Electronegativity and Atomic Radius Lecture Notes

Flashcards based on Electronegativity and Atomic Radius Lecture Notes

Atomic Radius

A periodic property related to the size of an atom.

Electronegativity

A periodic property related to the ability of an atom to attract electrons.

Electron Gain Enthalpy

Enthalpy related to the gain of an electron.

Ionization Enthalpy

Enthalpy related to the removal of an electron.

Metallic Character

How metallic something is

Nonmetalic Character

Character of not being metallic

Periodic Properties

The periodic properties discussed included electronegativity, atomic radius, electron gain enthalpy and ionization enthalpy

Effective Nuclear Charge

Across a period, effective nuclear charge generally increases.

Atomic Radius Trend

Across a period, atomic radius generally decreases.

Atomic Radius Trend

Down a group, atomic radius generally increases.

Ionization Enthalpy Trend

Increased nuclear charge leads to increased ionization enthalpy

Stability of configurations

Half filled and fully filled configurations are more stable

Ionization Enthalpy Trend

Ionization enthalpy generally increases across a period.

Ionization Enthalpy Trend

Ionization enthalpy generally decreases down a group.

Electron Gain Enthalpy

The energy change that occurs when an electron is added to a neutral atom in the gaseous phase.

Electron Gain Enthalpy Trend

Electron gain enthalpy becomes more negative across a period.

Electron Gain Enthalpy Trend

Electron gain enthalpy becomes less negative down a group.

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons.

Electronegativity Trend

Electronegativity generally increases across a period.

Electronegativity Trend

Electronegativity generally decreases down a group.

Nonmetallic Character Trend

Nonmetallic character generally increases across a period.

Nonmetallic Character Trend

Nonmetallic character generally decreases down a group.

Metallic Character Trend

Metallic character generally decreases across a period.

Metallic Character Trend

Metallic character generally increases down a group.

Lithium

Lithium has the smallest atomic radius in its group.

Fluorine

Fluorine has the smallest atomic radius in its period.

Cesium

Cesium has the largest atomic radius in its group.

Francium

Francium has the largest atomic radius in its period.

Noble Gases

Noble gases have very positive electron gain enthalpies.

Fluorine

The most electronegative element.

Francium

The most metallic element.

Series I elements

Series I contains Hydrogen and Helium

Series II elements

Series II contains Lithium to Neon

Series III elements

Series III contains Sodium to Argon

Series IV elements

Series IV contains Potassium to Krypton

Groups of Elements

Series of elements with increasing valency and oxides

Group I elements

Group I contains Hydrogen and other metals with a valency of 1

Group II elements

Group II contains Beryllium and other metals with a valency of 2

Group III B elements

Group III B contains Scandium and other transition metals

Group IV B elements

Group IV B contains Titanium and other transition metals

Group V elements

Group V contains Vanadium and other transition metals

Group VI elements

Group VI contains Chromium and other transition metals

Group VII B elements

Group VII B contains Manganese and other transition metals

Group VIII B elements

Group VIII B contains Iron, Cobalt and Nickle as transition metals

Group 0 elements

Noble Gasses are in what group?

Representative elements location

Representative elements tend to occur in Group IA-VIIA

D-Transition elements

Transition metals are referred to as D-Transition elements

F-Inner transition elements

Inner transition elements are referred to as F-Inner transition elements

Representative electron config

Representative elements in Group IIIA have an electron config ending in ns2np1

Representative electron config

Representative elements in Group IVA have an electron config ending in ns2np2

Atomic Radius

A measure of the size of an atom, often expressed in picometers (pm) or angstroms (Å).

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons towards itself.

Ionization Enthalpy

The energy required to remove an electron from a gaseous atom or ion.

Electron Gain Enthalpy

The change in energy when an electron is added to a neutral gaseous atom to form a negative ion.

Metallic Character

The term used to describe elements that exhibit properties characteristic of metals, such as luster, conductivity, and malleability.

