Organization of the PT
History of PT/Bohr Models
Electron Configuration
Periodic Trends
6 7
100
Which element is a metal?
a. Sulfur
b. Oxygen
c. Sodium
d. Iodine
Sodium (Na)
100
Who created the first Periodic Table by arranging elements based on increasing atomic mass/weight
Dmitri Mendeleev
100
The electron configuration 1s²2s²2p⁶3s²3p⁵ represents which element?
a. Argon (Ar)
b. Neon (Ne)
c. Chlorine (Cl)
d. Sulfur (S)
Chlorine (Cl)
100
what is ionization energy?
the amount of energy required to pull 1 or more valence electron away
100
Which element is in the 6th period and have 7 valence electrons?
Astatine (At)
200
Which element is not a metalloid?
a. boron
b. gallium
c. arsenic
d. germanium
b. gallium
200
Which scientist arranged the elements in order of increasing atomic number
Henry Moseley
200
What is the electron configuration for carbon?
1s²2s²2p2
200
Which element has the larger electronegativity?
Oxygen (O) or Astatine (At)
Oxygen (O)
200
Which elements are located at position 3d6 and 3d7
Iron (Fe) and Cobalt (Co)
300
Name an element that is in the Halogen family
Fluorine , Chlorine , Bromine, Iodine, Astatine
300
What is the name of the scientist who organized elements based on chemical properties
Johann Dobereiner
300
The abbreviated electron configuration for Iron (Fe) is:
a. [Ne]3s²3p⁶4s²
b. [Ar]4s²3d⁶
c. [Ar]4s²3d¹⁰
d. [Kr]5s²4d⁶
b. [Ar]4s²3d⁶
300
Rank the following elements from least to greatest atomic radius
Lithium (Li), Calcium (Ca), Iron (Fe), Iodine (I)
Li, Ca, Fe, I
300
elements with 6 or 7 valence electrons generally have ___________ (more, less or the same) electronegativity as elements with 1 or 2 valence electrons?
more! (closer to noble gases with 8ve)
400
Which group of metals is the most reactive?
Alkali metals
400
Draw the Bohr Model of Aluminum include the number of protons and neutrons
400
The abbreviated electron configuration [Ne]3s²3p³ represents which element
a. Nitrogen (N)
b. Silicon (Si)
c. Phosphorus (P)
d. Sulfur (S)
c. Phosphorous (P)
400
In a COMPLETE sentence explain why Krypton (Kr) has a smaller atomic radius than Potassium (K)
H: Kr has more protons which increases the nuclear pull
S: Kr is further to the right across the row/period
400
The 6th and 7th periods of the periodic table are unique because:
A. They contain only transition metals
B. They include the lanthanides and actinides
C. They have exactly 6 and 7 elements
D. They contain no metalloids
B. They include the lanthanides and actinides
500
Identify a metal, nonmetal and metalloid
answers will vary
500
Draw the Bohr Model for Silicon include the number of protons, neutrons and valence electrons
4 valence electrons 
500
What is the FULL electron configuration for Indium (In) atomic number 49
1s22s22p63s23p64s23d104p65s24d105p1
500
Why does Nitrogen have a greater electronegativity than silicon?
H: Nitrogen is smaller, has more protons/strong nuclear pull as well as 5ve which is closer to 8ve than Silicon
S: Nitrogen is further up in the group and over in the row
N has 5ve Si has 4ve
500
Carbon (atomic number 6) and nitrogen (atomic number 7) demonstrate which periodic trend?
A. Nitrogen has a lower electronegativity than carbon
B. Carbon has a larger atomic radius than nitrogen
C. Carbon has a higher ionization energy than nitrogen
D. Nitrogen has a lower ionization energy than carbon
B. Carbon has a larger atomic radius than nitrogen