Atoms and Elements, Physical Science

Atoms and Elements

I. Chemistry: Lecture 4 | 30:12 min

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Atoms and Elements

An atom is the smallest particle of any element, which is a pure form of matter.
Atoms can be broken down into subatomic particles: protons, neutrons, and electrons
An atom is made up of an electron cloud around a nucleus
Electrons constantly moving around the nucleus make up the cloud, protons and neutrons clumped together make up the nucleus
Protons and neutrons are make up of smaller particles called quarks
In a neutral atom, the number of protons = the number of electrons = the number of neutrons.
Electrons in the electron cloud have different amounts of energy. The model of electron configuration places electrons in seven energy levels.
The electrons in energy levels closest to the nucleus have less energy than those electrons in levels further from the nucleus.
Electrons fill the energy levels from the inner levels to the outer levels.
Inner levels are completely filled with 8 electrons before electrons are placed in the next level out. The first level is filled at 2 electrons.
The atomic number gives the number of protons in one atom of the element.
ISOTOPES are atoms of the same element that have different numbers of neutrons.
Isotopes are named with the symbol and the mass number.
MASS NUMBER is the sum of protons and neutrons in an atom.

A solute and a solvent combine to make a (1,0)20.

Solution

What type of mixture is a solution?

A homogeneous mixture.

What do you call a solution when water is the solvent?

An aqueous solution

What can you do to a chunk of rock salt in order for the salt to dissolve faster?

Heat, crush, and/or stir.

Changing the solutes, solvents, temperature or pressure will affect the (1,0)20 of a solution.

Solubility

Which solution has a higher concentration: 2 L of water combined with 20g of salt or 2L of water combined with 40g of salt?

2L of water with 40g of salt

If a substance has a pH of 6, is it an acid, a base, or neutral?

The substance is a weak acid

What is formed in the chemical reaction between an acid and a base?

Salt and water

Why does water make an excellent solvent?

The slight charges that exist in polar molecules of water help to attract tiny pieces of the solute and allow them to break off from the solute faster (dissolves faster)

Liquid mercury is dissolved by solid sodium to form a solution. Identify the solute and the solvent.

Mercury is the solute and sodium is the solvent.

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Answer

Atoms and Elements

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I. Chemistry
	Properties of Matter	30:50
	Energy	53:22
	Heat and States of Matter	48:48
	Atoms and Elements	30:12
	Periodic Table	47:23
	Chemical Bonding, Part I	51:06
	Chemical Bonding, Part 2	56:22
	Chemical Reactions	49:13
	Solutions, Acids, and Bases	29:00
II. Physics
	Waves	42:35
	Motion	37:21
	Forces	35:03
	Density & Buoyancy	23:43

