Chem: Ions, Compounds, and Atoms

Here are your flashcards formatted for easy copying into Knowt:

Flashcard Set: Chemistry Chapter 2 Review

Q: What does the atomic number represent?
A: The number of protons in an atom's nucleus.

Q: What is the mass number?
A: The sum of protons and neutrons in the nucleus.

Q: What does the symbol of an element represent?
A: The abbreviation of an element from the periodic table.

Q: How many protons does a neutral atom have?
A: Same as the atomic number.

Q: How many electrons does a neutral atom have?
A: Same as the number of protons.

Q: What is the average atomic mass?
A: The weighted average of all naturally occurring isotopes.

Q: What does the group name tell you?
A: The family of elements with similar chemical properties.

Q: What determines the charge of an ion?
A: The loss or gain of electrons.

Q: How do you determine the number of electrons in an ion?
A: Adjust the protons minus charge (e.g., Na⁺ has 11-1 = 10 electrons).

Isotopes

Q: How are isotopes of the same element alike?
A: They have the same number of protons and same chemical properties.

Q: How are isotopes of the same element different?
A: They have different numbers of neutrons, affecting mass.

Q: Symbol for chlorine-37?
A: 1737Cl^{37}_{17}Cl

Q: Symbol for carbon-12?
A: 612C^{12}_{6}C

Q: Symbol for oxygen-18?
A: 818O^{18}_{8}O

Q: Symbol for uranium-235?
A: 92235U^{235}_{92}U

Q: Symbol for hydrogen-3?
A: 13H^{3}_{1}H

Q: How do you find the number of neutrons in an isotope?
A: Mass number - atomic number.

Atomic Mass Calculation

Q: Formula for calculating atomic mass?
A: (Mass of Isotope 1×Abundance)+(Mass of Isotope 2×Abundance)(\text{Mass of Isotope 1} \times \text{Abundance}) + (\text{Mass of Isotope 2} \times \text{Abundance})

Q: What is the calculated atomic mass of carbon?
A: (12.000×0.9889)+(13.000×0.0111)(12.000 \times 0.9889) + (13.000 \times 0.0111).

Subatomic Particles

Ions & Their Names

Q: Name of Ca²⁺?
A: Calcium ion

Q: Name of N³⁻?
A: Nitride ion

Q: Symbol for rubidium ion?
A: Rb⁺

Q: Symbol for sulfide ion?
A: S²⁻

Q: Symbol for lead (II) ion?
A: Pb²⁺

Q: Symbol for permanganate ion?
A: MnO₄⁻

Naming Ionic Compounds

Q: Name of BI₃?
A: Boron triiodide

Q: Name of HgCl₂?
A: Mercury(II) chloride

Q: Name of Rb₃PO₄?
A: Rubidium phosphate

Writing Ionic Formulas

Q: Formula for potassium phosphite?
A: K₃PO₃

Q: Formula for copper (II) chlorate?
A: Cu(ClO₃)₂

Q: Formula for zinc sulfide?
A: ZnS

Naming Molecular Compounds

Q: Name of PCl₅?
A: Phosphorus pentachloride

Q: Name of N₂O₄?
A: Dinitrogen tetroxide

Writing Molecular Formulas

Q: Formula for dinitrogen heptaphosphide?
A: N₂P₇

Q: Formula for carbon tetrabromide?
A: CBr₄

Q: Formula for tricarbon hexoxide?
A: C₃O₆

Hydrocarbons

Q: Name of an 8-carbon alkane?
A: Octane (C₈H₁₈)

Q: Name of a 3-carbon alkene?
A: Propene (C₃H₆)

Q: Name of a 1-carbon alkane?
A: Methane (CH₄)

Acids

Q: Name of H₂SO₃?
A: Sulfurous acid

Q: Formula for nitric acid?
A: HNO₃

Q: Formula for hydrochloric acid?
A: HCl

Q: Formula for hydroiodic acid?
A: HI

Hydrates

Q: What does the formula of a hydrate indicate?
A: It shows the water molecules attached to the compound (e.g., CuSO₄·5H₂O).

This set should be easy to copy into Knowt for flashcard studying! Let me know if you need modifications. 😊

Compounds (CH 2-5)

Notes

Compounds

Formation of compounds

Ionic compounds

Molecular compounds

Compounds- A chemical combination of two or more different elements joined together in a fixed proportion.

Ex.  H₂0, CaCO₃, NaHCO₃   

Types of compounds

• Binary Compound: a compound containing two elements

Ex. NaCl, CaCl₂ 

• Ternary Compound: compound containing MORE than two elements

Ex. KNO₃, NH₄OH 

Chemical formulas indicate the number and type of atoms present in a compound

• A molecular formula shows the EXACT number of atoms of each element in the smallest unit of a substance H20

• An empirical formula shows the simplest whole-number RATIO of the atoms in a substance

Molecular v. Empirical

• For some compounds, the empirical formula is the SAME as the molecular formula

EX. CH₄ (methane) and NaCl* (sodium chloride)

  * for all ionic compounds, their formula is their empirical formula- they do not form molecules

• Different compounds can have the same empirical formula

EX. CH is the empirical formula for C₂H₂ (ethene) and C₆H₆ (benzene)

Formation of Compounds

Why do atoms combine? 

• Atoms combine to achieve stability 

How are compounds formed?

• Atoms must collide

• The valance electrons of the colliding atoms interact

Valence electrons: Electrons located in the outermost energy levels of an atom

Octet Rule: Atoms will gain, lose, or share electrons in order to fill their outer energy level

• Most atoms fill with 8 electrons (octet)

• Hydrogen and Helium fill with 2 (exception)

• A full valence shell results in chemical stability 

  • Achieve a mobile gas configuration 

• Whether atoms will transfer electrons or share electrons depends on what atoms are involved

Transfer or Share? 

