Intro to Chemistry, Basic Concepts - Periodic Table, Elements, Metric System & Unit Conversion

The Organic Chemistry Tutor・2 minutes read

The periodic table categorizes elements based on properties like valence electrons and reactivity, essential in understanding chemical bonding and behavior. Learning about different elements, their charges, and reactions aids in predicting and comprehending chemical interactions.

Insights

Alkali metals like sodium and potassium have one valence electron, forming ions with a plus one charge, while alkaline earth metals such as magnesium have two valence electrons, creating ions with a plus two charge.
Transition metals like zinc can have variable charges, with some typically having a plus two charge and others like copper having plus one or plus two charges.
Group 17 elements, the halogens like chlorine, have seven valence electrons, leading to ions with a negative one charge and are highly reactive nonmetals.
Carbon exists in various forms such as diamond and graphite, with diamond being a non-conductor of electricity and graphite being a conductor.
Isotopes like carbon-12 and carbon-13 have the same atomic number but differ in mass number and number of neutrons, impacting the average atomic mass calculation.
Naming compounds involves understanding prefixes for molecular compounds and recognizing monoatomic and polyatomic ions, essential for accurate chemical nomenclature.

Get key ideas from YouTube videos. It’s free

Recent questions

What are the characteristics of alkali metals?
Highly reactive, one valence electron, plus one charge.

Related videos

Summary

00:00

Chemical Elements and Bonding in Summary

The periodic table includes elements like hydrogen, lithium, sodium, potassium, and rubidium in the first column, known as alkali metals, which are highly reactive.
Alkali metals have one valence electron, leading them to form ions with a plus one charge, while alkaline earth metals like beryllium, magnesium, and calcium have two valence electrons, forming ions with a plus two charge.
Transition metals like scandium, titanium, and zinc have variable charges, with some like zinc typically having a plus two charge, while others like copper can be plus one or plus two.
Group 13 elements like boron and aluminum have three valence electrons, tending to form plus three charges, while group 16 elements like oxygen and sulfur have six valence electrons, forming ions with a negative two charge.
Group 17 elements, the halogens, including fluorine and chlorine, have seven valence electrons, forming ions with a negative one charge, and are highly reactive nonmetals.
Noble gases like helium and neon are chemically inert, stable, and do not participate much in chemical reactions, with neon being a non-reactive element.
Metals are found on the lower left side of the periodic table, while nonmetals are on the upper right side, with metalloids like silicon and germanium conducting a small amount of electricity.
Carbon exists in different forms as allotropes, such as diamond and graphite, with diamond being a non-conductor of electricity and graphite being a conductor.
The seven diatomic elements like hydrogen, nitrogen, and oxygen exist as molecules in their natural states, with hydrogen existing as H2 and oxygen as O2.
Ionic bonds involve the transfer of electrons between metals and nonmetals, forming ions that are attracted to each other, while covalent bonds involve the sharing of electrons, with polar covalent bonds having unequal electron sharing between different elements like hydrogen and fluorine.

20:57

Chemical Bonds, Isotopes, and Atomic Mass

A bond is considered polar if the electronegativity difference is greater than or equal to 0.5, otherwise it's nonpolar.
The bond between carbon and nitrogen is nonpolar since the electronegativity difference is 0.4.
Compounds with only carbon and hydrogen atoms are automatically nonpolar.
Ionic compounds result from a metal and a nonmetal combining, while covalent compounds form from two nonmetals.
Magnesium oxide (MgO) is ionic, carbon dioxide (CO2) is covalent, and water (H2O) is covalent.
Lithium chloride (LiCl) is ionic, fluorine (F2) is covalent, and ammonium chloride (NH4Cl) has both ionic and covalent bonds.
The atomic number represents the number of protons in an atom, while the mass number is the sum of protons and neutrons.
Isotopes have the same atomic number but differ in mass number and number of neutrons.
Carbon-12 and carbon-13 are isotopes of carbon with the same number of protons but different numbers of neutrons.
The average atomic mass is calculated using a weighted average based on the abundance of each isotope.

