Chemistry Winter Quizlet

-20⁰C = ____⁰F (Round to the nearest degree)

-4⁰F

57 mL = ______ L

0.057

How many significant digits area in the number 0.009?

1

Multiply the following three numbers and report your answer to the correct number of significant figures: 0.020 cm x 50 cm x 11.1 cm

1 x 10 cm³

Specific Heat

1. A physical property of a substance 2. The heat capacetiy of 1 gram of a substance.

1cm³ = ___ mL

1cm³ = 1mL

Centi

1m=10²cm. Unit prefix meaning one hundredth. Symbol = c

Milli

1m=10³mm. Unit prefix meaning one thousandth. Symbol = m

Micro

1m=10⁶µm. Unit prefix meaning one millionth. Symbol = µ

Nano

1m=10⁹nm. Unit prefix meaning one billionth. Symbol = n

2 cm = ______mm

20

Compound

A chemical compound is a pure chemical substance consisting of two or more different chemical elements that can be separated into simpler substances by chemical reactions.

exothermic reaction

A chemical reaction that releases energy to its surroundings

Tyndall

A colloid is one of the three primary types of mixtures, with the other two being a solution and suspension. Scatters light, does not settle on standing. A subtype of heterogeneous mixture.

Suspension

A colloid is one of the three primary types of mixtures, with the other two being a solution and suspension. Separates on standing. A subtype of heterogeneous mixture.

chemical formula

A combination of chemical symbols and numbers to represent a substance

Mole

A counting unit used to calculate objects that are very small in size and large in number

Temperature

A measurement of the average kinetic energy of a molcule

Metric System

A measurement system based on the number 10 which uses prefix to make the unit larger or smaller than the base.

Molecule

A molecule is two or more atoms join together chemically.

Significant figures

All certain digit and one estimated digit.

Wood Burning

Chemical Change

f block

Covers the Lathanides and Actinides

d block

Covers the Transition Metals

s block

Covers the alkaline metals and alkaline earth metals. It is spherically symmetrical

dichromate ion

Cr2O7 2-

chromate ion

CrO4 2-

Allotrope

Different forms of the same element. Pure substances!

Atomic Radii

Distance from nucleus to outermost e⁻shell. - ↑ down a group b/c more e⁻ are added to shell, ↓ across a period b/c more e⁻ and p⁺ are added & effective nuclear charge (e.n.c) is greater.

Techniques for Separating Mixtures

Distillation - separate two liquids w/ different boiling points Filtration - porous barrier to separate solids from liquids

Converting from atoms to moles

Divide the number of particles by Avogadro's number to determine the number of moles

hydrogen carbonate ion

HCO3 -

hydrogen phosphate ion

HPO4 2-

hydrogen sulfate ion

HSO4 -

Desired bunsen burner flame

Is blue with and inner and outer cone

ammonium ion

NH4 +

Hund's Rule

The Half Rule; No orbitals shall have a two electrons occupying it until all the orbitals in a subshell have been filled.

Tyndall Effect

The Tyndall Effect is the effect of light scattering in many directions in colloidal dispersion, while showing no light in a true solution.

Energy

The ability to do work

Heat Capacity

The amount of heat needed to raise the temperature of the object by 1 degree Celsius.

Mass

The amount of matter in an object. SI unit = kg

Volume

The amount of space that a substance or object occupies. SI = m³

True or false? All compounds are molecules but not all molecules are compounds.

True!

Compounds

Two or more elements combined CHEMICALLY; pure substance that CAN be separated by chemical means; can be identified by a chemical formula that is always the same

Mixtures (of Matter)

Types of Mixtures (Homogeneous & Heterogeneous)

Homogeneous Mixture

Uniform,constant composition; components are in a single phase; A.K.A: solutions

Z (number of protons)

atomic number

Dalton's Atomic Theory

1. All matter (materials) consists of very small particles called atoms. 2. An element consists of atoms of one type only 3. Compounds consist of atoms of more than one element and are formed by combining atoms in whole-number ratios. 4. In a chemical reaction, atoms are neither created nor destroyed

Heat of Fusion

1. The amount of heat needed to convert a solid at its melting point to a liquid. 2. The amount of heat needed to convert a unit mass of a substance from solid to liquid at its melting point 3. q= mHfus 4. M=Mass 5. Hfus= Heat of Fusion Heat of Fusion: 334 J/g 6. q= Heat in Joules

Heat of Vaporization

1. The amount of heat needed to convert a unit mass of a substance from its liquid phase to its vapor phase at a constant temperature. 2. q= mHvap 3. q= Heat(in Joules) 4. m= mass 5. Hvap= Heat of Vaporization 2260 J/g

Heat

1. The measure of the amount of energy transferred from one substance to another. 2. Heat is measured in Calories or Joules.

