Chemistry 1210 OSU Final

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How to set up a dimensional analysis equation

(Given Unit / 1 ) X (desire unit / given unit ) = desired unit

other halogens have an oxidation number of _________ in most binary compounds.

-1 Exception: When combined with oxygen, as in oxyanions, however, they have positive oxidation states.

Examples of exact numbers

-12 eggs in a dozen -1000 g in 1 kg -Exactly 2.54 cm in an inch -The number 1 in any conversion factor ex 1 m = 100 cm or 1 kg = 2.2046 lb -Counting objects

what is the oxidation number of S^2-

-2

The oxidation number of oxygen is usually _______ in both ionic and molecular compounds.

-2 Exception: peroxides, which contain the O2^2- ion, giving each oxygen an oxidation number of −1.

Nonmetallic elements aka nonmetals

-Elements in the upper right corner of the periodic table -differ from metals in their physical and chemical properties -can be gas or solid (one liquid)

Strong acids

-HCl -HBr -HI -HClO3 -HClO4 -HNO3 -H2SO4

Strong bases

-LiOH -NaOH -KOH -RbOH -CsOH -Ca(OH)2 -Sr(OH)2 -Ba(OH)2

How to find the sig fig

-Read the number from left to right -Counting digit starting with the first digit that is not zero -All nonzero digits are significant

How to from multi step molarity problems

-grams of A----> moles of A -moles A-----> moles of B -moles of B / molarity of B= volume of B or -moles B / volume of B= molarity

Calorie to Joule equation

1 cal = 4.184 J

1 mL is the same volume as...

1 cm^3

Which has a greater density 1 kg of air or 1 kg of iron?

1 kg of iron because it occupies a smaller volume while weighing the same amount

how to do combustion analysis

1. Convert CO2 grams into grams of C 2. Convert H2O grams into grams of H 3. Add grams of C and H and subtract it from the mass of the sample to get grams of oxygen 4. Convert C, H, and O to moles 5. Use the smallest mole amount to divide all the moles including the one used 4.If not an exact number multiple all numbers until it is (Ex: 1:1.5:1 has be multiplied by 2 and we get empirical formula of 2:3:2)

How to find a derived unit

1. Define the equation for quantity 2. Substitute the appropriate base units Ex speed is the ratio of distance traveled to elapsed time. So the derived SI unit for speed is the SI unit of distance -length (m) - divided by the SI unit for time - sec - which gives m/s or meters per second

Dalton's atomic theory

1. Each element is composed of extremely small particles called atoms 2. All atoms of a given element are identical but the atoms of one element are different from the atoms of all other elements 3. Atoms of one element cannot be changed into atoms of a different element by chemical reactions. Atoms are neither created nor destroyed and chemical reactions 4. Compounds are formed when atoms of more than one element combine. A given compound always has the same relative number and kind of atoms

Naming binary (two-element) molecular compounds

1. The name of the element farther to the left in the periodic table (closest to the metals) is usually written first. An exception occurs when the compound contains oxygen and chlorine, bromine or iodine (any halogen except fluorine) in which case oxygen is written last 2. If both elements are in the same group, the one closer to the bottom of the periodic table is named first 3. The name of the second element is given an -ide ending 4. Add Greek prefixes to indicate the number of atoms of each element Exceptions: 1. the prefix mono- is never used with the first element 2. When the prefix ends in A or O and the name of the second element begins with a vowel, the a or o of the prefix is often dropped

How to find empirical formula from percent composition

1. make the percentage given into grams (74.2%= 74.2g) 2.determine the moles by using molar mass 3. Using the smaller mole divide the other moles calculated including the one used 4.If not an exact number multiple all numbers until it is (Ex: 1:1.333:1 has be multiplied by 3 and we get empirical formula of 3:4:3)