40:21

Atomic Mass, Isotopes, Elements, and Conversion

99 as a decimal is 0.99; to convert percent to a decimal, divide by 100 or move the decimal point two units to the left.
Carbon 13 has a mass of 13 and a percentage of 0.01; multiplying 12 by 0.99 gives 11.88, while multiplying 13 by 0.01 results in 0.13. Adding 0.13 and 11.88 gives 12.01, the average atomic mass of carbon isotopes on Earth.
Boron has an average atomic mass of 10.81 and is element 5 on the periodic table, with two principal isotopes: boron 10 and boron 11.
The average atomic mass equation is average = m1p1 + m2p2; solving for boron's isotopes, 10.81 = 10x + 11(1-x), leading to x = 0.19 or 19% for boron 10 and 81% for boron 11.
A pop quiz on periodic table elements includes identifying transition metals (Fe), most reactive metal (Li), non-metal (Br), alkaline earth metal (Mg), and element with three valence electrons (Al).
Diatomic elements quiz involves identifying liquid at room temperature (Br), greatest electrical conductivity (Zn), metalloid (Si), solid at room temperature (I), and gas at room temperature (F).
Elements quiz continues with elements attracted to a magnet (Fe), forming colored solutions (Cr), inner transition metal (U), chemically inert (Ar), and sulfur's unique properties.
Quiz on substances classification includes molecule (CO2), pure element (Ar), ionic compound (MgS), pure element (Zn), molecule (F2), and explanations on atoms, molecules, and compounds.
Differentiating pure substances and mixtures, understanding homogeneous (salt water) and heterogeneous (oil-water) mixtures, and identifying air as a homogeneous mixture.
Unit conversion details: 1 mile = 5280 feet = 1.609 kilometers, 1 kilometer = 1000 meters, 1 meter = 100 centimeters, 1 inch = 2.54 centimeters, 3 feet in a yard, 12 inches in a foot, and 1 milliliter equals 1 cubic centimeter.

01:04:37

Metric Conversions: Volume, Time, Distance, Speed

1000 milliliters equals one liter, key for volume conversions
Common time conversions: 1 year = 365 days, 1 month ≈ 30 days, 1 day = 24 hours, 1 hour = 60 minutes, 1 minute = 60 seconds
To convert 460 meters to kilometers, use the conversion factor: 1 kilometer = 1000 meters
460 meters = 0.460 kilometers after dividing by 1000
Converting 75 millimeters to centimeters: 10 millimeters = 1 centimeter
75 millimeters = 7.5 centimeters after dividing by 10
Multi-step conversion: 0.25 kilometers to feet using 1 mile = 5280 feet and 1 mile = 1.609 kilometers
0.25 kilometers = 820.4 feet after calculations
Converting 36 square feet to square yards: 3 feet = 1 yard
36 square feet = 4 square yards after dividing by 9
Converting 5000 cubic millimeters to cubic centimeters: 10 millimeters = 1 centimeter
5000 cubic millimeters = 5 cubic centimeters after dividing by 10 three times
Converting 30 meters per second to miles per hour: 1 mile = 5280 feet, 1 mile = 1.609 kilometers
30 meters per second = 67.1 miles per hour after calculations
Metric system conversions: Terra (10^12), Giga (10^9), Mega (10^6), Kilo (10^3), Hectare (10^2), Deca (10^1), Deci (10^-1), Centi (10^-2), Milli (10^-3), Micro (10^-6), Nano (10^-9), Pico (10^-12)
Converting 170,000 centimeters to kilometers: 1 kilometer = 1000 meters, 1 centimeter = 0.01 meters
170,000 centimeters = 1.7 kilometers after calculations

01:25:33

Determining Volume, Density, and Compound Names

Volume of a rock can be determined through water displacement method
Volume of the rock is the difference between two values, 26.2 and 24.1, resulting in 2.1
Rock's volume is the increase in volume, which is 2.1
Rock's mass is 8.4 grams, leading to a density of 4 grams per milliliter
Density in grams per cubic centimeter is 4, answering the first part of the question
Density in kilograms per cubic meter is found by converting, resulting in 4000 kilograms per cubic meter
Gold bar value calculation involves finding volume, converting to grams using density, then to dollars based on gold price
A rectangular gold bar measuring 1 by 2 by 3 inches is worth $79,700.12
Determining significant figures involves counting non-zero numbers and specific zero placements
Rounding numbers for multiplication/division and addition/subtraction requires attention to significant figures
Naming compounds involves understanding prefixes for molecular compounds and recognizing monoatomic and polyatomic ions
Naming ionic compounds follows a pattern of metal name followed by ion name, such as sodium chloride being NaCl

