Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which
of these two isotopes of chlorine is more abundant?(p. 116)
Consider an element Z that has two naturally occurring isotopes with the following percent abundances:
the isotope with a mass number of 19.0 is 55 % abundant; the isotope with a mass number 21 of is 45%
abundant. What is the average atomic mass for element Z?(p. 116-117)
All atoms of the same element have the same ___________________ p. 110
Isotopes of the same element have different ____________________ p. 112.
In the space provided, write “true” if the sentence is true. Write “false” if the sentence is false.
(p. 110 -118)
_____ 1.
An atom has no mass.
_____ 2.
An electron is the smallest part of an atom.
_____ 3.
All atoms have the same mass.
_____ 4.
All protons have the same mass.
_____ 5.
All atoms of the same element have the same mass.
_____ 6.
An oxygen atom has the same atomic number as a hydrogen atom.
_____ 7.
To find the mass number of an atom, we add the protons and electrons.
_____ 8.
The atomic number of an atom is the number of neutrons it has.
_____ 9.
_____ 10.
______11.
Atoms of the same kind that have different numbers of neutrons are called isotopes.
Atomic number = mass number.
When an iron nail , its mass stays the same.
Complete the chart by filling in the missing information. Assume neutral atoms
(In a neutral atom the number of protons is equal to the number of electrons)(p. 110-113)
Name of
element
Isotope
Symbol
12
C
6
Atomic
Number
Mass
Number
Number of
protons
Number of
Electrons
Number of
Neutrons
Helium-4
30
Gold-197
35
79
16
O
8
207
53
82
127
Fill in the blank:
(isotope, ion, compound, a new element)Look up in glossary
An atom that you add an electron to become ______________
An atom with different number of neutrons is called ______________
An atom that reacts with another forms a _____________________
An atom that has a change in protons become a _______________
When atom is the ground state, what must happen for the atom to be in an excited state? Your notes
What must happen for this atom to return to ground state?p. 142
Would an electron have to absorb or release energy to jump from the second energy level to the third
energy level?p. 142-143
How light is produced (use words: electron, ground state , excited state)(p. 142)
Which types of waves have the longest wavelength and are used to carry signals for radar, TV and
radio?(p. 139)
What is the difference between second and third energy levels in Bohr’s model? The amount of energy
In Bohr’s model, what are maximum number of electron that can be held in the following energy level?
1st____________ 2nd________________ 3rd________________4th ____________________ (p. 132)
How are the orbitals in the electron cloud model different from the electron paths in the Bohr model?(p.
128-129)
A neutral atom has an electron configuration of 1s22s22p1. Determine the identity of the atom(p. 133-134)
A neutral atom has excited electron configuration of 1s22s22p53s2. Determine the identity of the atom(p.
133-134)
What is the electron configuration of potassium (K)?(p. 133-134)
___ ___ ___ ___ ___ ___ ___ ___ ___ ___ __ __ __ __ __
1s
2s
2p
3s
3p
4s
3d
Which of the following “rules” is being violated in each electron configuration below? Explain your
answer for each. Hund’s Rule, Pauli Exclusion Principle, Aufbau Principle (p. 133-135)
1.    __ __
1s
2s
2p
2.      ___  _ _
1s
2s
2p
3s
3.      
1s
2s
2p
3s
3p
  _
3p
4.          ___     
1s
2s
2p
3s
3p
4s
3d
What symbol is used for beta radiation?
(p. 810-815, p. 799-802)
What symbol is used for alpha radiation?
In the space provided, write “true” if the sentence is true. Write “false” if the sentence is false.
1.
Nuclei split during fission and combine during fusion
2.
Fission forms heavier elements
3.
Nuclei gain electrons during fusion and fission
4.
5.
6.
7.
8.
9.
10.
Two nuclei combine during fusion
Gamma ray has no mass
Gamma ray has positive charge
Beta particle has a negative charge
Alpha particle has a positive charge
Fission reaction releases large amounts of energy when nuclei split apart
During radioactive decay identity of nuclei changes.
A radioactive element has a half-life of 20 days. How much of a 100g sample would decay after 80 days?
P.804 – 806)
Carbon 14 has a half-life of 5,730 years. If an original sample was 100g of C14 and it is now 12.5g of C14,
how old is your sample?(p. 804 – 806)