Unit 4: The Periodic Table

The Periodic Table NC Essential Chemistry Standards:

Chm.1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties. Chm.1.2.1 Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds.

Chm.1.3 Understand the physical and chemical properties of atoms based on their position on the Periodic Table.Chm.1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition).Chm.1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table.Chm.1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.

Lesson 1

Periodic Law When elements are arranged in order of ____________________________,

there is a periodic repetition of their _________________ and ________________properties.

Elements can be divided into three categories:

1. _____________ _______ of the staircase

* form ______________ ions (________________)

* have luster, good _________________________, malleable, ductile, most are _________

2. _____________ _________ of the staircase

* form ______________ ions (________________)

* good ____________________, dull, brittle, shatter easily

3. __________________ (semi-metals) either side of the staircase

* ______________________ characteristics

Choose three colors and color/label the PT below based on type of element

Structure

Horizontal rows are called

_____________________

* Each new period adds another energy level for electrons.

Ex. Elements in period ___ have ___ energy level, period 3 ___ energy levels

Vertical columns are called

_______________________

* may be identified by 1-18 as in chart to the right

* may also be identified using group A/B numbers

Groups 1,2,13-18 or A groups include the _________________________________

Above the PT below label the groups and then color the main group elements

Metal =

Metalloid =

Nonmetal =

Alkali Metals (________________)

* ____ valence electron

Complete the dot structure for the following: Li Na K

* The most _______________ metals, therefore usually found in

compounds in nature (rarely ________________________)

* reactivity _______________ as you go down the group

* One valence electron makes them very reactive because

_______________________________________________________________________

* always form cations with a _____________

Hydrogen (________________)

* _____ valence electron, complete the dot diagram……. H

* only __________________ in Group 1A/1

* can lose or gain _____ electron, therefore can be a +1 or a -1 charge

Alkaline Earth Metals (________________)

* ____ valence electrons

Complete the dot structure for the following: Be Mg Ca

* _______________ metals, therefore usually found in

compounds in nature (rarely ________________________)

* reactivity _______________ as you go down the group

* Two valence electron makes them reactive because

______________________________________________________________

* always form cations with a _____________

Boron Family (________________)

* ____ valence electrons

Complete the dot structure for the following: B Al Ga

* All are _____________ except ___________ (metalloid)

* The metals tend to become +3 cations

Metals __________________ to

have a full valence shell, therefore

they always form ________________

ions called _________________.

The size of the cation is always

_______________ than the original

atom because it

_____________________________.

When the number of _____________

changes you have an _______.

Carbon Family (________________)

* ____ valence electrons

Complete the dot structure for the following: C Si Ge

* Combination of __________________, ________________________,

and a __________________________.

Nitrogen Family (________________)

* ____ valence electrons

Complete the dot structure for the following: N P As

* Combination of __________________, ________________________,

and __________________________.

Oxygen Family (________________)

* ____ valence electrons

Complete the dot structure for the following: O S Se

* Six valence electrons means that members of this group are only

______ electrons away from having an ________ in the outer shell.

They ______ 2 electrons to fill the valence shell

* Nonmetal members always

form ____________ with a

____ charge.

Halogens (________________)

* ____ valence electrons

Complete the dot structure for the following: F Cl Br

* Very _______________ nonmetals, therefore usually found in compounds

* reactivity _______________ as you go down the group

* Very reactive because 7 valence electrons means that members of this

group are only _____ electron away from having an ____________ in the

outer shell. They _______ one electron to fill the valence shell.

* Always form _____________ with

a _______ charge

Nonmetals __________________ to

have a full valence shell, therefore

they always form ________________

ions called _________________.

The size of the anion is always

_______________ than the original

atom because it has more electrons

______________________________

______________________________

Noble Gases (________________)

* ____ valence electrons (______ valence shell)

Complete the dot structure for the following: He Ne Ar

* Helium has ___________ energy level so it is full at ____ electrons

* DO NOT form _______

* most are ____________________________

Complete on the PT below: 1. Color each A group with a different color 2. Provide a key that identifies the name for each A group

Groups 3-12 or B groups include the _______________________________________

Above the PT below label the groups and then color the transition elements

Transition Metals (_____________________)

* most ___________________ metals

* many of these metals can have _____________________ ion charges

Ex. Iron _______________________, Copper ___________________________

* AKA _____________________

Inner transition Metals

* many are ______________________

* ______________ elements

* actinide series includes _______________ and plutonium

* AKA ______________________________

Color code and label the inner transition metals on the PT below

Lesson 2 – PT Trends

Periodic Trends Specific patterns that are present in the periodic table (mostly

____________________) related to certain properties

1. Atomic radius/________________/_______________ LABEL chart below!

* It is all about the _________

of the atom NOT the _______

* Atoms get larger going _______

because each ____________ down

adds _____ energy level (n)

* Atoms get smaller going across a

period because more ____________

pull the ____________ closer to the nucleus

Practice

* Which is the largest atom? F, Br, or At

* Which is the smallest atom? K, Cu or Kr

* Order the atoms from the largest to the smallest. Br, Ca, Ge

* Order the atoms from the largest to the smallest. Ba, C, K

2. Electronegativity

* Ability to ____________ electrons in a chemical bond

* Most electronegative ____

Least electronegative ____

* Noble gases have __________

electronegativity because they

have ____________________

* The more _____________ an element has in its valence shell the ________________ the

electronegativity. RESULT EN ____________________________________________

* As you move down ______________, valence electrons get further away from the positive

nucleus (bigger atoms). RESULT EN _______________________________________

Practice

* Which atom is the most electronegative? F, Br, or At

* Which atom is the least electronegative? K, Cu, or As

* Order the atoms from most to least electronegative. Ca, Br, Ge

* Order the atoms from most to least electronegative. N, Bi, As

3. Ionization Energy

* ______________ needed to pull off one

_______________ (make an ion)

* The ___________ the IE, the harder it is

to ____________________________

* Small atoms have a _________ IE because

the ____________ are very close to the positive nucleus

* Atoms with ________ EN have a ________ IE because if it is easy for the atom to grab

electrons it will be __________________________________________________________

Practice

* Which atom has the highest ionization energy? Cl, Br or At

* Which atom has the lowest ionization energy? K, Cu, or Kr

* Order the atoms from highest to lowest ionization energy. Ca, Br, Ge

* Order the atoms from highest to lowest ionization energy. N, Bi, As

4. Metallic Character

* The more likely an atom is

to ________ an electron,

the ______________ the

metallic character

* The ______________ the

valence shell is from the

nucleus the easier it is to lose an electron so metallic character _______________

* As electronegativity or ionization energy ____________, metallic character ____________