Metals and nonmetals will transfer electrons

• ionic compound

• ionic bond

• Metals lose (become positive) and nonmetals gain electrons (become negative)

Nonmetals will share electrons with other nonmetals and metalloids

• molecular compound 

• Covalent bond

Properties of Compounds

Ionic 

Ex. NaCl 

Ionic bonds-strong bond/attraction between ions

High melting points

Brittle solide @ room temp

Electoryocltes

Soluble in water

TO BE STABLE # HAS TO BE 8

Molecular (Covalent)

Ex. CO₂

_{Covalent bonds-weaker attractipn}

_{Low melting points/boling points}

_{solids/liquids/gases at room temp}

_{Nonelectroyletes.} 

Ionic Compound: A compound composed of ions

An ion is an atom, or group of atoms, that has a net positive or negative charge. 

• cation – ion with a positive charge

If a neutral atom loses one or more electrons it becomes a cation. 

• anion – ion with a negative charge

If a neutral atom gains one or more electrons it becomes an anion. 

A monatomic ion contains only ONE atom  (Na+ or Cl-)

A polyatomic ion contains more than one atom (HCO3-bicarbonate) (CN- Cyanide) (OH- hydroxide) 

Determining Charge

• Ions have either gained or lost electrons in order to have a full valence

• Typically 8 electrons

Using the valence for the atom, determine whether it is easier to gain or lose in order to make 8

Valence? 

• Use the periodic table

• Atoms in the same group have the same valence

(on the periodic table to show the valenece electrons) 

Charge? 

Naming Cations

• If the charge is always the same (representative elements/Group A), just write the name of the element

  • K⁺  potassium ion\

  • ZINC 2+

  • SILVER 1+ (TRICK THAT WAINSCOTT JEWELRY IS HER NUMBER ONE CHOICE) 

    • ZINC AND SLIVER NEVER GET ROMAN NUMERALS. ZINC IS ALWAYS +2 AND SILVER IS ALWAYS 1+. NO ROMAN NUMERALS

• Transition metals can have more than one type of charge, so we use Roman numerals to indicate what the charge is

  • Cr²⁺ chromium (II) ion

  • SN (TIN) +PB (LEAD) NEED A ROMAN NUMERAL

Name These

Al³⁺   

• ^{AL- ALUMINUM  ION}

Ca²⁺     *CA- CALCIUM ION 

Fe³⁺     *Fe^{3+    IRON (III) ION} 

Fe²⁺     *fE 2+ iRON (II) ION 

Naming Anions (DIFFERENT THEN CATIONS) 

• Always the same

• Change the element ending to -IDE

Ex.  F1^- Fluorine

                                                     -ide Fluoride ion

Name These

Cl^1-   

• ^{CHLPRODE ION}

N^3-

• ^{NITRIDE  ION}

S^2- 

• SULFIDE ION

P^3- 

• PHOSFIDE  ION

Polyatomic Ions

• Groups of atoms that are COVALENTLY_ bonded with an overall CHARGE

• Easiest to just memorize 

Naming Ionic Compounds

• often a metal + nonmetal

  • Simply name the ion

  • sodium chloride (NaCl), calcium carbonate (CaCO3), magnesium oxide (MgO), potassium bromide (KBr), aluminum chloride (AlCl3), iron (II) oxide (FeO), and copper (II) sulfate (CuSO4)

• Transition metal ionic compounds

  • indicate charge on metal with numerals

  • iron(III) oxide (Fe2O3), copper(II) chloride (CuCl2), manganese(IV) oxide (MnO2), mercury(II) oxide (HgO), chromium(III) chloride (CrCl3), cobalt(II) bromide (CoBr2), and vanadium(V) fluoride (VF5). 

  • FE CL2

Write the names of the following

Na₂Se

KCl 

CaSO₄ 

Ca₃N₂

Sc₃P₂ 

PbO₂

PbO 

(NH₄)₂O

Formulas of Ionic Compounds (GET FROM MS. SIEGAL)

The sum of the charges on the cation(s) and anion(s) in each formula unit must equal ________

To Determine the formula:

1. Write the symbol of each ion including the charge

2. Find the least common multiple (LCM) for the charges of the ions

3) Determine what factor* you must multiply each charge by in order to get the LCM

* This factor is the subscript in the formula

Molecular Compounds- Compounds that form molecules

Molecular (covalent) Compounds

• Combination of nonmetals or nonmetals and metalloids

• A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds

A diatomic molecule contains only TWO atoms

Ex. H₂, N₂, O₂, Br₂, HCl, CO

A polyatomic molecule contains more than two atoms

Ex. O₃, H₂O, NH₃, CH₄

The Seven Diatomic Elements (must have two of the same element) 

Br₂  I₂  N₂  Cl₂  H₂  O₂  F₂

Naming Molecular Compounds (Inorganic) 

• Use prefixes to determine the number of atoms of each element present in a molecule

• The last element always ends in -ide

Some guidelines…

• The prefix “mono-” may be omitted for the first element in the formula

Ex. PCl₃  is  phosphorus trichloride NOT monophosphorus trichloride

• Avoid vowel combinations of “ao”; omit the ending “a” in the prefix

Ex. Dinitrogen Tetroxide NOT Tetraoxide

Name These

CCl₄  carbon tetrachloride 

N2O dinitrogen monoxide 

SF₆  sulfur hexafluoride 

Write formulas for these

Remember:  Use prefixes to tell you the number

Arsenic trichloride  ArCl₃ 

Dinitrogen pentoxide  N₂O₅ 

Tetraphosphorus decoxide  P₄ O₁₀