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Periodic Table Review Flashcards | StudBud
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Periodic Table Review
Periodic Table Review
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#O'Hair Review of the #Periodic #trends and basic information about the #Periodic #Table.
Flashcards
33 cards
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Practice quiz
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Questions
33
Answers
1
Which trends increase moving left to right?
Nuclear charge
Ionization energy
Electronegativity
Shielding
2
This atomic property is the ability to steal electrons from another atom
Ionization energy
Huh? What?
Atomic radius
Electronegativity
3
The ________ are a group of colorless, odorless gases that are extremely unreactive
Inert gases
Halogens
Lanthanides
Alkali metals
4
How do I find the number of protons in an atom?
Subtract atomic number from atomic mass
Subtract atomic mass from atomic number
It is equal to the number of protons
Its equal to the atomic number
5
This atomic property is the interference from electrons between the nucleus and valence shell
Ionization energy
Shielding
Blocking
Electronegativity
6
The
d
-block is known as:
Transition Metals
Rare Earth Metals
Lanthanide Series
Alkaline Earth Metals
7
Noble gases are generally unreactive because:
They have no valence electrons
Most of them have eight valence electrons
They are too snooty
Their number of protons equals the number of electrons
8
What makes
d
-block and
f
-block elements so difficult to tell apart?
They all react with main group elements
They are all radioactive
They all have the same valence shell configuration
They all have the same number of neutrons
9
Helium is the only reactive noble gas because it does not have eight valence electrons
True
Cheetos
Wait... this isn't American History class?!?!
False
10
Name the halogen in period 4.
Calcium (Ca)
Strontium (Sr)
Bromine (Br)
Iodine (I)
11
This atomic property refers to an atom's ability to hold onto its own valence electrons
Ionization energy
Conductivity
Electronegativity
Atomic radius
12
When placed in water, which of the following would react violently (explode)?
Promethium (61Pm)
Lithium (3Li)
Neon (10Ne)
Scandium (21Sc)
13
What does an atom use to overcome another's ionization energy?
Ionization energy cannot be overcome
Electonegativity
Conductivity
Shielding
14
What is an isotope?
An atom with a different number of electrons
An atom with a different number of neutrons
An atom with a different number of protons
An atom with a different number of photons
15
How do I find the number of neutrons in an atom?
Subtract atomic number from atomic mass
Its equal to the atomic number
Subtract atomic mass from atomic number
It is equal to the number of protons
16
The electron configuration of this element is 1s
2
2s
2
2p
6
3s
2
3p
4
Phosphorus (P)
Sulphur (S)
Selenium (Se)
Chlorine (Cl)
17
Atoms form compounds and chemical reactions all occur because elements want:
To divide up their energy
To lower their tau values
To share protons
A full valence shell
18
Group 1A is known as:
Alkali Metals
Rare Earth Metals
Alkaline Earth Metals
Halogens
19
This term is used to describe the ability to pull a metal into a wire:
Malleable
Conductivity
Luster
Ductile
20
How do I find the number of electrons in an atom?
It is equal to the number of protons
Subtract atomic number from atomic mass
Subtract atomic mass from atomic number
Its equal to the atomic mass
21
If I change the number of electrons, I have made a(n):
Isotope
Different element
Abomination
Ion
22
Which element is larger (has the bigger radius)?
Francium (87Fr)
Fluorine (9F)
Sulphur (16S)
Molybdenum (42M)
23
The "octet rule" says:
All elements want eight shells of electrons
All elements want a full valence shell
All elements want eight valence electrons
All elements want to be in bed by 8pm
24
These two properties of atoms drive all of the periodic trends.
Nuclear charge and electron configuration
Shielding and atomic number
Atomic mass and atomic number
Shielding and nuclear charge
25
What property do we use to tell one atom from another?
Group number
Number of protons
Number of electrons
Number of neutrons
26
This atomic property is the amount of attractive power of the positive charges
Electronegativity
Nuclear charge
Shielding
Ionization energy
27
Most of the elements surrounding the "staircase" are called:
Nonmetals
Metalloids
Metals
Metallic nonmetals
28
Which of the following properties does NOT describe a nonmetal?
Nonconductive
Powdery
Brittle
Shiny
29
The Rare Earth Metals are generally man-made and:
Unreactive
Radioactive
Stable
Have full valence shells
30
The electron configuration of this element is [Kr] 5s
2
4d
3
Vanadium (23V)
Phosphorus (15P)
Niobium (41Nb)
Arsenic (33As)
31
Name one of two things that give an atom mass?
Electrons
Neutrons
Photons
Protons
32
Electronegativity increases moving right and up because:
Shielding is increasing; nuclear charge is decreasing
Nuclear charge and shielding are both increasing
Shielding is decreasing; nuclear charge is staying the same
Nuclear charge is increasing; shielding is decreasing
33
Elements in a group have similar properties because they all have:
A full octet
The same number of valence electrons
The same number of protons
The same last name
