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Chem - Periodic Table Patterns > Chem Test #4 > Flashcards

Chem Test #4 Flashcards

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1
Q

Electronegativity _____ left to right

A

Increases

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2
Q

Z eff (effective nuclear charge) ___________ top to bottom

A

Stays the same

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3
Q

Electron affinity becomes ___________ top to bottom

A

Less negative

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4
Q

Electronegativity __________ top to bottom

A

Decreases

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5
Q

Inner core electrons repelling

A

The valence electrons do not experience the full attraction of the nuclear charge because the inner core electrons reduce the positive nuclear charge (shielding effect)

The electrons in different levels are closer to each other than the nucleus so they repel

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6
Q

Net nuclear charge formula

A

Z eff = Z - S
Z is the atomic number
S is the number of inner core electrons (non valence)

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7
Q

Parent atom vs ion

A

The cation ion will be smaller than the parent ion because it loses electrons and the valence electrons are more strongly attracted to the nucleus
The anion is the opposite

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8
Q

Size of cations across a period

A

When the cations all have the same electron configuration the nuclear charge increases across a row. The increased attraction between the electrons pulls the outer shell closer. So… the atomic radius decreases.

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9
Q

Ionization Energy

A

The minimum amount of energy required to remove an electron from an atom

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10
Q

Ionization Energy

A

The minimum amount of energy required to remove an electron from an atom

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11
Q

IE increases from left to right because….

A

The valence electrons get closer as the Z eff increases so there is a greater force of attraction.

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12
Q

IE decreases from top to bottom because….

A

The Z eff stays the same down a group so the nuclear charge doesn’t affect it.
The atomic radii is larger and makes them easier to remove.

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13
Q

Exceptions to the IE rule

A

Boron and oxygen
Boron: The outer most electron in Boron is further away from the nucleus in the 2p orbital
Oxygen: In an orbital with a second electron and experiences repulsion

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14
Q

Electron affinity

A

The energy change that occurs when an electron is acquired by a neutral gaseous ion
It releases energy and is measured in kJ mol-1
Noble gases do not have ea

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15
Q

Which group has the most negative ea

A

Group 17 because they love to attract electrons

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16
Q

What groups has the max ea value and why

A

Group 2 because the electron is being added to a new orbital
Group 15 because the electron is being added to a orbital with one electron already with repulsion

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17
Q

Electronegativity

A

The relative attraction that an atom has for a shared pair of electrons in a covalent bond

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18
Q

Why the electronegativity increase from left to right and decrease up and down

A

Increase because the Z eff increases and the atom has an increased attraction
Decrease because the radii increases and the bonding electrons are further from the nucleus

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19
Q

Physical properties of alkali metals

A

Good conductors
Low densities
Low melting points
Soft
Melting and boiling points decrease down a group

20
Q

Chemical properties of alkali metals

A

Ionic compounds
Solids
Reactions with water become more vigorous down a group

21
Q

Reactions with water and alkali metals

A

They all produce metal hydroxide and hydrogen gas
Basica solution produced
H20 is the oxidizing agent, metal is reducing one

22
Q

Physical properties of group 17

A

Diatomic molecules
F and Cl are gases, Br is a liquid, I and At are solids
Melting/Boiling points increase down the group

23
Q

Colours of group 17

A

F -pale yellow
Cl - yellow green
Br - red brown
I - purple

24
Q

Chemical properties group 17

A

Very reactive
Reactivity decreases down a group

25
Q

Reaction of halogens with group 1 metals

A

Alkali metals lose one electron (oxidized)
Halogens gain one electron (reduced)
Form an ionic bond

26
Q

Halogens bonding with ionic bond with a metal and a halogen

A

Down the group the oxidizing ability decreases
The smaller (radii) halogen displaces the larger halogen
Takes on the colour of the one that was displaced

27
Q

Determining between I2 and Br2

A

Add hydrocarbon solvent to both solutions, I2 will become purple

28
Q

Period 3 oxides

A

Ionic character of period three oxides decrease from left to right
Become more ionic down a group
Oxides only conduct electricity in the molten state

29
Q

Period 3 oxides basic and acidic

A

Basic - Na2O, MgO
Amphoteric - Al2O3
Acidic - SiO2, P4O10 / P4O6 , SO3 / SO2, Cl2O7 / Cl2O

30
Q

Oxidation state of an element

A

0

31
Q

Oxidation states in an ionic compound

A

Equal to their charges

32
Q

Definition of transition metals

A

An element that forms at least one stable cation with an incomplete 3d sublevel

33
Q

Why there is a small decrease in atomic radii

A

The nuclear charge increases because 1 proton is added but this is offset by the addition of the inner 3d electron

34
Q

Physical properties of transition metals

A

-high electrical and thermal conductivity
-high melting point
-malleable
-high tensile strength
-ductile

35
Q

Delocalized electrons

A

The electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
High conductivity

36
Q

Magnetic properties of transition metals

A

Since they unpairs of spinning electrons, they have magnetic properties

37
Q

Scandium forms a ______ solution

A

Colourless

38
Q

What is a catalyst

A

Substance that speeds up the rate of a chemical reaction

39
Q

Why transition metals have multiple oxidation states

A

Why transition metals have multiple oxidation states

40
Q

Why does the 4d orbital split

A

It is because the ligands with the lone pair of electrons are in between the axises and experience less repulsion from the nucleus, and therefore have more energy

41
Q

Why does these ligand compounds emit colour

A

An electron wants to go from the lower energy level to the higher one, this emits colour

42
Q

Energy gap vs wavelength of light

A

the bigger the gap the smaller the wavelength, more energy in the wavelength, higher frequency in the wavelength

43
Q

Colour absorbed vs emitted

A

Complemntary

44
Q

How charge effects the colour

A

As the metal ion charge increases, the gap energy increases
The energy of the light absorbed increases

45
Q

How indignity of the metal effects the colour

A

More d electrons means higher gap energy

46
Q

How type of ligand effects the colour

A

We replace some of the other ligand with a new one and see what colour is produced
If the colour has a higher energy, the new ligand has a greater splitting ability

Chem - Periodic Table Patterns (3 decks)

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