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GOB Chemistry Study Guide: Matter, Elements, and Atomic Structure

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Test 1 Study Guide: GOB Chemistry

Overview

This study guide covers foundational topics in General, Organic, and Biological (GOB) Chemistry, focusing on matter, elements, the periodic table, and atomic structure. The material is organized according to the test outline and lecture content provided.

Matter and Energy

Classification of Matter

  • Pure Substances: Materials with a fixed composition and distinct properties. Examples: elements (e.g., gold, oxygen) and compounds (e.g., water, sodium chloride).

  • Mixtures: Physical combinations of two or more substances. Can be homogeneous (uniform composition, e.g., saltwater) or heterogeneous (non-uniform, e.g., salad).

States of Matter

  • Solids: Definite shape and volume; particles are closely packed.

  • Liquids: Definite volume, no definite shape; particles can move past each other.

  • Gases: No definite shape or volume; particles are far apart and move freely.

Physical vs. Chemical Changes

  • Physical Change: Alters the form or appearance but not the composition (e.g., melting ice).

  • Chemical Change: Produces new substances with different properties (e.g., rusting iron).

Changes of State

  • Melting: Solid to liquid

  • Freezing: Liquid to solid

  • Boiling/Evaporation: Liquid to gas

  • Condensation: Gas to liquid

  • Sublimation: Solid to gas

  • Deposition: Gas to solid

Energy Concepts

  • Specific Heat: The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.

  • Formula:

  • Where q = heat (J), m = mass (g), c = specific heat (J/g°C), ΔT = temperature change (°C).

  • Boiling Point: The temperature at which a liquid changes to a gas.

Elements and the Periodic Table

Element Names and Symbols

  • Be able to spell and recognize the chemical symbols for common elements (see list below).

Element

Symbol

Aluminum

Al

Argon

Ar

Arsenic

As

Barium

Ba

Boron

B

Bromine

Br

Cadmium

Cd

Calcium

Ca

Carbon

C

Chlorine

Cl

Chromium

Cr

Cobalt

Co

Copper

Cu

Fluorine

F

Gold

Au

Helium

He

Hydrogen

H

Iodine

I

Iron

Fe

Lead

Pb

Lithium

Li

Magnesium

Mg

Manganese

Mn

Mercury

Hg

Nickel

Ni

Nitrogen

N

Oxygen

O

Phosphorus

P

Potassium

K

Rubidium

Rb

Sulfur

S

Silicon

Si

Selenium

Se

Tin

Sn

Uranium

U

Zinc

Zn

Periodic Table Structure

  • Periods: Horizontal rows on the periodic table.

  • Groups: Vertical columns; elements in the same group have similar chemical properties.

  • Metals, Nonmetals, Metalloids: Metals are typically shiny, conductive, and malleable; nonmetals are more likely to be gases or brittle solids; metalloids have properties intermediate between metals and nonmetals.

Periodic Trends

  • Atomic Size: Generally increases down a group and decreases across a period.

  • Ionization Energy: The energy required to remove an electron from an atom; increases across a period and decreases down a group.

  • Metallic Character: Increases down a group and decreases across a period.

Atoms and Atomic Structure

Atomic Theory

  • Atoms are the basic units of matter, composed of protons, neutrons, and electrons.

  • Protons: Positively charged particles in the nucleus.

  • Neutrons: Neutral particles in the nucleus.

  • Electrons: Negatively charged particles in orbitals around the nucleus.

Atomic Number, Mass Number, and Isotopes

  • Atomic Number (Z): Number of protons in the nucleus; defines the element.

  • Mass Number (A): Total number of protons and neutrons.

  • Isotopes: Atoms of the same element with different numbers of neutrons.

  • Calculating Atomic Mass:

Electron Configuration

  • Electrons are arranged in shells, subshells, and orbitals.

  • Shells: Principal energy levels (n = 1, 2, 3, ...).

  • Subshells: s, p, d, f (types of orbitals within a shell).

  • Orbitals: Regions of space where electrons are likely to be found.

  • Electron configuration describes the arrangement of electrons in an atom.

Example: Electron Configuration of Oxygen (O)

  • Atomic number = 8

  • Electron configuration: 1s2 2s2 2p4

Lab: Elements

  • Be familiar with the names and symbols of common elements.

  • Understand how to identify elements based on their properties and periodic table position.

Test Format

  • Section A: Multiple Choice (24 points)

  • Section B: True & False (10 points)

  • Section C: Diagram (5 points)

  • Section D: Matching (5 points)

  • Section E: Short Answers (16 points)

  • Total: 60 points

Note: You will not have access to a periodic table during the test. Memorize key element names, symbols, and periodic trends.

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