01:48:39

Chemical Naming and Formula Writing Essentials

Cl- is called chloride, with the ide ending for monoatomic ions.
Naming elements: MgO is magnesium oxide, CaS is calcium sulfide, AlBr3 is aluminum bromide, GaN is gallium nitride, ZnF2 is zinc fluoride.
Naming ionic compounds with polyatomic ions: BaSO4 is barium sulfate, LiClO3 is lithium chlorate, KCN is potassium cyanide, NaOH is sodium hydroxide, Sr3(PO4)2 is strontium phosphate, Mg(NO3)2 is magnesium nitrate.
Importance of knowing polyatomic ions for chemistry problems.
Using the Roman numeral system for compounds with multiple oxidation states.
Naming compounds based on oxidation states: CuCl is copper(I) chloride, CuCl2 is copper(II) chloride, FeS is iron(II) sulfide, Fe2S3 is iron(III) sulfide, PbO is lead(II) oxide, SnO2 is tin(IV) oxide.
Writing formulas for ionic compounds: LiCl, CaSe, AlN, MgBr2, Al2(SO4)3, Na3PO4, PbS2.
Nomenclature of acids: Sulfuric acid (H2SO4), Sulfurous acid (H2SO3), Hydrosulfuric acid (H2S), Perchloric acid (HClO4), Hypochlorous acid (HClO), Hydrochloric acid (HCl).
Writing formulas for acids based on their names: Phosphoric acid (H3PO4), Carbonic acid (H2CO3), Hydrobromic acid (HBr).

02:11:24

Chemistry Basics: Formulas, Mass, and Molar Mass

Hydrobromic acid formula is HBr, requiring the addition of one hydrogen.
Iodic acid, a polyatomic ion with oxygen, has the formula HIO3.
Iodic acid formula is HIO3 due to a negative one charge.
Acetic acid formula is HC2H3O2, needing the addition of one hydrogen.
Mass in chemistry is measured in grams, with one kilogram equaling a thousand grams.
A mole is a large quantity, akin to a dozen representing 12.
Molar mass is the ratio of mass to moles, with carbon's molar mass being 12.01 grams per mole.
Molar mass of methane (CH4) is 16 grams per mole.
Sodium hydroxide's molar mass is 40 grams per mole.
Glucose's molar mass is 180 grams per mole.

02:30:10

Chemical Reactions and Balancing Equations Explained

4 times 6 equals 24, and 24 times 10 to the 23rd power is 2.4 times 10 to the 24th atoms of helium.
To convert 3 times 10 to the 23 atoms of argon to grams, first convert atoms to moles using Avogadro's number: 1 mole of argon atoms equals 6 times 10 to the 23 atoms.
The molar mass of argon is approximately 40 grams per mole, so 40 grams of argon equals one mole of argon.
After calculations, the conversion results in 20 grams of argon.
Combustion reactions involve reacting propane (C3H8) with oxygen gas to produce CO2 and water.
Balancing a combustion reaction involves ensuring the atoms on both sides of the reaction are equal by adjusting coefficients.
For the combustion reaction of propane, balancing involves adjusting coefficients to have three carbon atoms, eight hydrogen atoms, and ten oxygen atoms on both sides.
Ethanol (C2H5OH) reacting with oxygen to produce CO2 and water requires balancing to have two carbon atoms, six hydrogen atoms, and seven oxygen atoms on both sides.
Combining zinc with elemental bromine results in the formation of zinc bromide, showcasing a combination reaction that is also a redox reaction.
Calcium oxide reacting with water to produce calcium hydroxide exemplifies a combination reaction that is not a redox reaction, as there are no pure elements involved.

02:48:39

Oxidation States and Redox Reactions Explained

Aluminum is in the zero oxidation state as a pure element, but in its compound, it is in the plus three oxidation state.
Hydrogen is typically in the plus one oxidation state when bonded to a non-metal like chlorine, but in a metal bond, it usually has a minus one oxidation state.
In the redox reaction discussed, aluminum is oxidized as it goes from zero to three oxidation states, while hydrogen in HCl is reduced from one to zero.
Aluminum, being oxidized, acts as the reducing agent, while hydrogen, being reduced, acts as the oxidizing agent.
In single replacement reactions, an element reacts with a compound, distinguishing it from double replacement reactions where compounds react.
Balancing the reaction involves ensuring equal numbers of each element on both sides, adjusting coefficients as needed.
In a double replacement reaction like the one discussed, the net ionic equation is derived by first writing the total ionic equation, then eliminating spectator ions to obtain the net equation.

Try it yourself — It’s free.