What are the 3 States of Matter?

1. solid 2. liquid 3. gas

water's density?

1.00g/mL

Kilo

10³m=1 km. Unit prefix meaning one thousand. Symbol = k

Mega

10⁶m=1 Mm. Unit prefix meaning one million. Symbol = M

Giga

10⁹m= 1Gm. Unit prefix meaning one billion. Symbol = G

64⁰F = ____⁰C (Round to the nearest degree)

18⁰C

Equivalence statement

2 statements with different units that are equal. Ex: 1 inch = 2.54 cm

3.5 g = ______mg

3,500

The speed of light in a vacuum is exactly 299,792,458 meters per second. Write this number in scientific notation with the coefficient rounded to the hundredths place.

3.00 × 10⁸

Write 3,465 in scientific notation.

3.465×10³

How many significant digits are in the number 0.000005721?

4

Water (H₂0) Specific Heat

4.18 J/g °C or 1.00 cal/g °C

Write 45,870,320 in scientific notation.

4.587032 × 10⁷

Find the sum of 23.6 liters, 4.75 liters, 12.065 liters, and 9.11 liters using the correct precision.

49.5 L

Divide the following numbers and report your answer to the correct number of significant figures: 0.530 g / 0.1010 mL = ?

5.25 g/mL

67.2 m = ______ cm

6,720

7,939 mg = ______ g

7.939

Which symbol makes the following statement true? 7,500 ______ 7.5 × 10³

=

Which symbol makes the following statement true? 568 ______ 5.1 × 10²

>

coefficient

A number placed in front of a formula in an equation to indicate the number of molecules of a substance

subscript

A number written slightly below and to the right of a chemical symbol that shows how many atoms of an element are in a compound.

Units

A particular amount (g, L, km)

Dimensional Analysis

A problem solving method scientists use to convert units of measurement. Uses equivalence statements as ratios and cross out units.

chemical reaction

A process that produces one or more substances that are different from the original substance (like baking or burning)

Chemical property

A property or characteristic of a substance that is observed during a reaction in which the chemical composition or identity of the substance is changed:

Pure substance

A pure element or compound contains only ONE substance, with no other substances mixed in. Impure materials are mixtures of elements, mixtures of compounds, or mixtures of elements and compounds.

endothermic reaction

A reaction that absorbs energy in the form of heat.

chemical equation

A representation of a chemical reaction that uses symbols to show the relationship between the reactants and the products

Quantum Numbers

A series of numbers to classify location of electron

Precipitate

A solid that forms from a solution during a chemical reaction.

products

A substance formed as a result of a chemical reaction

reactants

A substance or molecule that participates in a chemical reaction

Electron Affinity (EA)

Ability to acquire e. When atom accepts electron, energy is released (meaning it's negative) - ↑ up a group b/c atomic size decreases upwards, ↑ across a group b/c of increased enc.

Electronegativity

Ability to attract shared e⁻ to itself. - ↓ down a group b/c greater the size of atom, more electron shielding occurs, ↑ across a period. Group 18 does not apply.

silver ion

Ag +

Alloy

An alloy is a solid mixture that contains two or more metals (occasionally a non-metal like carbon) mixed together.

Atom

An atom is the smallest constituent unit of matter that has the properties of a chemical element.

Element

An element is a type of atom that is defined by its atomic number (#of protons in its nucleus). Ex: Au, S, Fe

Conversion Factor

An equivalence statement written as a ratio: 1inch/2.54cm or 2.54cm/inch

Mass Spectrometer

An instrument used to determine the relative atomic mass of an element.

Calorimeter

An object used to measure the heat in a chemical reaction.

Chemical Change

Any change that results in the formation of new chemical substances. At the molecular level, chemical change involves making or breaking of bonds between atoms.

Matter

Anything that has mass and occupies space.