Chemistry: Physical Science

I. Chemistry
	Properties of Matter			30:50
		Intro		0:00
		Matter		0:07
			Matter	0:08
			Substance, Element, and Compound	0:47
			Homogeneous and Heterogeneous Mixture	1:47
			Suspension, Colloid, and Solution	3:16
		Physical Properties		5:25
			Appearance: Color, Shape, Size, Density, and State of Matter	5:26
			Behavior: Viscosity, Magnetism, Malleability, and Ductility	8:00
		Physical Changes		10:29
			Physical Changes	10:30
		Chemical Properties		14:38
			Chemical Properties	14:39
		Chemical Changes		16:35
			Chemical Changes	16:36
			Signs of Chemical Change	16:55
		Example 1: Identify the Mixtures Listed		19:21
		Example 2: Physical or Chemical Change?		23:38
		Example 3: How Can You Separate a Mixture of Sand, Gravel, Iron, Filings, Salt, and Water?		25:04
		Example 4: Physical/Chemical Property and Change		27:27
	Energy			53:22
		Intro		0:00
		Energy		0:03
			Energy Overview	0:04
		Potential Energy		1:48
			Potential Energy	1:49
			Mechanical (Elastic) Potential Energy	1:54
			Chemical Potential Energy	3:15
			Nuclear Energy	4:06
			Gravitational Potential Energy	4:43
		Kinetic Energy		7:34
			Kinetic Energy	7:35
			Thermal Energy	8:03
			Radiant Energy	8:57
			Electrical Energy	9:47
			Sound	10:17
			Motion	10:54
			Kinetic Energy: Example	11:31
		Law of Conservation of Energy		12:47
			Law of Conservation of Energy	12:48
			Electrical to Radiant	13:21
			Chemical to Thermal	14:34
			Potential to Kinetic	15:10
			Friction	18:48
		Energy Resources		20:06
			Nonrenewable: Fossil Fuels	20:51
			Nonrenewable: Nuclear	21:56
			Renewable: Solar	26:50
			Renewable: Wind	29:22
			Renewable: Tidal	31:10
			Renewable: Hydroelectric	32:30
			Renewable: Geothermal	35:24
		Example 1: Gravitational Potential Energy		38:40
		Example 2: Kinetic Energy		42:20
		Example 3: Maximum and Minimum Potential and Kinetic Energy		44:48
		Example 4: Should We Use Renewable or Nonrenewable Resources to Generate Electricity?		46:31
	Heat and States of Matter			48:48
		Intro		0:00
		Temperature		0:04
			Temperature	0:05
			Fahrenheit to Celsius	2:15
			Celsius to Fahrenheit	4:29
			Kelvins to Celsius and Celsius to Kelvins	5:50
		Thermal Energy		8:06
			Thermal Energy, Kinetic Energy, and Potential Energy	8:07
			Changing Thermal Energy: Temperature	9:11
			Changing Thermal Energy: State of Matter	9:37
			Changing Thermal Energy: Amount of Matter	10:12
		Heat		10:59
			Heat	11:00
			Specific Heat	12:21
		Transfer of Thermal Energy		15:15
			Conduction	15:16
			Convection	16:43
			Radiation	19:57
		States of Matter		20:43
			Solids: Arrangement of Atoms, Shape, Volume, and Molecular Motion	21:35
			Liquids: Arrangement of Atoms, Shape, Volume, and Molecular Motion	23:49
			Gases: Arrangement of Atoms, Shape, Volume, and Molecular Motion	25:33
			Plasma: Arrangement of Atoms, Shape, Volume, and Molecular Motion	27:02
		Changing States of Matter		27:49
			Melting	27:50
			Freezing	28:15
			Vaporization	29:04
			Boiling	29:17
			Condensation	31:21
			Temperature and Time Graph	32:18
		Thermal Expansion		36:19
			Thermal Expansion of Solids	37:16
			Thermal Expansion of Liquids	38:17
			Thermal Expansion of Gases	39:46
		Example 1: Converting Temperatures		40:28
		Example 2: Thermal Energy		43:35
		Example 3: Quick Matching		44:58
		Example 4: Why Does It Feel Cold When You Put Your Hand On the Table?		45:50
		Example 5: Heat Transfer		46:48
		Example 6: Changing States of Matter		47:29
	Atoms and Elements			30:12
		Intro		0:00
		Atoms		0:05
			Atoms	0:06
		Atomic Structure		1:01
