PT trends Flashcards by Stephanie Schneider

PERIOD

horizontal row

How well did you know this?

Not at all

Perfectly

GROUP

vertical column

How well did you know this?

Not at all

Perfectly

PERIODIC LAW:

The properties of the chemical elements recur periodically when the elements are arranged from lowest to highest atomic numbers

How well did you know this?

Not at all

Perfectly

Alkali Metals:

elements in the 1st column (except H)

How well did you know this?

Not at all

Perfectly

Alkaline Earth Metals:

elements in the 2nd

column

How well did you know this?

Not at all

Perfectly

Halogens:

elements in the column headed by Flourine

How well did you know this?

Not at all

Perfectly

Noble Gases:

elements in the column headed by He

How well did you know this?

Not at all

Perfectly

Lanthanides:

elements in the row starting with

Lanthanium

How well did you know this?

Not at all

Perfectly

Actinides:

elements in the row starting with actinum

How well did you know this?

Not at all

Perfectly

The Properties of Metals:

• Reflect light when polished
• Are opaque
• Good conductors of electricity and heat
• Are generally flexible when in thin sheets
• Are generally malleable (can be hammered into thin
sheets) and ductile (drawn or stretched into wires)
• Usually solid at room temp

How well did you know this?

Not at all

Perfectly

The Properties of Non‐metals:

• Are gases, liquids or brittle solids at room temperature
• Are poor heat and electrical conductors
• If solids, are dull to lustrous in appearance and opque to
translucent

How well did you know this?

Not at all

Perfectly

The Properties of Metalloids:

• They have properties which resemble metals more

than non‐metals

How well did you know this?

Not at all

Perfectly

The important difference between metals and

metalloids:

• Metals: Electrical conductivity DECREASES
with INCREASING temperature
• Metalloids: Electrical conductivity
INCREASES with INCREASING temperature

How well did you know this?

Not at all

Perfectly

Metallic Properties: Left to right across the table & reason

• Left to right across the table ‡ metallic properties
decrease
‐ Reason: Moving from the metal side to the non‐metal
side of the PT

How well did you know this?

Not at all

Perfectly

Metallic Properties: Down a family

• Down a family ‡ metallic properties increase

How well did you know this?

Not at all

Perfectly

Describe Atomic Radius in terms of attraction

• Atomic radius is influenced by the force of
attraction between the positive nucleus and the
negative e‐
• This attraction is the ‘glue that holds the atom
together’
• The larger the charges the greater the forces

Atomic Radius: Down a family & reason

• Down a family ‡ atomic radius increases
‐ Reason: As you move down you increase the number of energy levels
• This means that the e‐ are farther away from the
nucleus
• The greater the distance between the p & e‐ ‡
decreased force of attraction
• Therefore the nucleus can’t hold the e‐ close and the
atomic radius increases

Atomic Radius: Left to right across the table & reason

• Left to right across the table ‡ radius decreases
‐ Reason: you are moving along the same energy level but increasing the # of p and #e
• More p & e = more charge ‡ greater force of attraction
between the p and the e‐
• Therefore the nucleus holds the e‐ closer and the
radius decreases in size

What is Electrical conductivity dependent on? What is electricity?

• Electrical conductivity depends on the atom’s ability
to transfer e‐
• Electricity is the movement of e‐

The better an atom holds on to its e‐:

the less its ability of the atom to transfer e‐ = decreased ability to be a conductor

E. conductivity: The worse an atom hangs on to its e‐: (conductor ability)

the greater the ability of the atom to transfer e‐ = increased ability to be a conductor because electricity is the movement of e-

Electrical conductivity: Increased charge=

more p & e‐:
• Increased force of attraction
• Decreased distance of orbitals ‡ increased
force of attraction
• Increased force of attraction between p & e‐
will increase the hold that the nucleus has on
the e‐ and the decrease the ability for the e‐ to
move

Electrical conductivity: Decreased distance of orbitals=

increased force of attraction

What does Increased force of attraction between p & e‐do?

increase the hold that the nucleus has on
the e‐ and the decrease the ability for the e‐ to
move

Electrical conductivity: Left to right across the PT & reason

• Left to right across the PT ‡ conductivity decreases ‐ Reason: The nucleus has a strong hold on the e‐because of the decreased atomic radius • e‐ are less able to move (they are very attracted to the nucleus)

Electrical conductivity: Down a family on the PT & reason

• Down a family on the PT ‡ conductivity increases ‐ Reason: The nucleus has a lesser hold on the e‐ because of the increased atomic radius • e‐ are able to move more freely (more distance between the e‐ and the nucleus)

Relationship between conductivity and | atomic radius:

‐ Large radius ‡ increased conductivity | ‐ Small radius‡decreased conductivity

Relationship between conductivity and | metallic characteristics:

‐ Increased conductivity ‡ increased metallic characteristics ‐ This makes sense because we know that metals are good conductors

Ionization energy: define

energy required to steal an e‐ from an atom • It is based on how well the nucleus can hang onto its own e‐

Ionization energy: Smaller atomic radius =

greater hold that the atom has on its e‐ = greater the ionization energy

Ionization energy: Larger atomic radius =

lesser hold that the atom has on its e‐ = smaller ionization energy

Ionization energy: Left to right across the PT & reason

• Left to right across the PT ‡ ionization energy increases ‐ Reason: The nucleus has a strong hold on the e‐ because of the decreased atomic radius • Can hold onto its own e‐ and can also steal other e‐

Ionization energy: Down a family on the PT & reason

• Down a family on the PT ‡ ionization energy decreases ‐ Reason: The nucleus has a lesser hold on the e‐ because of the increased atomic radius • Cannot hold onto its own e‐ very well therefore won’t be able to steal others’ e‐ either

Electronegativity: define

the ability of a bonded atom to attract shared electrons to itself

Electronegativity: Big radius =

smaller attractive power of the | nucleus = smaller electronegativity

Electronegativity: Left to right across the PT & reason

• Left to right across the PT ‡ electronegativity increases ‐ Reason: The nucleus has a strong hold on the e‐ because of the decreased atomic radius = is able to attract e‐ - Small Radius = Large Attractive Power

Electronegativity: Down a family on the PT & reason

• Down a family on the PT ‡ electronegativity decreases ‐ Reason: The nucleus has a lesser hold on the e‐ because of the increased atomic radius = can’t attract other e‐ - • Down a family on the PT ‡ electronegativity decreases ‐ Reason: The nucleus has a lesser hold on the e‐ because of the increased atomic radius = can’t attract other e‐

Do noble gases have the ability to bond with other | atoms?

Do noble gases have electronegativity? Why?

No, they don't bond with other atoms