How to make a BCA chart

1. write the balanced equation 2. convert the moles or reactants to mole of desired product, which ever is the smallest is the limiting reactant 3. use the moles of limiting reactant and stoichiometric equivalence to get moles used by excess reactant 4. subtract amount the excess reactants initial amount of moles from moles used to get amount of excess left

Density of water

1.00 g/cm^3 aka 1.00g/mL

The magnitude of kinetic energy

1/2mv^2 *as velocity or mass increases so does KE

Room temperature in Celsius

25 degrees Celsius

How to find # of Cu atoms in 3g of Cu

3g Cu x (1 mol Cu/63.5 g Cu) x (6.02 x 10^23 atoms/1 mol Cu)= 3x10^22

Avogadro's number

6.02 x 10^23

Using stoichiometric equivalence to find grams of CO2 from grams of C4H10

8 mol CO2= 2 mol C4H10 1.00g C4H10 x (1 mol/58.0 g C4H10) x (8 mol CO2/2 mol C4H10) x (44.0g CO2/ 1 mol CO2)= 3.03g CO2

periodic table

A chart of all chemical elements currently known, organized by their properties.

Molecular formula

A chemical formula that indicates the actual number of atoms in each element in one molecule of a substance Ex CH4 H2O

Empirical formula

A chemical formula that shows the kinds of atoms and their relative numbers in a substance in the smallest possible whole number ratios

redox reaction

A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation-reduction reaction.

Angstrom

A common non-S I unit of length that is used to measure atomic dimensions 1A = 10^-10m

Ionic compound

A compound composed of cations and anions

Naming polyatomic ions with -ide

A few polyatomic anions also have names ending in -ide Ex OH^- hydroxide ion Ex CN^- cyanide ion Ex Osub2^2- peroxide ion

Structural formula

A formula that shows not only the number and kinds of atoms in the molecule but also the arrangement of the atoms

Conversion factor

A fraction whose numerator and denominator are the same quantity expressed in different units

Solvent

A liquid substance capable of dissolving other substances

Precision

A measure of how closely individual measurements agree with one another

Mass (Kg)

A measure of the amount of material in an object

Temperature

A measure of the hotness or coldness of an object It is a physical property that determines the direction of heat flow

dimensional analysis

A method of problem-solving in which units are multiplied together or divided into each other along the numerical values Ensures that the final answer of a calculation has the desired units

Perspective drawings

A model that uses wedges and dashed lines to depict bonds that are not in the plane of the paper. Crude 3-D shape

Diatomic molecule

A molecule consisting of two atoms Ex: H2, O2, N2, F2, Cl2, Br2, and I2

Anion

A negatively charged ion

Electrons

A negatively charged subatomic particle found outside the atomic nucleus. It is a part of all atoms. Aka CATHODE RAYS

Chemical formula

A notation that uses chemical symbols with numeric subscripts to convey the relative proportions of atoms of the different elements in a substance

Oxyanions

A polyatomic anion that contains one or more oxygen atoms

Oxidative number

A positive or negative whole number assigned to an element in a molecule or ion on the basis of a set of formal rules

Cations

A positively charged ions

Proton

A positively charged subatomic particle found in the nucleus of an atom

Distillation

A process that depends on the different abilities of substances to form gases Used in homogeneous mixtures

Filtration

A process that uses a porous barrier to separate materials based on the size of their particles.

metathesis reaction

A reaction in which two substances react through an exchange of their ions Ex:Ax+bY ---> AY+by

standard solution

A solution of know concentration

Scientific law

A statement of what is always observe to happen to the best of our knowledge

Heat spontaneously flows from...

A substance at a higher temperature to one at a lower temperature High to Low

nonelectrolyte

A substance that dissolves in water but does not contain ions and does not conduct an electric current

Solute

A substance that is dissolved in a solvent to form a solution.