			Electron Cloud	1:02
			Nucleus, Protons, and Neutrons	1:43
			Quarks	2:07
		Protons, Neutrons, Electrons		2:40
			Protons, Neutrons, Electrons: Location	2:42
			Protons, Neutrons, Electrons: Electric Charge	3:05
			Examples	4:10
		Electron Configuration		5:32
			Electron Configuration	5:33
		Elements		12:22
			Atomic Number	13:05
			Carbon	13:15
			Oxygen	14:49
			Important Elements for Living Things	16:25
		Isotopes		17:04
			Isotopes	17:05
		Example 1: Atomic Structure and Electrical Charge		21:16
		Example 2: Electron Configuration		23:13
		Example 3: Electron Configuration		24:57
		Example 4: Use the Periodic Table to Complete the Table Below		26:08
	Periodic Table			47:23
		Intro		0:00
		Periodic Table		0:06
			Atomic Number, Chemical Symbol, and Atomic Mass	0:07
		Groups and Periods		4:14
			Groups and Periods	4:15
		Electron Dot Diagrams		10:05
			Electron Dot Diagrams	10:06
		Ion Formation		19:09
			An Ion Forms When an Atom Gains or Loses Electrons	19:10
			A Positive Ion Forms When an Atom Loses and Electron	20:25
			A Negative Ion Forms When an Atom Gains an Electron	26:49
		Oxidation Numbers		28:51
			Oxidation Numbers	28:52
		Metals, Nonmetals, Metalloids		34:52
			Metals, Nonmetals, Metalloids	34:53
		Example 1: Group and Period		37:39
		Example 2: Electron Dot Diagrams		39:50
		Example 3: How do Fluorine and Calcium Become Ions?		42:10
		Example 4: What Are 2 Ways to Find the Oxidation Number of Sodium?		44:58
	Chemical Bonding, Part I			51:06
		Intro		0:00
		Chemical Bonds Form Compounds		0:17
			Atoms and Electrons	0:18
			H2O	2:14
			HCl	3:36
			C6H12O6	4:16
			Ca(NO3)2	5:06
			Review: Dot Diagrams	7:10
			Review: Ion Formation	8:30
		Ionic Bond		9:57
			Ionic Bond	9:58
			Sodium and Fluorine	10:41
			Magnesium and Chlorine	16:30
		Covalent Bond		22:19
			Covalent Bond	22:20
			Hydrogen and Carbon	23:58
			Hydrogen and Oxygen	27:28
		Multiple Covalent Bonds		29:03
			Single Covalent Bond	29:04
			Double Covalent Bond	29:40
			Triple Covalent Bond	31:50
		Polar and Nonpolar Molecules		33:33
			Polar Molecules	33:34
			Unequal sharing of Electrons and Electronegativities	35:02
			Nonpolar Molecules	37:46
		Example 1: Elements and Atoms		38:42
		Example 2: Dot Diagram of the Bond That Forms Between Magnesium and Oxygen		41:17
		Example 3: Dot Diagram of the Bond That Forms Between Nitrogen and Oxygen		45:24
		Example 4: Polar or Nonpolar?		47:22
	Chemical Bonding, Part 2			56:22
		Intro		0:00
		Bonding Atoms Make Compounds		0:05
			Binary Compounds	0:06
			Reviwew: Oxidation Number	1:14
		Naming Ionic Compounds		1:45
			Naming Ionic Compounds	1:46
			NaCl	2:26
			MgCl2	5:04
			Al2S3	6:52
		Writing Formulas of Ionic Compounds		10:03
			Writing Formulas of Ionic Compounds	10:04
			Beryllium Fluoride	10:17
			Lithium Nitride	12:24
			Calcium Bromide	13:53
		Polyatomic Ions		15:31
			Polyatomic Ions	15:32
			Ammonium Phosphate	17:21
			Aluminum Hydroxide	19:37
			Magnesium Chlorate	20:54
			NaOH	21:47
			(NH4)2O	22:17
			Mg(NO3)2	22:56
		Special Ions		23:28
			Iron (III) Iodide	24:28
			Lead (IV) Chloride	26:30
			Chromium (III) Oxide	27:31
			Fe3P2	29:18
			CuI2	31:51
			PbBr2	33:04
		Naming Covalent Compounds		33:57
			Naming Covalent Compounds	33:58
			Examples	35:03
		Ionic or Covalent?		39:50
			Ionic vs. Covalent: Electron	39:51
			Ionic vs. Covalent: State At Room Temperature	10:23
			Ionic vs. Covalent: Metal, Nonmetal, Metalloids	41:02
			Ionic vs. Covalent: Naming	41:35
		Example 1: Write the Names or Formulas for Each Ionic Compound		42:50