Isotopes

Atoms of same elements with different numbers of neutrons.

barium ion

Ba 2+

Physical change verbs

Bend, tear, boil, freeze, melt

bromide ion

Br -

Chemical change verbs

Burn, tarnish, combust, cook, digest

acetate ion

C2H3O2 -

oxalate ion

C2O4 2-

cyanide ion

CN -

carbonate ion

CO3 2-

calcium ion

Ca 2+

Physical change

Changes that result in a difference in display without changing the composition.

Proton

Charge: +1 Mass: 1.660539 x 10^-24g

Electron

Charge: -1 Mass: 9.10938291 × 10-28 grams

Neutron

Charge: 0 Mass: 1.660539 x 10^-24g Discovered by British physicist James Chadwick in 1932. Found Beryllium to emit neutrons and based on mass calculations, he was able to prove that the particles were in fact neutrons and not gamma rays as previously though.

Adding Aluminum foil to copper chloride solution

Chemical Change

Burning magnesium metal

Chemical Change

Dynamite exploding

Chemical Change

Giving your hair a permanent

Chemical Change

Iron Rusting

Chemical Change

Milk souring

Chemical Change

Passing an electric current through water

Chemical Change

Silver tarnishing

Chemical Change

Corrosive Liquid

Chemical Property

Gasoline is flammable

Chemical Property

Helium will not form compounds

Chemical Property

Inert gas

Chemical Property

Sodium has the ability to combine with chlorine

Chemical Property

chloride ion

Cl -

Heterogeneous Mixtures

Composition is NOT uniform; individual substances are distinct; components are not blended smoothly

p block

Covers column of Boron to the Noble gases. It is dumbbell shaped.

Density

D=M/V. The ratio between mass and volume.

____________ is a technique used to separate elements in a compound. This process breaks chemical bonds.

Electrolysis

Pure Substances can be either __________ or __________

Elements / Compounds

Continuous Spectrum

Emitting a range of wavelengths continuously. Such as a rainbow created when light penetrates a glass prism.

Law of Conservation of Energy

Energy cannot be created or destroyed.

Potential energy

Energy due to position.

Exothermic

Energy moves from system to the surroundings.

Endothermic

Energy moves from the surroundings to the system.

Ionization Energy (IE)

Energy required to remove an e⁻from gas phase. "Jumps" really high once a stable ion is formed. - ↑ up a group b/c atom size decreases and becomes hard to pull e⁻ away , ↑ across a group b/c greater enc means stronger pull to nucleus.

Physical property

Ex: luster, odor, color, density, temperature, boiling point, malleability, ductility

fluoride ion

F -

Filtration

Filtration is a separation technique that is used to separate heterogeneous mixtures solid that has not dissolved in a liquid (for example a precipitate).

Fills the entire volume of a container

Gas

Converting grams to moles

Given 237g of H2O, how many moles?

Molar Mass of a single molecule

Grams per mole

Alkali Metals

Group 1 elements: Most chemically reactive, very soft, forms ions with Group 17 elements, and rapidly oxidize.

Alkaline Earth Metals

Group 2 elements: Forms basic solutions w/ water, hard, have higher mp, bp, and density than Group 1.

Halogens

Group 7 elements: salt formers. all diatomic molecules, except At; all nonmetals, form ionic salts with Group 1 elements

Noble Gases

Group 8 elements: least reactive (inert) of all elements; all nonmetals, have a full outer shell.

hydride ion

H -

dihydrogen phosphate ion

H2PO4 -

Metalloids

Have intermediate properties of metals and nonmetals.

Quantum Mechanical Model of the Atom

Heisenberg, de Broglie, and Schrodinger created this. The truth is, electrons have wave-length properties and occupy orbitals (each holds only 2 electrons).

mercury (II) ion

Hg 2+

mercury (I) ion

Hg2 2+

Solution

Homogeneous mixture.

iodide ion

I -

Law of Multiple Proportion

If two elements X and Y combine in different ways to form more than one compound, the masses of X that combine with a fixed mass of Y can be expressed as a ratio of small whole numbers (Ex. When Mass of N: 1.00g N₂O -> Mass of O: 0.571g; NO -> Mass of O: 1.14g; NO₂ -> Mass of O: 2.28g; NO₃ -> Mass of O: 4.57g) - John Dalton, 1804

Heisenberg Uncertainty Principle

It states that it is impossible to pinpoint location of electron and the momentum of a particle simultaneously.

