Atoms and the Periodic Table

The Electron Configuration: Exceptions (Simplified)

The Electron Configuration: Exceptions (Simplified) Concept 2

The Electron Configuration: Exceptions (Simplified) Example 1

When electron configuration ends with d4, an s orbital electron is promoted to d orbital to create half filled orbital:d5.

Ag has 2 more d electrons and the same number of s electrons as Pd.

Ag has 1 more d electron and the same number of s electrons as Pd.

Ag has 2 more d electrons and 1 less s electron than Pd.

Ag has 1 more d electron and 1 less s electron than Pd.

Ag has 1 more d electron and 1 more s electron than Pd.

A comparison of the electron configurations of palladium (Pd) and silver (Ag) indicates that:&nbsp;

The Electron Configuration: Exceptions (Simplified) Concept 1

Which of the following is the correct electron configuration of gold?&nbsp;

Illustrate the exception to the electron configuration of molybdenum.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/acc283c84aa0209b-1608576552494.jpg"class="fr-fic fr-dii">

p and d subshells are most stable when either half filled or totally filled with electrons.

The Electron Configuration: Exceptions (Simplified) Concept 4

When electron configuration ends with d9, an s orbital electron is promoted to d orbital to create completely filled orbital:d10.

The Electron Configuration: Exceptions (Simplified) Concept 3

Learn the toughest concepts covered in your GOB - General, Organic, and Biological Chemistry class with step-by-step video tutorials and practice problems.

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GOB Chemistry

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Matter and Measurements

Ionic Compounds

Molecular Compounds

Classification & Balancing of Chemical Reactions

Chemical Reactions & Quantities

Energy, Rate and Equilibrium

Gases, Liquids and Solids

Solutions

Acids and Bases

Nuclear Chemistry

BONUS: Lab Techniques and Procedures

BONUS: Mathematical Operations and Functions

Clutch Version GOB/Intro

Solubility and Intermolecular Forces

Solubility deals with the dissolving of a solute in a solvent&nbsp;in order to create a solution.

Auto-Ionization

In a Self-Ionization reaction two water molecules react with one another, where one acts an acid and the other as a base.

Lewis Dot Structures: Ions (Simplified)

Lewis Dot Structures of Ions involves losing or gaining valence electrons to draw the most likely structure.

Distillation & Floatation

Distillation&#160;and&#160;Floatation&#160;represent&#160;procedures that can be used to separate components of a mixture.&#160;

Calculate Oxidation Numbers

Calculating Oxidation Numbers is the first pivotal step in understanding redox reactions.&nbsp;

Solubility: Temperature Effect

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. This solution can be classified as saturated, unsaturated or supersaturated.

Valence Shell Electron Pair Repulsion Theory (Simplified)

Using VSEPR Theory, locations of surrounding elements and lone pairs around central element can be determined.

Electromagnetic Spectrum (Simplified)

The Electromagnetic Spectrum is the different forms of radioactive energy that exists in our universe.

Dipole Moment (Simplified)

Dipole arrows are used anytime a molecule possesses a dipole moment, which happens when a molecule is polar.&nbsp;

Measuring Radioactivity

Measuring Radioactivity involves utilizing different conversion factors.&nbsp;

Ionic Bonding

Under Ionic Bonding, a position ion forms a bond with a negative ion.

Electronic Structure

Electronic Structure of the atom is based on the following principles:shell, subshell and orbital.

Intermolecular Forces and Physical Properties

Intermolecular forces influence physical properties.&nbsp; We will look at direct and indirect relationships.

Mass Percent

Mass Percent is the percentage of a particular element within a compound.&nbsp;

Density of Geometric Objects

The Density of geometric objects generally includes spheres, cubes and cylinders.&nbsp;

Mole Concept

The Mole Concept involves the interconversions between different unit amounts of a substance.

Boiling Point Elevation

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Ka and Kb

Associated with any weak acid or weak base is a Ka or Kb value respectively.

Intensive vs. Extensive Properties

Intensive Properties are independent and Extensive Properties are dependent on the size or amount of substance present

Le Chatelier's Principle

Le Chatelier's Principle&nbsp;explains what happens to a system at equilibrium when it is disturbed.&nbsp;

Ionic Salts (Simplified)

When an acid and base undergo a neutralization reaction they form ions, which can create acidic, basic or neutral solutions.

Endothermic & Exothermic Reactions

Endothermic and Exothermic Reactions involve the absorbing and releasing of thermal energy respectively.&nbsp;&nbsp;

Bohr Model (Simplified)

In the Bohr Model, electrons can move up and down to different orbitals or shells based on absorbing or releasing of energy.

Law of Conservation of Mass

"In a chemical reaction, no matter is created or destroyed, but instead changes form."

Solutions: Mass Percent

Mass Percent can be examined as the percentage of solute found within a given amount of solution. &nbsp;

Gas Evolution Equations (Simplified)

A Gas Evolution Equation is a molecular equation that involves the creation of specific gases.&nbsp;

Molecular Formula

The&nbsp;molecular formula gives the actual number of atoms.

Molality

Molality (m)&nbsp;represents the amount of solute dissolved per kilogram of solvent.&nbsp;

Physical & Chemical Changes

A physical change involves a change in the phases of matter, whereas a chemical change involves a change in chemical bonds.&nbsp;

Ions (Simplified)

Ions represent elements that possess either a positive charge or a negative charge.

Periodic Table: Element Symbols

The Element Symbols of the Periodic Table represent the abbreviated form of an element.