		Example 2: Write the Names or Formulas for Each Covalent Compound		46:13
		Example 3: Name the Following Ionic Compounds		49:44
		Example 4: Provide the Formulas for the Following Ionic Compounds		52:19
		Example 5: Ionic or Covalent?		54:21
	Chemical Reactions			49:13
		Intro		0:00
		Chemical Reactions		0:05
			Chemical Reactions	0:06
			Chemical Formula Example	0:54
			Reactants and Products	3:50
		Conservation of Mass		4:58
			The Total Mass of the Reactant Must Equal the Total Mass of the Products	4:59
			Balancing Chemical Equations	6:42
		Balancing Equations		11:12
			Example 1: Balancing Equations	11:27
			Example 2: Balancing Equations	14:15
			Example 3: Balancing Equations	16:28
		Types of Reactions		19:17
			Synthesis	19:18
			Decomposition	20:09
			Single-Displacement	20:54
			Double-Displacement	22:12
			Combustion	23:34
		Energy in Chemical Reactions		24:41
			Chemical Reactions and Activation Energy	24:42
			Endergonic Reactions	25:55
			Exergonic Reactions	27:51
		Rate of Chemical Reactions		29:42
			Rate of Chemical Reactions Overview	29:43
			Temperature	30:51
			Concentration	31:26
			Agitation	32:08
			Surface Area	32:29
			Pressure	33:06
			Catalysts and Inhibitors	33:18
		Example 1: Translate Into Chemical Equations		34:32
		Example 2: Law of Conservation of Mass		37:35
		Example 3: Balance the Following Equations		40:33
		Example 4: Math Each Equation With the Correct Type of Reaction		44:58
		Example 5: Exothermic or Endothermic Reaction?		48:21
	Solutions, Acids, and Bases			29:00
		Intro		0:00
		Solutions		0:06
			Definition of Solution	0:07
			Solute and Solvent	0:26
			Example: Salt Water	0:35
			Example: Carbonated Water	1:03
		Dissolving		1:49
			Dissolving	1:50
			Example: Liquid Dissolves a Solid at the Surface of the Solid	3:54
			Aqueous Solutions: Water as Solvent	4:42
		Increasing the Rate of Dissolving		5:33
			Stir	5:34
			Crush	6:37
			Heat	7:36
		Solubility		8:31
			Definition of Solubility	8:32
			Compare the Solubility of Sugar in Water vs. Salt in Water	8:44
			Factors that Affect Solubility	11:45
		Concentration		12:45
			Concentration	12:46
		pH Scale		15:21
			pH Scale: Acids, Neutral, and Bases	15:22
		Acids and Bases		18:01
			Chemical Properties	18:02
			Physical Properties	18:43
			pH Scale	19:31
			Examples of Acids and Bases	19:36
			Acids and Bases React Together to Form Salt and Water	20:09
		Example 1: Identify the Solutes and Solvents for the Following Solutions		21:26
		Example 2: Temperature and the Rate of Dissolving/Solubility of a Solid		23:57
		Example 3: How Can You Make a Solution Have a Higher Concentration?		25:44
		Example 4: Acids and Bases		27:57
II. Physics
	Waves			42:35
		Intro		0:00
		Waves		0:05
			Introduction to Waves	0:06
			Mechanical Waves	1:24
			Electromagnetic Waves	1:50
		Mechanical Waves		2:13
			Transverse	2:14
			Longitudinal (Compressional Waves)	4:00
		Properties of Waves		7:26
			Transverse and Compressional Waves: Wavelength	7:27
			Transverse and Compressional Waves: Frequency (Hz)	9:32
			Transverse and Compressional Waves: Amplitude	11:30
			Wavelength and Frequency are Related	13:40
		Wave Speeds		15:01
			Wave Speeds	15:02
		Behavior of Waves		18:06
			Reflection	18:33
			Refraction	22:42
			Diffraction	24:25
		Electromagnetic Waves		26:00
			Electromagnetic Waves	26:01
		Visible Light		30:49
			Visible Light	30:50
			Opaque	34:25
			Translucent	34:54
			Transparent	35:41
		Example 1: Label the Transverse Wave		36:59
		Example 2: Label the Compressional Wave		38:13