Cathode Ray Tube

J.J. Thomson worked on cathode rays which he suggested consists of very small negatively charged particles called electrons. He then developed the Plum Pudding Model.

Heterogeneous Mixtures - examples

Juice with pulp; fruit salad, chef's salad, Greek salad; vegetable soup; oil/vinegar/soil and water; crunchy peanut butter; carbonated soft drinks

Kelvin Scale

K = C + 273.15. A temperature scale with zero degrees K defined as absolute zero (no molecular movement)

Non-metals

Lack all physical properties of metals; brittle

lithium ion

Li +

Has a definite volume but it takes the shape of a container

Liquid

Aufbau Principle

Literally building up from the bottom; e⁻ fills lowest energy level first.

Law of the Conservation of Mass

Mass is neither created nor destroyed. Therefore the total mass of matter following a chemical reaction is equal to the total mass of matter before the start of the reaction. Brought to you by Antoine Lavoisier!

Mass to Particle Conversions

Mass must first be converted to moles and then moles to particles Can be combined into one equation for a mass to particle conversion

Molar Mass of a Compound

Mass of one mole of formula units For example: H2O

law of conservation of mass

Matter is not created or destroyed in any chemical or physical change

rate of reaction

Measure of how fast a chemical reaction occurs

Distilation

Method for separating liquid mixtures into their individual components by boiling.

magnesium ion

Mg 2+

permanganate ion

MnO4 -

Metals

Most elements are this; conducts heat and electricity, is malleable, ductile, and lustrous

Converting from moles to atoms

Multiply the number of moles by Avogadro's number to determine the number of atoms or particles for a particular element

nitrite ion

NO2 -

nitrate ion

NO3 -

sodium ion

Na +

Molar Mass / Molecular Weight

Number of atoms X Grams per mole

Valence Electrons

Number of outermost e⁻; determine chemical properties

oxide ion

O 2-

hydroxide ion

OH -

Effective Nuclear Charge

Overall attraction that e⁻ experiences.

phosphate ion

PO4 3-

Absorption Spectrum

Pattern of dark lines against a coloured background.

To find an element look on the _________ ________

Periodic Table

Density, color, odor, hardness, shape, weight, change of state (melting / freezing / evaporation / condensation / sublimation / deposition / dissolving) are all examples of _____________ properties

Physical

Boiling alcohol

Physical Change

Cutting your hair

Physical Change

Dry ice changing to carbon dioxide gas

Physical Change

Iodine subliming

Physical Change

Sugar dissolving in water

Physical Change

Water evaporating

Physical Change

Water vapor condensing

Physical Change

Wood being carved

Physical Change

Car oil is a viscous liquid

Physical Property

Hard mineral

Physical Property

Malleable Metal

Physical Property

Shiny Metal

Physical Property

red powder

Physical Property

silly putty is an amorphous solid

Physical Property

the freezing point of water is 0˚C

Physical Property

Noble Gas Configuration

Preceding noble gas represents core e⁻ of atom (ex. CA = [Ar]4s²

Paramagnetism

Property of attraction to magnetic field. atoms of these substances have unpaired e⁻

Diamagnetism

Property of repulsion to magnetic field. atoms of these substances have paired e⁻.

Chemical Properties

Reacts or doesn't react Forms a new compound... a new color is produced...a gas is formed...a solid is formed from two liquids

Rounding off

Reducing the digits in a number while trying to keep its value similar.

sulfide ion

S 2-

sulfite ion

SO3 2-

sulfate ion

SO4 2-

Distillation

Separation of two or more substances based on boiling point.

Emission Spectrum

Series of lines against a dark background.

Radioisotopes

Short for radioactive isotopes. Unstable atomic nucleus and emit energy and particles when it changes to a more stable form. Goes through radioactive decay. Examples of human use: Positron Emission Tomography (PET) Cobalt-60 (emits gamma rays to treat cancer) Carbon-14 (Half life: 5730, archaeology)

tin (IV) ion

Sn 4+

Definite shape, definite volume.

Solid

Electromagnetic Spectrum (EMS)

Spectrum of wavelengths that comprise the various types of electromagnetic radiation (ex. radio waves, microwaves, infrared radiation, ultraviolet radiation, X-rays, and gamma rays.)

