Chem - 1B Matter and Change

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50 Terms

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Chemistry

the study of the composition, structure, and properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes

  • physical science

  • All chemistry deals with chemicals - any substance that has a definite composition

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Energy

the ability to move or change matter

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Periodic Table

where elements are organized

  • groups/families: Vertical columns of the periodic table (18)

  • periods: Horizontal rows of elements in the periodic table

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zigzag line on the periodic table separates

metals (left) and nonmetals (right)

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Types of Elements

  • Metals

  • Nonmetals

  • Metalloids

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Metals

elements that are good electrical conductors and good heat conductors

Most are:

  • solid at room temperature

  • malleable (can be hammered or rolled into thin sheets)

  • ductile (can be drawn into a fine wire)

  • silvery or grayish white luster

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Nonmetals

elements that are poor conductors of electricity and heat

Most are:

  • gases

  • one is a liquid (bromine)

  • solids include carbon, phosphorus, and sulfur, and are britter

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Metalloids

elements that have some characteristics of both metals and nonmetals

Elements located on staircase between metals and nonmetals

All are solid at room temperature, less malleable but not very brittle, semiconductors of electricity

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Matter

anything that has mass (measure of the amount of matter) and takes up space

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Atom

the smallest unit of an element that maintains the chemical identity of that element

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Element

pure substance that cannot be broken down into simpler, stable substances

  • made of one type of atom

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Compound

a substance that can be broken down into simple stable substances

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Mixture

a blend of two or more kinds of matter, each of which retains its own identity and properties

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Types of mixtures

  • Homogeneous

  • Heterogenous

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Homogeneous

Mixtures uniform in composition also called solutions

ex:

  • salt water

  • iced tea

  • maple syrup

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Heterogenous

Mixtures that are not uniform throughout

ex:

  • chocolate chip cookie

  • salad

  • boba

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Classification of matter

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Extensive Properties

Depend on the amount of matter that is present like volume and mass

ex:

  • Volume

  • Mass

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Intensive Properties

Does not depend on the amount of matter present

ex:

  • Color

  • Melting Point

  • Density

  • Conductivity

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Chemical Properties

Relate to a substance’s ability to undergo changes that transform one substance into different substances

ex:

Burning Charcoal + Oxygen -> Carbon Dioxide

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Chemical Changes

Changes in which one or more substances are converted into different substances

  • Also called Chemical Reactions

  • Reactant → Products

ex:

Carbon + Oxygen -> Carbon Dioxide

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How do you know a chemical change has occurred?

  • color change (cooking)

  • formation of a precipitate (chunky mik)

  • formation of a gas (baking soda + vinegar)

  • evolution of energy as light (glowstick)

  • evolution of energy as heat (burning wood)

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Physical Properties

Characteristics that can be observed or measured without changing the identity of the substance including melting point and boiling point

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Physical Changes

Change that does not involve a change in the identity of the substance

ex

  • melting

  • grinding

  • cutting

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Change of State

a physical change of a substance from one state to another (ripping up paper)

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What are the states of matter?

  • Solid

  • Liquid

  • Gas

  • Plasma

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Solid

  • definite volume and definite shape

  • Very high density because particles are extremely close together

  • Incompressibility since they are so tightly packed

  • Low to no diffusion (millions of times slower than liquid diffusion)

  • Form crystal structures or amorphous solids

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Crystal

A type of solid where there is a 3D arrangement in a fixed pattern and includes gemstones

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Amorphous

A type of solid that lacks definite pattern

  • includes glass and plastic

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Liquid

  • Definite volume, but an indefinite shape

  • takes shape of the container

  • Higher density than gases due to close arrangement of particles (medium density)

  • Attraction between liquid particles caused by intermolecular forces

  • Less compressible than gases

  • Liquids will diffuse together

  • Liquids have surface tension - force that pulls adjacent liquids together

  • Capillary action - attraction of the surface of a liquid to the surface of a solid

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Gas

  • No definite shape or volume

  • Can expand to fill any volume

  • Gas particles glide past each other because they don’t attract

  • Extremely low density

  • Highly compressible (can be squished together to make smaller volume)

  • Gases will mix together automatically

  • Diffusion - spontaneous mixing caused by random motion

  • Effusion - process by which gas particles pass through a tiny opening

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Plasma

a high-temperature physical state of matter in which atoms lose most of their electrons, particles that make up atoms

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Surface tension

force that pulls adjacent liquids together

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Capillary action

attraction of the surface of a liquid to the surface of a solid

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Diffusion

spontaneous mixing caused by random motion

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Effusion

process by which gas particles pass through a tiny opening

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Chart of Solid, Liquid, Gas + their Properties

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Diagram of Change of State

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Phase Change Diagram

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What does the Kinetic-Molecular Theory of Matter state?

particles of matter are always in motion

  • Kinetics = movement

  • Molecular = molecules, particles, things

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5 Assumptions of the Kinetic-Molecular Theory of Matter (KMT

  • Gas particles are very tiny but have huge space between them (they take up more space than necessary)

  • Collisions between gas particles and between particles and container walls are elastic (no net loss of total kinetic energy)

  • Gas particles are in continuous, rapid, random motion

  • There are no forces of attraction between gas particles

  • The temperature of a gas depends on the average kinetic energy of the particles of the gas (move faster at higher temps)

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Ideal vs. Real Gas

Ideal gas = Is a hypothetical gas that perfectly fits all the assumptions of the KMT (kinetic-molecular theory)

Real gas = is a gas that doesn’t behave completely according to the assumptions of the KMT

  • At very high temperatures and low pressures real gases act most like ideal gases

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Barometer

a device used to measure atmosphereic pressure

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Manometer

a device used to measure the pressure of an enclosed gas sample

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are pressure and volume indirectly or directly related?

indirectly related

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are volume and temperature indirectly or directly related?

directly related

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are pressure and temperature indirectly or directly related?

directly related

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Accuracy

measuring near true value

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Precision

getting consistent results

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explain how a student can be accurate, precise, or both 

A student can be accurate if they have a low percent error

A student can be precise if they get the same answer more than once

A student can be both if they consistently get the correct answer multiple times