Types of Chemical Reactions

Types of Chemical Reactions are classified by the products that they form.&nbsp;

Dilutions

In Dilutions, a solvent (usually water) is added to a concentrated solution.&nbsp;

Resonance Structures (Simplified)

Resonance Structures are used to represent the different possible bonding arrangements of a molecule.

Percent Yield

The Percent Yield determines how successful the product yield is in a chemical reaction.&nbsp;

Periodic Table: Group Names

The Periodic Table can be further classified into Periods and Groups.&nbsp;

What is Chemistry?

Chemistry is the science that deals with the composition, structural arrangement and properties of substances.

Periodic Trend: Ionic Radius (Simplified)

Ionic Radius is the distance between an ion's nucleus and its most outer occupied electron shell.

Balancing Redox Reactions: Basic Solutions

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.

Metric Prefixes

Metric Prefixes are “labels” that can be placed in front of base units.&nbsp;

Alpha Decay

An alpha decay or alpha emission occurs when an unstable nucleus ejects an alpha particle to create a new element.

Gas Stoichiometry

Gas Stoichiometry involves chemical reactions that contain gases.

Electrolytes (Simplified)

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.

Solution Stoichiometry

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Bronsted Lowry Acid and Base

Types of Radiation

Radioactive reactions deal with the chemical instability of the nucleus in an atom. Heavy (large atomic mass) elements undergo radioactive reactions in order to increase the stability of their nuclei.&nbsp;

Ions and the Octet Rule (Simplified)

The Octet Rule states that main-group elements will generally form enough bonds to obtain 8 electrons in their valence shell.

Multiplication and Division Operations

Multiplication and division of values in scientific notation.&#160;

Electronic Structure: Electron Spin

Electron Spin deals with the rotational spin (up or down) of an electron inside an orbital.

Periodic Table: Phases (Simplified)

Under standard conditions of temperature and pressure, the elements can exist as solids, liquids or gases.

Periodic Trend: Ranking Ionic Radii

Ranking Ionic Radii for the elements begins with first counting their total number of electrons.&nbsp;

Law of Definite Proportions

"Different samples of a pure chemical compound always contain the same proportions of elements by mass."

Molecular Models

Molecular Models represent a way to describe the chemical bonds between elements through the use of color-coded balls for elements.

Test for Ions and Gases

Below are the useful tests that can be employed to identify ions and gases within&#160;typical laboratory procedures.&#160;

The Quadratic Formula

The quadratic formula can be used to solve for the variable x when given an algebraic equation in the form of:ax2&#160;+ bx&#160;- c.&#160;

Calculating Molar Mass

Molar Mass is a physical property that represents the mass of a substance divided by the amount of that substance.

Henderson-Hasselbalch Equation

pH of Strong Acids & Bases

Significant Figures: Precision in Measurements

Significant Figures are used to discuss the level of precision in any measurement.&nbsp;

Heating and Cooling Curves

In&nbsp;Heating&nbsp;and&nbsp;Cooling curves we have the representation of the amount of heat absorbed or released during phase changes.&nbsp;

Atomic, Ionic and Molecular Solids

Crystalline solids represent structures with well-organized patterns and shapes. Amorphous solids represent structures that lack an organized pattern or shape.&nbsp;

Density

Density represents the mass of an object or compound within a given volume.&nbsp;

Atomic Mass (Simplified)

The atomic mass of an element can be found on the Periodic Table.

Specific Gravity

&nbsp;From the simplest view, Specific Gravity represents density without the units.&nbsp;

Radioactive Half-Life

Half-Life is the amount of time required for half of a radioisotope to decay.

SI Units (Simplified)

The International System of Units (SI) represents the modern form of the metric system.

The Ideal Gas Law Derivations

The&nbsp;Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables.&nbsp;

Addition and Subtraction Operations

Addition&#160;and&#160;subtraction&#160;of values in scientific notation.&#160;

Ions and the Octet Rule

Periodic Table: Elemental Forms (Simplified)

The elements on the Periodic Table exist in different forms in nature.

Periodic Trend: Ionization Energy (Simplified)

Ionization Energy&nbsp;is the energy required to remove an electron from a gaseous atom or ion.&nbsp;

Intermolecular Forces (Simplified)

Intramolecular Forces are the bonding forces within a molecule. Intermolecular Forces are the attractive forces between 2 molecules.

Spontaneous Reaction

Thermodynamics is the branch of physical science concerned with heat and its transformations to and from other forms of energy.&nbsp;

Osmolarity

Osmolarity (ionic molarity) represents the number of moles of ions per liter of solution.&nbsp;

Periodic Trend: Atomic Radius (Simplified)

The atomic radius of an element is the distance from its nucleus to its outer electron shell.

Power and Root Functions

Logarithmic&#160;and&#160;natural logarithmic functions&#160;of numbers.&#160;

Acid-Base Introduction

Acids are covalent compounds with H+ ion connected to a nonmetal anion or polyatomic ion. Bases&nbsp;are ionic compounds with metal cation connected to OH- anion, although can also be N containing covalent compounds.

Naming Acids

Acids, for the most part, are covalent compounds that begin with a hydrogen.&nbsp;

Complete Ionic Equations

Complete Ionic Equations show aqueous compounds as fully dissociated ions.&nbsp;

Molecular Equations

Molecular Equations show reacting molecules involved in a chemical reaction.&nbsp;

Heat Capacity

Heat Capacity is the amount of heat required to change the temperature of a substance.&nbsp;

GOB Chemistry

The Electron Configuration: Exceptions (Simplified)

Electron Configuration Exceptions

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