Pauli Exclusion Theory

States that any orbital can hold a maximum of two electrons of opposite spin.

Modern View of the Atom

Stresses that the nucleus (of protons and neutrons) take up the center and is extremely small. Just as the nucleus accounts for the weight, the electrons around it account for the space.

SI Units

System of units of measurements that is widely used all over the world. There are only four units that we covered in depth: Mass (kg), length (m), volume m³, temperature (k)

Law of Definite Proportion

The law states that a compound always has the same proportions of elements by mass. For example, if you measure the mass of sulphur and oxygen in sulphur tri-oxide, SO₃ will always contain 1 part sulphur and 3 parts oxygen by mass.

Atomic Mass Units

The mass of a single atom of an element 1 a.m.u. = 1.66 X 10^-24 grams

Avogadro's Number

The number of representative particles in one mole of a substance 6.02 X 10^23

Formula Units

The simplest ratio of ions for the compound Used to describe compounds rather than single elements

The hottest part of an optimal flame is:

The top of the inner cone

Conversion Factors

To convert mass to particles follow down arrows To convert particles to mass follow up arrows

Isoelectronic

Used to describe atoms that have same e⁻ configuration (Ne = Na⁺)

Filtration

Used to remove a solid from a liquid:f Ex: separate coffee grounds from coffee solution

Rutherford's Gold Foil Experiment

Using a block containing radioactive alpha particles, Rutherford shot these particles at a piece of gold foil which projected these deflected beams onto a circular zinc sulfide fluorescent screen. This lead to the discovery of the nucleus as some alpha particles were deflected at astonishing angles and there had to have been a denser mass in the atom.

Orbital Diagram

Using boxes to represent "building up" of atoms

Solid or liquid that is in the gaseous state

Vapor

Scientific notation

Way of writing very small or very large numbers. Consists of a coefficient, base ten and an exponent. Ex: 2.5 x 10³

zinc ion

Zn 2+

Chemical Changes (chemical reaction)

burning, combustion, corrosion, decomposition, digestion explosion, fermentation, oxidation, photosynthesis, rusting, tarnishing

Evidences of a Chemical Reaction

change in color, change in odor, production of a gas (bubbling), production of heat or light or sound, absorbing of heat or light

law of conservation of energy

energy cannot be created or destroyed only changed from one form to another

Kinetic energy

energy due to motion of molecules (chemistry)

Surroundings

everything that surrounds the system (including the thermometer!)

Millikan Experiment

found the mass of the electron.

Atomic Spectrum of Hydrogen

hv = Energy. (h = 6.63 x 10⁻³⁴J s; frequency) When hydrogen bonds absorb energy, the bonds break and become excited. Immediately, they release it as light and gives off a unique emission spectrum.

Coal

ignore

Fossil Feuls

ignore

Greenhouse effect

ignore

Infrared radiation

ignore

Natural Gas

ignore

Petroleum

ignore

Add energy to a solid and it becomes a __________

liquid (melting)

What two states of matter will flow?

liquids & gases

A (number of neutrons)

mass number

Electron Configuration

method to indicate distribution of e⁻in atom. (eg.1s²: 1st energy level, s block, 2 electrons)

Physical Change Examples

phase changes (Melting-Freezing or Boiling-Vaporizing-Condensating or sublimating-depositing); crumpling, crushing, cutting, folding, mangling, mixing, tearing, sawing, etc

Types of Solutions

solid-solid mixture ( alloys - usually two metals) solid-liquid mixture ( salt+water or sugar+water) liquid-liquid mixture (water+alcohol or water+antifreeze) gas-liquid mixture (O₂and CO₂ in seawater) gas-gas [air - N₂and O₂; scuba tank gases]

Ionic Radii

states: - cations are smaller b/c of lost outer e⁻ - anions are larger b/c of gained outer e⁻

System

the chemical or physical change that you are studying

chemical bond

the force that holds two atoms together in a molecule

Common Compounds

water (H₂O) table salt (NaCl) sucrose - sugar (C₆H₁₂O₆) carbon dioxide (CO₂) carbon monoxide (CO) ammonia (NH₃) hydrogen peroxide (H₂O₂) methane gas (CH₄)

Sublimation

when a solid changes directly to a gas (solid CO₂ turns to a vapor)