CHM 114- Midterm Exam Guide - Comprehensive Notes for the exam ( 27 pages long!)
ASU
CHM 114
MIDTERM EXAM
STUDY GUIDE
CHM 114-Lecture 1-Introduction
Chemistry: the study of matter and the changes matter undergoes
Atom: smallest building block of matter
Matter (see ppt for definition) is categorized by its properties (any characteristic that allows us
to recognize and distinguish matter)
• Properties of matter affected by atomic composition and structure organization
• Observation of matter occur on a macroscopic (eyesight) and submicroscopic (atomic)
levels
• Physical properties examples: color, odor, density, melting/boiling point, and hardness
• Chemical properties example: flammability
• Physical vs. Chemical Changes and Intensive Vs. Extensive Properties (see ppt for more
information)
*definition of physical and chemical properties is similar to definition of physical and
chemical changes
*chemical change is also referred to as a chemical reaction
States of Matter (classification of matter)
• Gas (vapor)
o Particles far apart
o No fixed volume (assumes the shape of its container)
o Can be compressed to occupy smaller volume
• Liquid
o Particles flow less easily than gas particles, but more than solid particles
o Distinct volume
o Cannot be compressed
• Solid
o Particles locked into place
o Definite shape and volume
find more resources at oneclass.com
find more resources at oneclass.com
o Cannot be compressed
• Changes in temperature and/or pressure leads to the changing of states
Pure Substance: matter that has a fixed composition and distinct properties
Element: 1) substance made up of atoms with the same atomic number
2) substance that cannot be separated into simpler substances through chemical
means
*see ppt to see how elements are arranged and denoted on the periodic table
• Compounds vs. Mixtures (see ppt for more detail)
• Law of Constant Composition (aka the Law of Definite Proportions): the composition of
pure compound is always the same, regardless of its source
Separation of Mixtures
• Mixtures can be separated by taking advantage of the elemental properties of its
components
• Methods
1) Filtration: separation of solids from a fluid (either gas or liquid) by allowing the fluid
to pass through a filter
2) Distillation: use of heat to separate the components of a liquid by boiling it and then
condensing the vapor that results
o Good Reference: https://www.youtube.com/watch?v=98b028c6h44
*NOT IMPORTANT FOR LECTURE, USEFUL OF LAB ONLY
Units of Measure
• Properties of matter are usually quantitative
• Metric system and SI Units
*Check Atoms, Ions, and SI Units Tab under Additional Chapter Notes on Blackboard for
reference
• Temperature
find more resources at oneclass.com
find more resources at oneclass.com
Document Summary
Chemistry: the study of matter and the changes matter undergoes. *definition of physical and chemical properties is similar to definition of physical and chemical changes. *chemical change is also referred to as a chemical reaction. Pure substance: matter that has a fixed composition and distinct properties. Element: 1) substance made up of atoms with the same atomic number. 2) substance that cannot be separated into simpler substances through chemical means. *not important for lecture, useful of lab only. Units of measure: properties of matter are usually quantitative, metric system and si units. *check atoms, ions, and si units tab under additional chapter notes on blackboard for reference: temperature, celsius (oc) vs kelvin (k, conversion: k = oc + 273. 15, conversion for celsius to fahrenheit and vice versa. Of = (9/5) oc + 32: absolute zero: lowest attainable temperature ( 0 k or -273. 25 oc) Density (see ppt for definition: density and weight are not the same thing.
