Chem honors unit 1: Matter and Change

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Organic chemistry

The study of chemistry that is carbon-containing

Inorganic chemistry

The study of chemistry that deals with non-organic things (non-carbon containing things)

Biochemistry

The study of chemistry that pertains to living things

Analytical chemistry

The science of obtaining, processing, and communicating information about the composition and structure of matter

Physical chemistry

The study of properties/changes of matter and energy associated

Theoretical chemistry

The study of the mathematical perspective of the behavior of chemical compounds

Matter

Anything that has mass and takes up space.

What can be matter?

Can be solid, liquid, gas or plasma

What can’t matter do?

Be created or destroyed (in normal chemical reactions). However, it can change forms

Law of Conservation of Mass (also called Conservation of Matter and Conservation of Energy)

In a normal chemical reaction, matter cannot be created or destroyed. It can only change forms.

Mass

A measure of the amount of matter in an “object”

What units do we use for mass?

g, mg, kg

States of Matter- Solids

definite shape, definite volume

States of Matter-Liqiuds

no definite shape, definite volume

States of Matter- Gasses

no definite shape, no definite volume

Gasses (vs vapors)

are typically in the gaseous phase at room temperature.

Vapors (vs gasses)

are substances that are typically in the solid or liquid phase at room temperature.

Phase changes

As temperature changes, as well as pressure, substances can change phases.

What can phase changes go to/from?

can be from solid ←🡪 liquid ←🡪 gas or even solid ←🡪 gas.

Melting/Freezing

Occurs when a substance changes from solid ←🡪liquid

What temps does melting/freezing occur?

Melting of ice and freezing of water both occur at 0ºC.

Boiling/Condensing

occurs when a substance changes from liquid ←🡪gas.

What temps does boiling/condensing occur?

Water boils at 100ºC. Steam condenses at 100ºC

Sublimation

occurs when a substance changes directly from solid to gas.

sublimation example

Dry ice (solid CO 2 ) and iodine sublime

Properties of Matter

Describe the composition, structure and behavior of a substance.

Properties of matter examples

color, mass, boiling pt., flammability, taste

Qualitative Properties

a property that can be expressed without measurement

Quantitative properties

a property that uses measurement

Quantitative properties example

mass, temperature, melting point

Qualitative properties example

color, smell, flammability, reactivity with water

Extensive properties

depend on the amount of matter present

Intensive properties

not dependent on the amount of matter present

Extensive properties example

Mass, volume

Intensive properties example

Temp, color, ratios of 2 extensive properties

Physical properties

observable with the senses and can be determined without destroying the object.

Physical properties examples

mass, length, density, specific heat

Chemical properties

indicates how something reacts (or doesn’t) with something else.

Chemical properties examples

via destroying the substance or having a chemical reaction

Physical change

a change in matter that does not involve a change in the composition of individual substances.

Does Physical change produce a new substance?

no

Chemical change

a change in matter that does involve a change in the composition of a substance

physical change examples

salt in boiling water(just changing form), sponge in water

Does chemical change produce a new substance?

yes

Chemical change examples

burning wood, rusting, baking soda and vinegar

Indicators/Signs of a Chemical

Change/Reaction

color change

Indicators/Signs of a Chemical

Change/Reaction

Precipitate(solid) formed when 2 solutions react

Indicators/Signs of a Chemical

Change/Reaction

gas produced(bubbles)

Indicators/Signs of a Chemical

Change/Reaction

Odor change (smells diff)

Indicators/Signs of a Chemical

Change/Reaction

energy change (gain or lose energy)

Types of heat and energy change

endothermic and exothermic

exothermic

energy (light/heat) is lost/given off; it can feel warmer

exothermic examples

fire, hand warmers

endothermic

Energy (light/heat) is gained/taken in; it can feel cooler

endothermic examples

chemical icepack, photosynthesis

There can be an energy change (endothermic or exothermic) even if there is not a chemical change

true

pure substance

Matter with the same composition throughout. It can be an element or a compound.

Elements

simplest form of matter that can’t be broken down into smaller substances

Element examples

Kr, K, Mg, B, Al

compounds

chemical combination of 2 or more elements joined together in a fixed proportion

what are compounds represented by?

by a formula

mixture

A combination of two or more substances in

which each substance keeps its unique set of

properties. It can be separated into two or

more pure substances.

types of mixtures

Heterogeneous and homogeneous

Heterogeneous mixture

A mixture that has multiple phases.

– Individual substances can clearly be “seen” in the

mixture and are not uniformly distributed.

Homogenous mixture

A mixture that has one phase; substances are

evenly distributed.

– There is a constant composition throughout.

Heterogeneous mixture examples

Skittles, hetero ppl

Homogeneous mixture examples

redbull, cookies, air

what are Homogeneous mixtures are also known as

Homogeneous mixtures are also known as

solutions

Solutions consist of?

solute and solvent

Solute

the substance being dissolved

Solvent

the substance that dissolves the

solute.

solute and solvent example

water and salt

Alloy

A solid solution usually made up of two or

more metals

alloy examples

stainless steel, brass, bronze

Periodic Table of Elements

The periodic table is organized into periods and

groups/families based on properties.

Periods are horizontal or vertical?

horizontal

how many periods are there

there are 7 periods numbered from top to bottom

(1-7)

what does each new period represent

each period represents a new energy level

groups are vertical or horizontal?

vertical

how many groups

there are 18 groups numbered from left to right

(1-18)

do elements within groups have similar properties

yes

Metals are left or right of the stair- step

left of the stair-step

metals can do what with heat and electricity

conduct heat and electricity well

Metals have how much luster

high luster/shiny (often gray or white, but can be yellow

or brown)

Are metals malleable and ductile?

yes

what phase of matter is metal typically

generally solids at room temperature

• (Hg is a liquid)

Nonmetals are left or right of the stair- step

right of the stair-step

Nonmetals can do what with heat and electricity

do not conduct heat and electricity well

Nonmetals have how much luster

lack luster

are Nonmetals malleable and ductile

brittle, not really

what phase of matter is nonmetals typically

many are gases at room temperature (some are

solids, Br is a liquid)

Metalloids are left or right of the stair- step

Along/touching the stair-step

Metalloids

B, Si, Ge, As, Sb, Te, Po, At

Metalloids have what properties

have properties of both metals and nonmetals

Metalloids can do what with electricity

some are semiconductors, they conduct electricity better than nonmetals but not

as well as metals

how to make metalloids more conductive

conductivity can be improved by doping – adding

another element

h

hydrogen

Is hydrogen an alkali metal or alkaline earth metal

Group 1 ( Alkali metals)

li

lithium

Is lithium an alkali metal or alkaline earth metal

Group 1 ( Alkali metals)