Accelerated Chemistry Chapter 1 Notes Name ______

Accelerated Chemistry Chapter 1 Notes Name ______(Student’s edition)

Chapter 1 problem set: 4, 5, 7, 9, 14, 18, 19, 20, 21, 24, 29

1.1 What is Chemistry?

Chemistry - the study of the , , and of substances and the they undergo. example – .

Most of the building materials, clothes, and medicines today are the result of .

Branches of Chemistry

- carbon chemistry - non-carbon chemistry - the study of energy and matter - the chemistry of living things - chemistry that identifies, quantifies, and qualifies

The Scientific Method - a logical way of solving problems

1. – state facts, collect data, search literature

qualitative vs. quantitative data ( vs. )

2. – organize data, analyze data, find relationships that lead to a hypothesis

Hypothesis – a statement - an educated guess about why a law occurs - may be discarded after later experiments or may become a law

Law - a describing a wide variety of behavior in nature Example: periodic law

3. Theorizing – how something occurs – often involves models Example: atomic theory

Theory - a generalization that explains a body of facts, but remains .

4. Testing – based on predicting the outcomes of an .

If testing fails, go back to steps 1, 2, or 3

1.2 Matter and Energy

Matter

Matter – anything that has and takes up .

Mass and weight – used interchangeably, but there is a difference…

Mass – quantity of , fixed amount

Weight - effect of on matter – changes with location

Law of Conservation of Mass – matter cannot be or in an ordinary chemical reaction (keyword being ordinary)

Energy

Energy – the ability to cause or do .

Kinetic – energy of

Potential – energy

Law of Conservation of Energy – energy can be from one form to another, but cannot be created or destroyed in an ordinary chemical reaction.

Why ordinary again? Extraordinary reactions ( ) happen where mass is converted into ( )

Types of energy – electrical, mechanical, chemical, sound, heat, electromagnetic radiation (energy of waves)

States of Matter

Phase of matter Solid Liquid Gas

Diffusion Particle closeness Definite volume Definite shape Compressibility Density Attractive Forces

Plasma – gas at extremely high temperature ( 1 x 108 K) where ______separate from the nucleus

Draw pictorial representations of phases of matter here:

Solid Liquid Gas

Properties and Changes of Matter

Properties – that enable us to distinguish one kind of matter from another

Physical property - Properties that can be observed without changing the of the material – 2 types of physical properties:

Intensive – of the amount ex. mp, bp, density, color, temperature

Extensive – on the amount ex. size, weight, mass, length, volume, heat

Chemical property – a property that can be observed when changing a substance into a substance ex: ______

Physical change – change in a substance which change the substance into something new. Ex.

Chemical change – a process where one or more substances are converted into other substances with characteristics.

Na (s) + Cl2 (g) → NaCl (s) reactant reactant product

Examples of chemical changes – .

Signs of a chemical change: ______

Precipitate – formation of a solid when mixing two

Energy and Changes in Matter - Chemical reactions involve energy

Exothermic ( heat) Endothermic ( heat)

Reactants → Products + Reactants + → Products water (l) → ice + heat →

Graph Graph

Other reactions – synthesis of water (exo), decomp. of CaCO3 (endo)

Classification of Matter Chart

Pure substance – a sample of Mixture – combination of two or matter where every particle is the ______more kinds of matter, but each ______its own properties

Element – substance that cannot be ______Homogeneous– uniform composition ______by ordinary chemical change where every sample is the same example – ______example – ______

Compound – substance that _____ be decomposed Heterogeneous – composition is _____ into 2 or more substances by chemical change uniform where samples are different example –______example – ______

All elements and compounds are homogeneous. Only some mixtures are homogeneous. Homogenous mixtures are transparent.

______– the smallest particle of some elements. Examples – ______

______– the smallest part of some elements and the smallest particle of all compounds Examples (elements) – ______Examples (compounds) – ______

Any element that is made of single atoms is also made of molecules, but the reverse is not necessarily true!

Classify these examples – Iron (Fe), milk, distilled water, tap water, chili, Co, CO, PbCl2

Law of Definite Composition – When a chemical compound is broken down, it always gives the same ______of its constituent elements (Joseph Proust – 1799)

Example – sugar C6H12O6 – ______(______)

1.3 The Chemical Elements

Draw picture of periodic table here – label group/family, period, metals, metalloids, nonmetals

Metals – (shine) Malleable (malleability) – ability to be into a sheet Ductility (ductile) – ability to be . High tensile strength – resistant to when pulled heat and electricity

Nonmetals – opposite of metals

Metalloids – some properties of metals and nonmetals – .

Nobel gases - .