Ch: 6 Chemistry - Periodic Trends

second ionization energy.

The energy required to remove an electron from an ion with a 1+ charge

ionization energy.

The energy required to remove an electron from an atom

first ionization energy.

The energy required to remove the first electron from an atom

Halogens

The non-metals of Group 7A

Cation

type of ion formed by Group 2A elements

Group

vertical column in the periodic table

Organize the following elements below from lowest EN (1st) to largest EN value (4th) cesium______ calcium______ helium ______ fluorine ______

1st helium 2nd calcium 3rd cesium 4th fluorine

Period

A horizontal row of elements in the periodic table

Explain what is an anion.

A negatively charge ion

Explain what is a cation.

A positively charged ion

Give three examples of a transition metal.

Silver (Ag) Gold (Au) Platinum (Pt)

Give examples of 2 pairs of elements having the most similar chemical and physical properties

Strontium & Magnesium

Organize the following elements below from smallest (1st) to largest radius (4th) sulfur ______ selenium______ chlorine______ bromine______

1. sulfur 2. chlorine 3. selenium 4. bromine

Explain the role electrons play for the atom

An electron from one atom is transferred to another and then you create two ions as one atom loses an electron and one gains one.

Name the group 3a elements.

Boron (B), Aluminum (Al), Gallium (Ga), Indium (In) & Thallium (Ti)

How did chemists begin to organize the known elements?

Chemists used the properties of elements to sort them into groups.

Name the scientist known to have developed the Periodic Table and explain how he arranged the elements.

Dmitri Mendeleev arranged the periodic table by the chemical properties and relative atomic masses of the elements.

Name the 4 blocks elements are found in and the 7 element categories found in these blocks.

Elements are found in the s, p, d, f blocks

How can elements be classified based on their electron configurations?

Elements can be sorted into noble gases, representative elements, transition metals, or inner transition metals based on their electron configurations.

representative elements

Elements in groups 1A through 7A & because they display a wide range of physical and chemical properties.

Metal

Elements that are good conductors of heat and electric current. 80% are metals, high luster, du tile, malleable.

nonmetals

Elements that are poor conductors of heat and electric current. Are gases, solids, & red liquid

What are the trends among the elements for first ionization energy, ionic size, and electronegativity?

First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period. Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from left to right across a period.

alkali metals.

Group 1A elements

Explain how atomic size changes from left to right and top to bottom on the periodic table..

In general, atomic size increases from top to bottom within a group and decreases from left to right across a period.

What are the trends among the elements for atomic size?

In general, atomic size increases from top to bottom within a group and decreases from left to right across a period.

Describe the elements in the modern periodic table were and are currently arranged.

In the modern periodic table, elements are arranged in order of the increasing atomic number and in order of atomic mass

Identify the elements in the third period with the largest and smallest atomic radius.

In the third period the largest is Argon and the smallest and sodium..

For the following trends below, explain if they increase (I) or decrease (D) as you move from left to right across the periodic table. Ionization Energy _______ Electro-Negativity _______ Atomic Radii _______ Atomic Mass _______

Ionization Energy - I Electro-Negativity - I Atomic Radii - D Atomic Mass - I

How do ions form?

Positive and negative ions form when electrons are transferred between atoms.

Name the category of elements considered to be a poor conductor of electricity and give 5 examples.

The nonmetals are a poor conductor of electricity because nonmetal compounds don't have a metallic structure, most nonmetals are gases at room temperature, a few nonmetals are solids, one nonmetal, bromine, is a dark-red liquid and they have no free electrons which help in conducting electricity.

What type of information can be displayed in a periodic table?

The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms.

Describe how the Periodic Table is divided in 3 sections.

The periodic table is divided in to 3 different sections of elements which are metal, nonmetals, & metalloids

Explain what periods in the modern periodic table corresponds to

The properties of the elements within a period change as you move across a period from left to right.The pattern of properties within a period repeats as you move from one period to the next.t

Explain how does atomic radius change from left to right across a period in the periodic table.

The radius increases as you go from top to bottom in the periodic table.

What is the underlying cause of periodic trends?

The trends that exist among these properties can be explained by variations in atomic structure.

Explain how does atomic radius change from top to bottom in a group in the periodic table.

This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.

Electronegativity

ability of an atom to attract electrons when the atom is in a chemically combined compound

ion

an atom or group of atoms that has a positive or negative charge.

Alkaline Earth element

any of the strongly basic metals of group II of the periodic table

metalloid

generally has properties that are similar to those of metals and nonmetals.

atomic radius

one-half the distance between the nuclei of two atoms when the atoms are joined

periodic law

repetition of properties occurs when elements are arranged in order of increasing atomic number

electrons

subatomic particles that are transferred to form positive and negative ions

noble gases

the elements in Group 8A of the periodic table.

ionization energy

the energy required to remove an electron from an atom

transition metal

the highest occupied s sublevel and a nearby d sublevel contain electrons.

inner transition metal

the highest occupied s sublevel and a nearby f sublevel generally contain electrons.