ATOMIC STRUCTURE AND THE PERIODIC

TABLE

Bellwork*Write the answer and a short explanation as to why you chose that answer.

Bellwork Question #1 Why is cobalt (Co) placed before nickel (Ni)

on the periodic table of the elements even though it has a higher average atomic mass than nickel? A. Nickel has one more proton. B. Cobalt was discovered first. C. Nickel has fewer electrons. D. Cobalt has a lower density.

Bellwork Question #2 Which of the following will allow you to

always determine the identity of an element?A. The number of protonsB. The number of electronsC. The number of neutronsD. The atomic mass

Bellwork Question #3 Two elements have the same number of

protons but different numbers of neutrons, these two elements are known as: A. Family MembersB. IsotopesC. Beta ParticlesD. Atomic mass units

Bellwork Question #4 The atomic number of Sodium is 11 and

the atomic mass of Sodium is 23. Which of the following shows how many neutrons sodium has? A. 11B. 12C. 23D. 34

State Standard 1a

Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass.

The Atom

Subatomic Particles

A proton is a positive particle A neutron is a neutral particle An electron is a negative particle The proton and neutron are in the nucleus.

State Standard 1b

b. Students know how to use the periodic table to identify metals, semimetals, non-metals, and halogens.

Types

Elements on the periodic table belong to one of three types metals, nonmetals and semimetals (metalloids)

Metals of the Periodic Table

Non-metals of the periodic table

Semimetals/ Metalloids

Families/Groups

Elements on the periodic table belong to families/Groups.

These families are- Alkali Metals, Alkaline Earth Metals, Transition Metals, Halogens and Noble Gases.

State Standard 1c

c. Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms.

Ionization Energy The energy required to remove one

electron from an atom. Ionization energy increases as you

move to the right and up.

Electronegativity The ability of an element to attract

electrons. Electronegativity increases right and up.

Atomic Radius The size of atoms decreases to the right, and

increases as you move down.

Ions An ion is an element with a charge. Cations (positive ions) are smaller

than anions (negative ions).

Ionic Radius Ionic radius decreases to the right and

increases as you go down.

State Standard 1dd. Students know how to use the periodic table to determine the number of electrons available for bonding.

Number of Electrons Available for Bonding Bonding Electrons AKA Valence Electrons Valence Electrons are the electrons in the

outer orbital.

Valence Electrons

Valence Electrons are the same by group #

State Standard 1e

e. Students know how to draw Lewis dot structures.

Lewis Structure Lewis Structure is the chemical symbol

surrounded by the number of valence electrons.

Quiz

Question 1

How many valence electrons are shown here?

a. 13 b. 8 c. 3 d. 5

Question 2

What family does Chlorine belong to? a. Alkali Metals b. Alkaline Earth Metals c. Transition Metals d. Halogens

Question 3

The largest family on the periodic table is:

a. Alkali Metals b. Alkaline Earth Metals c. Transition Metals d. Halogens

Question 4

Families on the periodic table share the same number of:

a. Protons b. Electrons c. Valence Electrons d. Neutrons

Question 5

A subatomic particle that carries no charge and has a mass nearly equal to that of a proton is a

A. proton. B. neutron. C. electron. D. isotope.

Question 6

Comparing Oxygen, Sulfur, Nitrogen and Phosphorus.

A. Oxygen is the largest ion. B. Sulfur is the largest ion C. Nitrogen is the largest Ion D. Phosphorus is the largest ion.

Question 7

Which of the following atoms has the largest atomic radius?

A barium (Ba) B chlorine (Cl) C iodine (I) D magnesium (Mg)

Question 4

Which of the following elements has Lewis dot structure most similar to silicon?

A. Aluminum B. Gallium C. Germanium D. Arsenic