Chapter 4- The Periodic Table Flashcards
Who is known as the father of the modern periodic table
Mendeleev
Mendeleev
Published 1st period table in 1869
How did Mendeleev arrange elements
In order of increasing atomic mass and by properties, both physical and Chemical
Moseley
Reorders the elements on the periodic table by atomic number In1911
Group
Vertical
Period
Horizontal
Metal
Located to the left of the zig zag
Nonmetal
Located to the right of the zig zag
Metalloid
Located along the zig zag line
Location of alkali metals
Group 1
Alkali properties
Silvery
Soft
Very reactive
React strong with water
Location of Alkaline earth metal
Group 2
Alkaline earth metal properties
Harder and denser
Higher melting points
Less reactive
Transition metals
D block elements
Why does the D block contain 10 groups
There are 5 d orbitals and each contain 2 electrons
Location of halogen
Group 17
Halogen properties
Most reactive of the nonmetals
Reactive with most levels to form salts
Location of noble gases
Group 18
What is the arrangement of noble gases
Stable
Inner transition metals
Lanthides amd actinides
Groups 6 and 7
How is the periodic law demonstrated within groups of the periodic table
Elements in a group have similar properties
Why are elements not in strict increasing order
They are in order of the atomic number, not the atomic mass
What info is recorded on the periodic table
Atomic number and mass, element name, symbol, and on some you can find the electron configuration
How could you organizes elements according to the trends
Make predictions
How is the periodic table periodic
Properties of the elements occur periodically
Who discovered periodic law
Mendeleev
Who established atomic numbers as the basis for organizing
Mosley
Three sets of elements that has been added since mendeleevs time
Helium, krypton, xenon
Why are electrons important
They find the elements chemically properties
Why do elements in the same group have similar properties
They have similar electron configurations
Into how many blocks is the table divided and what are they called
4 blocks,
S,p,d,f
What does each block represent
The energy level and sub level that is being filled with electrons
Why does the s block span two groups of elements
S orbitals only hold two electrons
Group configuration of each element in group 1
Ns1
Group configuration of each element in group 2
S2
Ending electron configuration of the element in period 3, group 1
3s1
Why does the p block span six groups
3p orbitals hold 6 electrons
Why are there no p block elements in period 1
P orbitals don’t start until the 2nd energy level
Ending electron configuration of each element in group 14
Ns2np2
In what period does the first d energy sublevel appear
Period 4
In what period does the first f energy sublevel appear why
6 because that is where they fall in terms of electrons going in to atoms
Why are members of group 18 unreactive
There is a stable arrangement of electrons
Determine the group, period, and block for the following elements
1s1
[Ne]3s23p1
1s1- s block, group 1, period 1
[Ne]3s2 3p1- p block, group 13, period 3
Describe the relationship between atomic radio and atomic numbers
As atomic number increases the atomic radii decreases
What are the smallest and largest first ionization energies
Smallest- Fr
Largest- He
If an element has a low ionization energy is it easy or hard to remove an electron? Reactive or unreactive?
Easier to remove and will be reactive
What happens to a numeral atom if it loses one electron
It becomes positive
Why do the first two elements in the first period not have ionic radii
Hydrogen- too small
Helium- doesn’t form ions
How can you figure out the charge of an ion
Charge = protons - electrons