Nonmetallic Character

The term used to describe elements lacking metallic properties, typically exhibiting properties such as brittleness and poor conductivity.

Periodic Properties

The properties and trends of elements arranged in the periodic table, including atomic radius, electronegativity, ionization enthalpy, and electron gain enthalpy.

Atomic Radius Trend (Across a Period)

Across a period, atomic radius generally decreases due to increasing nuclear charge.

Atomic Radius Trend (Down a Group)

Down a group, atomic radius generally increases due to increasing electron energy levels.

Ionization Enthalpy Trend (Across a Period)

Across a period, ionization enthalpy generally increases due to increasing nuclear charge and decreasing atomic radius.

Ionization Enthalpy Trend (Down a Group)

Down a group, ionization enthalpy generally decreases due to increasing atomic radius and shielding effect.

Electron Gain Enthalpy Trend (Across a Period)

Across a period, electron gain enthalpy generally becomes more negative (more exothermic) due to increasing nuclear charge.

Electron Gain Enthalpy Trend (Down a Group)

Down a group, electron gain enthalpy generally becomes less negative (less exothermic) due to increasing atomic radius and shielding effect.

Electronegativity Trend (Across a Period)

Across a period, electronegativity generally increases due to increasing nuclear charge and decreasing atomic radius.

Electronegativity Trend (Down a Group)

Down a group, electronegativity generally decreases due to increasing atomic radius and shielding effect.

Metallic and Nonmetallic Character Trends (Across a Period)

Across a period, metallic character generally decreases, while nonmetallic character increases.

Metallic and Nonmetallic Character Trends (Down a Group)

Down a group, metallic character generally increases, while nonmetallic character decreases.

Metals

Elements in this group exhibit properties such as luster, conductivity, and malleability.

Nonmetals

Elements in this group lack metallic properties like luster and conductivity.

Alkali Metal Atomic Radius

Smallest atomic radius: Lithium

Heavy Metal Atomic Radius

Largest atomic radius: Cesium

Electronegativity

Most electronegative element: Fluorine

Trends

Across a period, the general trend is that atomic radius decreases, ionization energy increases, and electronegativity increases.

Trends

Down a group, the general trend is that atomic radius increases, ionization energy decreases, and electronegativity decreases.

Ions

Elements with high ionization energies are less likely to lose electrons and tend to form anions.

Ions

Elements with low ionization energies are more likely to lose electrons and tend to form cations.

Electron Affinity

The energy change that occurs when an electron is added to a neutral atom in the gaseous phase.

High Electronegativity

Elements that readily accept electrons and have a strong tendency to form anions.

Metals

Elements with high metallic character readily lose electrons to form cations.

Reactivity

Down a group, reactivity increases with increasing atomic size.

Reactivity

Across a period, reactivity increases with increasing number of valence electrons.

Group 1A Elements

Representative electron configuration: ns1

Group 2A Elements

Representative electron configuration: ns2

Group 3A Elements

Representative electron configuration: ns2np1

Group 4A Elements

Representative electron configuration: ns2np2

Group 5A Elements

Representative electron configuration: ns2np3

Group 6A Elements

Representative electron configuration: ns2np4

Group 7A Elements

Representative electron configuration: ns2np5

Group 8A Elements

Representative electron configuration: ns2np6

Transition Metals

These elements are characterized by the filling of the d orbitals.

Inner Transition Metals

These elements are characterized by the filling of the f orbitals.

Effective Nuclar Charge

The effective nuclear is the actual nuclear charge experienced by an electron.

Shielding Effect

Shielding effect reduces effective nuclear charge

Effective nuclear charge electronegativity

Higher effective nuclear charge increases electronegativity

Atomic Number

Increased number of protons in nucelus

Effective shielding

Down group effective shielding increases

Period elements

Elements in the same period, same outer shell

Shielding

Increase shielding as you go down

Group II losing electrons

Group II elements lose electrons easily

Ionization Enthalpy

Ionization Enthalpy is required, endothermic