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chemistry > PT trends > Flashcards

PT trends Flashcards

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1
Q

PERIOD

A

horizontal row

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2
Q

GROUP

A

vertical column

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3
Q

PERIODIC LAW:

A

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

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4
Q

Alkali Metals:

A

elements in the 1st column (except H)

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5
Q

Alkaline Earth Metals:

A

elements in the 2nd

column

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6
Q

Halogens:

A

elements in the column headed by Flourine

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7
Q

Noble Gases:

A

elements in the column headed by He

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8
Q

Lanthanides:

A

elements in the row starting with

Lanthanium

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9
Q

Actinides:

A

elements in the row starting with actinum

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10
Q

The Properties of Metals:

A

• 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

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11
Q

The Properties of Non‐metals:

A

• 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

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12
Q

The Properties of Metalloids:

A

• They have properties which resemble metals more

than non‐metals

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13
Q

The important difference between metals and

metalloids:

A

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

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14
Q

Metallic Properties: Left to right across the table & reason

A

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

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15
Q

Metallic Properties: Down a family

A

• Down a family ‡ metallic properties increase

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16
Q

Describe Atomic Radius in terms of attraction

A

• 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

17
Q

Atomic Radius: Down a family & reason

A

• 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

18
Q

Atomic Radius: Left to right across the table & reason

A

• 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

19
Q

What is Electrical conductivity dependent on? What is electricity?

A

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

20
Q

The better an atom holds on to its e‐:

A

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

21
Q

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

A

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

22
Q

Electrical conductivity: Increased charge=

A

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

23
Q

Electrical conductivity: Decreased distance of orbitals=

A

increased force of attraction

24
Q

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

A

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

25
Q

Electrical conductivity: Left to right across the PT & reason

A

• 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)

26
Q

Electrical conductivity: Down a family on the PT & reason

A

• 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)

27
Q

Relationship between conductivity and

atomic radius:

A

‐ Large radius ‡ increased conductivity

‐ Small radius‡decreased conductivity

28
Q

Relationship between conductivity and

metallic characteristics:

A

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

29
Q

Ionization energy: define

A

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

30
Q

Ionization energy: Smaller atomic radius =

A

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

31
Q

Ionization energy: Larger atomic radius =

A

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

32
Q

Ionization energy: Left to right across the PT & reason

A

• 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‐

33
Q

Ionization energy: Down a family on the PT & reason

A

• 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

34
Q

Electronegativity: define

A

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

35
Q

Electronegativity: Big radius =

A

smaller attractive power of the

nucleus = smaller electronegativity

36
Q

Electronegativity: Left to right across the PT & reason

A

• 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

37
Q

Electronegativity: Down a family on the PT & reason

A

• 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‐

38
Q

Do noble gases have the ability to bond with other

atoms?

A

No

39
Q

Do noble gases have electronegativity? Why?

A

No, they don’t bond with other atoms

chemistry (16 decks)

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