Acid

A substance whose molecules yield hydrogen ions (H^+) when dissolved in water

The Celsius Scale

A temperature scale on which water freezes at 0 and boils at 100 at sea level

Theory

A tested model or explanation that has predictive powers and that accounts for all available observations

Atomic mass unit

A unit based on exactly 12 amu for the mass of the isotope of carbon that has six protons and six neutrons in the nucleus 1 amu = 1.66054 x 10^-24 g

Calorie

A unit of energy It is equal to the amount of energy needed to raise the temperature of 1 g of water by 1°C from 14.5 C to 15.5 C

How to name and formulate a cation ionic compound

A. Cations formed from metal atoms have the same name as the metal B. If a metal can form cations with DIFFERENT CHARGES, the positive charge is indicated by a Roman numeral in parentheses following the name of the metal

How to write an acid formula

Acids are always written with an H as the first element Ex HCl Ex H2SO4

Dilution

Adding water to a solution in order to decrease the concentration

What is the SI unit used for electric current?

Ampere (A or amp)

Derived Unit

An S I unit obtained by multiplication or division of one or more of the SI base units

Electrolyte

An aqueous solution that contains ions and conducts an electric current

Ion

An atom that has had its electrons removed or added so that it has a electrical charge Ions can be positively or negatively charged depending on whether electrons are lost (positive) or gained (negative) by the afoms

Neutron

An electrically NEUTRAL particle found in the nucleus of an atom.. it has approximately the same mass as a proton.

Polyatomic ion

An electrically charged group of two or more atoms Ex:NH4^+

Mass spectrometer

An instrument used to measure the precise masses and relative amounts and mixtures of substances

salt

An ionic compound made from the neutralization of an acid with a base. -it is aqueous

Composition of an acid

Anion connected to enough H+ ions to neutralize (balance) the anions charge Ex SO4^2- ion requires two H^+ ions , forming H2SO4

Property

Any Characteristic That Can Be Used To Identify a particular type of matter and distinguish it from other types

Changes of state

Any change from liquid gas or solid is a physical change

Inorganic compound

Any compound not containing carbon and hydrogen

Examples of inexact numbers

Any number obtained by measurement Any measurement obtained by equipment has inherent limitations and errors Human errors Physical surroundings vary

Elements

Any substance that cannot be broken down into simpler substances

Matter

Anything that has mass and takes up space

Structure

Arrangement of atoms

Quantitative

Associated with numbers

Qualitative

Associated with quality as in size appearance value etc

Submicroscopic

Atoms and molecules

Isotope

Atoms of the same element containing same number of protons but different numbers of neutrons and therefore having different masses

Chemical energy is consumed when

Bonds between atoms are broken

Chemical energy is released when...

Bonds between atoms are formed

What is an Atom?

Building blocks of matter (singular)

Alkane with four carbons

Butane

What is the empirical formula of C2H4?

CH2

A combustion reaction between a hydrocarbon and oxygen form...

CO2 and H2O

Capital C Calorie vs c calorie

Calorie (note the capital C) is 1000 times larger than a calorie 1 Cal = 1000 cal = 1 kcal

What is the SI unit used for luminous intensity?

Candela (cd)

The -ium ending

Cations formed from molecules composed of NONMETAL atoms have names that end in -ium Ex NH4^+ ammonium ion Ex H3O^+ hydronium ion

Naming an acid containing an anion that ends in -ate or -ite

Change -ate to -ic Change -ite to -ous Then add the word acid

Naming an acid containing an anion that ends in -ide

Change the -ide to -ic and add the prefix hydro- and follow with the word acid Ex Cl^- chloride becomes HCl hydrochloric acid Ex S^2- sulfide becomes H2S hydrosulfuric acid

Ions of the same element that have different charges have different....

Chemical and physical properties

Name the acid HClO2

Chlorous acid

What is the first step of the scientific method?

