Chemistry Regents
Mr. Markic
Page 1 of 6
Chapter 6 - The Periodic Table
Mendeleev’s Periodic Table
• Mendeleev arranged the elements in his periodic table in order of _________________________
Modern Periodic Table
 elements are arranged in order of __________________________________________________

Groups = _____________ ______ - _______
elements have _________________ properties

Periods = _____________ ______ - _______
____________ to the principal energy level (also known as _________________)
Three ways to classify elements
 Elements can be classified into metals, nonmetals, and semimetals.

Elements can also be classified into _________________ or _________________.
Metals
 Metals are ________ conductors of _________________ and _________________.

They are _________________ and _________________.

Metals can be pounded into thin sheets (______________) and drawn into wires (____________).

Metals do not hold onto their valence electrons very well. They have low ___________________
and therefore form ______________ ions.
Nonmetals
 Nonmetals are ___________ conductors of ______________ and _________________.

Exception: graphite is a good conductor.

Nonmetals are ___________. If you hit them with a hammer, they shatter and turn to powder.

Good examples of nonmetals are _____________, _____________, and all the ___________.

The _______ diatomic molecules are all nonmetals (__________________________________).

Remember that hydrogen is a nonmetal even though it is located on the ________ side of the
table with the metals.

Nonmetals strongly __________ their electrons. They have ________ electronegativity values
and therefore form ______________ ions.
Metalloids (Semimetals)
 These elements have properties that are ____________ those of the ________ and __________.

They are very important for making _________________ and _________________ __________.

Silicon (_____), germanium (_____), and tellurium (_____) are shown.

Different books include polonium (Po) and leave out astatine (At).
Chemistry Regents
Mr. Markic
Page 2 of 6
Reference Table

Trends:
1. Across a period, metallic character →
Why?
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2. Down a group, metallic character →
Why?
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Sample Exercise
Which of these sets of elements have similar physical and chemical properties?
a) Oxygen, nitrogen, carbon, boron
c) Nitrogen, neon, nickel, niobium
b) Strontium, magnesium, calcium, beryllium

Name two elements that have properties similar to those of the element sodium
•
Identify each element as a metal, metalloid, or nonmetal
•
a) Gold
c) Sulfur
b) Silicon
d) Barium
Identify each property below as more characteristic of a metal or nonmetal
a) Gas at room temperature
d) Poor conductor of electric current
b) Brittle
e) Shiny
c) Malleable

In which pair of elements are the chemical properties of the elements most similar?
a) Sodium and chlorine
b) Nitrogen and phosphorus
c) Boron and oxygen
Chemistry Regents
Mr. Markic
Page 3 of 6
Classifying the Elements

Alkali Metals –
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Alkaline Earth Metals –
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Halogens –

Noble Gases –

Representative Elements –

Transition Elements –
Classifying Review
 Which of the following are transition metals?
 Cu
 Au
 Sr
 Al
 Cd
 Ge
 Co
Periodic Trends
1. Trends in Atomic Size
2. Trends in Ionization Energy
3. Trends in Ionic Size
4. Trends in Electronegativity
1. Trends in Atomic Size (Table _____)
Atomic Radius – one _______ of the distance between the nuclei of two atoms of the same element
Group Trends in Atomic Size
From top to bottom the size trends __________________
Why?


Period Trends in Atomic Size
From left to right the size trends _________________
Why?


Chemistry Regents
Mr. Markic
Page 4 of 6
Sample Exercise
• Which element in each pair has atoms with a larger atomic radius?
a) Sodium or lithium
c) Carbon or germanium
b) Strontium or magnesium
d) Selenium or oxygen
Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and
sodium.
Ions
 Form when ____________ are __________________ between atoms

An ion with a ____________ charge (_______ electrons) is called a ____________

An ion with a ____________ charge (____________ electrons) is called an ____________

Ionization Energy - the energy required to ____________ an electron from an atom (table_____)
2. Trends in Ionization Energy
 Found on table ______

The ability to become a ____________ charge
Group Trends in Ionization Energy
• From top to bottom IE __________________ (____________ to take away e-)
Why?


Period Trends in Ionization Energy
 From left to right IE increases (difficult to take away e-)
Why?


Sample Exercise
• Which element in each pair has greater first ionization energy?
a) Lithium or boron
b) Magnesium or strontium
c) Cesium or aluminum
Chemistry Regents
Mr. Markic
•
Page 5 of 6
Arrange the following groups of elements in order of increasing ionization energy.
a) Be, Mg, Sr
b) Bi, Cs, Ba
c) Na, Al, S
3. Trends in Ionic Size
Ion – When an atom __________ or __________ electrons
Cation
• When an atom ________ an electron (becomes ________)
•
Radius becomes __________ than the original atom
Why?
•
Anion
• When an atom ________ an electron (becomes ________)
•
Radius becomes __________ than the original atom
Why?
•
Sample Exercise
Which particle has the larger radius in each atom/ion pair?
a) Na or Na+
c) I or I-
b) S or S2-
d) Al or Al3+
In each pair, which ion is larger?
a) Ca2+ or Mg2+
b) Cl- or P3-
4. Trends in Electronegativity
 The ability of an atom to __________ an _______________
 Found on table ______
Group Trends in Electronegativity
From top to bottom; electronegativity values _______________
c) Cu+ or Cu
Chemistry Regents
Mr. Markic
Page 6 of 6
Why?

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Periodic Trends in Electronegativity
From left to right; electronegativity values _______________
Why?


Sample Exercise
Which element in each pair has a higher electronegativity value?
a) Cl or F
c) Mg or Ne
b) C or N
d) As or Ca
Which element in each pair has a greater attraction for electrons?
a) Ca or O
c) H or O
b) O or F
d) K or S
Periodic Property
Metallic Character
Atomic Radius
Ionization Energy
Ion Size
Electronegativity
Across a Period
Down a Group