Chem 1124 Chapter 1 Flashcards

-State of Matter

-Fixed Shape

-Fixed Volume

Solid

-State of Matter

-Takes Shape of Container

-Forms Horizontal Surface

-Fixed Volume

Liquid

-State of Matter

-Expands to Fill Container

Gas

-State of Matter

-Gaseous

-Contains appreciable numbers of electrically charged particles

*Kinda like superheated Gas

Plasma

The total amount of matter within an object is described as an objects ___.

Mass

___ refers to the force that gravity exerts on an object.

*Differs per planet

Weight

The Law of Conservation of ___ states:

Whatever we begin with, no matter what changes it goes through, will have the same building blocks.

*Melt a piece of candy; whatever it’s made of is still around in that puddle and in the air

Matter

When matter changes among solid, liquid, or gaseous states, it goes through a ___ change.

Physical

When matter converts from one type to another entirely, it experiences a ___ change.

*Typically, irreversible

Chemical

-Pure Substance

-Composed of only one type of atom

Ex. Diamond (100% C)

Oxygen(100% O)

Element

-Pure Substance

-Composed of 2+ different atoms

Ex. H2O (Water) = O and H

NaCl (Table Salt) = Na and Cl

Compound

When 2+ substances are combined without chemical reaction occurring is described as a ___.

*Can be separated by a physical process

Ex. Brass, Air, Sand, CCCD Ice Cream

Mixture

-Mixture

-Uniform Composition

-Looks the same throughout mixture

Ex. Brass, Air

Homogenous

-Mixture

-Composition Varies

-Looks different throughout mixture

Ex. Sand, CCCD Ice Cream

Heterogenous

-Characteristic

-Stays same no matter chemical composition

-Can be measured without changing matter’s identity

Ex. Electrical Resistance

Density

Hardness

Boiling/Freezing Point

Physical Property

-Change in State/Properties of Matter

-No change in chemical composition

Ex. Melting

Boiling

Evaporation

Crushing

Physical Change

-Can be observed when chemical reaction occurs

-Chemical composition has changed

Ex. Flammability

Chemical Bond Formation

Breaking Chemical Bonds

Reactivity with O2

Chemical Properties

-Change in state/property of matter

-Change in chemical composition

Ex. Rusting

Burning Wood

Fruit Rotting

Chemical Change

-Weight

-Volume

-Internal Energy

-Size

-Length

-Area

these are all examples of ___ properties.

*Depends on amount of matter present (More stuff vs. less matters)

Extensive

-Boiling Point

-Melting Point

-Hardness

-Density

-Malleability

-Refractive Index

these are all examples of ___ properties.

*Does not rely on amount of matter present (More stuff vs. less stuff doesn’t matter)

Intensive

In this class, we use a __ to measure length.

*Represented by m

Meter

In this class, we use a __ to measure mass.

*Represented by kg

Kilogram

In this class, we use a __ to measure time.

*Represented by s

Second

In this class, we use __ to measure temperature.

*Represented by K

Kelvin

In this class, we use a __ to measure amount of substance.

*Represented by mol

Mole

Density = Mass/___

*Density determines what floats

Volume

To change a standard unit to microunit you have to multiply it by 10 to the ___.

-6

To change a standard unit to milliunit you have to multiply it by 10 to the ___.

-3

To change a standard unit to kilounit you have to multiply it by 10 to the ___.

3

To change a standard unit to megaunit you have to multiply it by 10 to the ___.

6

To change a standard unit to centiunit you have to multiply it by 10 to the ___.

-2

All nonzero digits are ___ significant

Always

Zeros are only significant ___.

Sometimes

__ digits in scientific notation are significant.

All

Zeros in between non-zeros are significant

True

Trailing zeros are significant except after a decimal

False

Leading zeros are __ significant

Not

How many sig figs?

6.57 × 10^9

3

How many sig figs?

0.00000004

1

How many sig figs?

2,561,000

4

When identifying sig figs for multiplication/division:

*The answer should have as many sig figs as your __ uncertain number (number with least number of sig figs)

Most

When identifying sig figs for addition/subtraction:

*The answer has as many sig figs as the __ places of the number we are adding with the least number of decimal places

Decimal

When figuring out sig figs of a problem with multiplication/division and addition and subtraction:

Do not ___ until all done solving the problem.

Round

-Close to the true value

-Average of measurements is close to the truth

A value is ___ if these are true.

Accurate

-Is repeatable

-Does not necessarily need to be close to the truth

-Consistent results

Precise

This is a diagram of an ___

Atom

The blue dots in the atom represent ___.

*e⁻

-1 charge

Electrons

The red dots in the atom represent ___.

p+

+1 charge

*Determines the identity of an element

Proton

The green dots in the atom represent ___.

n°

No charge

Neutrons

An ___ is:

-An element with the same number of protons and electrons

-Has a differing number of neutrons

-Has a different mass due to differing number of neutrons

Isotope

For an atomic symbol:

“A” represents our ___ ___.

*Consists of the number of protons + Neutrons in atom

Mass Number

For an atomic symbol:

“Z” represents our ___ ___.

*Consists of the number of protons

Atomic Number

For an atomic symbol:

“X” represents our ___ ___.

*One or two letter abbreviation of element name

Element Symbol

When an atom has a differing number of electrons than its number of protons, the atom is described to be an ___.

Ion

-Ion

-More Protons than electrons (Can only remove electrons)

-Positive Ion

Cation

-Ion

-Less Protons than electrons (Can only remove electrons)

-Negative Ion

Anion

Protons — Electrons = ___ ___ of an atom.

Total Charge

Unit used to deal with small masses of individual atoms

*(amu)

Atomic Mass Unit

This equation is how you find the ___ ___ of elements

Average Mass

The little number next to the hydrogen (H) is referred to as a ___.

Subscript

The big number next to the hydrogen (H) is referred to as a ___.

Coefficient

___ formula uses the chemical abbreviation to signify the number/types of atoms present in a molecule/compound.

Molecular

___ formula gives us same info as molecular formula but also how atoms are connected.

Structural

6.022×10²³ is also referred to as ___.

*A mole of something

*Nₐ

Avogadro’s Number

A compounds ___ formula indicates:

-Types of atoms present

-Simplest Whole-Number Ratio of number of atoms in the compound

Empirical Formula