		Example 3: What Happens to the Frequency of a Wave as the Wavelength Increases?		39:12
		Example 4: Law of Reflection and Light Wave		40:48
	Motion			37:21
		Intro		0:00
		Distance vs. Displacement		0:04
			Distance	0:05
			Displacement	0:49
		Speed		4:47
			Speed	4:48
			Instantaneous Speed	6:14
			Average Speed	6:40
			Velocity	7:25
		Distance-Time Graphs		8:21
			Distance-Time Graphs	8:22
		Acceleration		13:38
			Acceleration Definition	13:39
			Acceleration Equation	15:23
			Positive Acceleration	18:43
			Negative Acceleration	18:52
		Speed-Time Graphs		20:56
			Speed-Time Graphs	20:57
		Example 1: Displacement, Distance, and Average Speed		25:15
		Example 2: Velocities		28:02
		Example 3: Acceleration		28:59
		Example 4: Distance and Time		30:19
		Example 5: Speed and Time		34:08
	Forces			35:03
		Intro		0:00
		Force		0:04
			Force Definition	0:05
			Net Force	1:44
			Balanced Forces	3:06
			Unbalanced Forces	4:23
			Forces Examples	5:09
		Friction		7:53
			Friction Definition	7:54
			Static Friction	8:23
			Sliding Friction	9:35
			Rolling Friction	10:11
			Fluid Friction	11:13
			Air Resistance	12:10
		Newton's Laws of Motion		14:06
			First Law of Motion	14:07
			Inertia	15:56
		Newton's Laws Continued		17:13
			Second Law of Motion	17:14
			Third Law of Motion	18:35
		Gravitational Force		24:17
			Gravity and Gravitational Force	24:18
		Example 1: Horizontal Force, Frictional Force, and Net Force		28:36
		Example 2: Net Force and Acceleration		29:38
		Example 3: Gravitational Force		30:35
		Example 4: Force of Air Resistance and Net Force		32:32
	Density & Buoyancy			23:43
		Intro		0:00
		Density		0:05
			Definition of Density	0:06
			Density = Mass / Volume	1:01
		Density of Irregular Objects		3:58
			Density of Irregular Objects	3:59
		Buoyant Force		7:46
			Buoyancy	7:47
			Archimedes' Principle	9:23
		Floating and Sinking		12:47
			Floating and Sinking: Looking at Density	12:48
		Example 1: Density of an Object		16:15
		Example 2: Density of Yourself		17:28
		Example 3: Using Archimedes' Principle to Predict If an Object Will Sink or Float in Water		19:38
		Example 4: Will Aluminum, Gold, and Oil Float or Sink When Placed Into Water?		22:06

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Atoms and Elements

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Features Overview

Atoms and Elements

A solute and a solvent combine to make a (1,0)20.

Solution

What type of mixture is a solution?

A homogeneous mixture.

What do you call a solution when water is the solvent?

An aqueous solution

What can you do to a chunk of rock salt in order for the salt to dissolve faster?

Heat, crush, and/or stir.

Changing the solutes, solvents, temperature or pressure will affect the (1,0)20 of a solution.

Solubility

Which solution has a higher concentration: 2 L of water combined with 20g of salt or 2L of water combined with 40g of salt?

2L of water with 40g of salt

If a substance has a pH of 6, is it an acid, a base, or neutral?

The substance is a weak acid

What is formed in the chemical reaction between an acid and a base?

Salt and water

Why does water make an excellent solvent?

The slight charges that exist in polar molecules of water help to attract tiny pieces of the solute and allow them to break off from the solute faster (dissolves faster)

Liquid mercury is dissolved by solid sodium to form a solution. Identify the solute and the solvent.

Mercury is the solute and sodium is the solvent.

Answer

Atoms and Elements

Chemistry: Physical Science

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