Collect information via observations of natural phenomena and experiments

How to know charges of ions

Column number for metals= charge Column number for nonmetal-8=charge

Mixtures

Combinations of two or more substances in which each substance retains its chemical identity

Isomer

Compound whose molecules have the same overall composition but different structures Ex 1-propanol and 2-propanol are structural isomers that have the same molecular formula but different structures

Hydrocarbon

Compounds composed of only carbon and hydrogen

Alcohol

Compounds of carbon and hydrogen containing only carbon-carbon single bonds Obtained by replacing an H atom of an alkane with an -OH group Name dervived from alkane but end in -ol

Alkanes

Compounds of carbon and hydrogen containing only carbon-carbon single bonds (it's a hydrocarbon)

Structural isomers

Compounds that have the same molecular formula but different structural formulas

Organic compounds

Contain carbon and hydrogen, often in combination with oxygen nitrogen or other elements

Electrolysis

Decompose water (compound) into its basic elements hydrogen and oxygen by passing an electrical current through it 11% hydrogen and 89% oxygen

Fahrenheit to Celsius equation

DegreeC= 5/9 (F-32)

Celsius to Fahrenheit equation

DegreeF = 9/5 (C) + 32

Temperature should always be specified when reporting...

Density (if not we assume 25 C)

Density equation

Density = mass / volume

How to find density with mass and volume

Density = mass / volume

Extensive properties

Depend on the amount of sample Ex depend on mass or volume

Potential energy

Determined by the position of an object relative to other objects "Stored energy" that arises from the attractions and repulsiones an object experiences in relation to other objects

Methods of Separating mixtures

Dissolving Magnet Filtration Distillation Column chromatography

Intensive properties

Do not depend on the amount of a sample being examined Can be used to identify substances Ex: Temp, melting point, and density

Naming alkanes

Each alkane has a name that ends in -ane Ex C8H18 is octane

What are the compositions of matter?

Element, compound, or mixture

Groups

Elements that are in the same column of the periodic table Elements within the same group or family exhibit similarities in their chemical behavior

Metallic elements aka metals

Elements that are usually solids at room temperature, exhibit high electrical and heat conductivity, and appear lustrous. Most of the elements in the periodic table are metals

Metalliods

Elements that lie along the diagonal line separating the metals from the non-metals in the periodic table The properties of the metalloides are intermediate between those of metals and nonmetals

Transition metals

Elements that occur in the middle of the periodic table Commonly form cations with different charges

Naming polyatomic anions containing oxygen (oxyanions)

End in either -ate or -ite and are called oxyanions Ex NO3^- nitrate ion Ex NO2^- nitrite ion Ex SO4^2- sulfate ion Ex SO3^2- sulfite ion

who discovered the proton?

Ernest Rutherford

Who disproved the plum pudding model?

Ernest Rutherford therefore JJ had beef with him

Atoms differing in number of neutrons

Ex 12/6C reads carbon-12 6 protons and 6 neutrons VS carbon atoms that have 6 protons and 8 neutrons has mass number 14

How to set up a dimensional analysis equation with multiple conversion factors

Ex speed in mi/hr = (515 m/s) ( 1 km/ 10^3 m) (1 mi / 1.6093 km) (60s/1 min) (60 min/1 hr)= 1.15 x 10^3 mi/hr

What are the two types of numbers encountered in scientific work?

Exact numbers and inexact numbers

Electrostatic potential energy

Form of potential energy which arises from the interactions between charged particles I.e. Opposites attract vs same charge repels Strength increases as the magnitude of the charge increases and decreases as the distance between charges increases

What is the second step of the scientific method?

Formulate a hypothesis

What is the fourth step of the scientific method?

Formulate a theory based on the most successful hypotheses

Giga

G=10^9

States of matter

Gas solid or liquid

What are the physical states?

Gas, solid, or liquid

Metals that form only 1 cation (only one possible charge)

Group 1A 2A and Al3+ (group 3A) and two transition metal ions: Ag^+ (group 1B) and Zn^2+ (group 2B)

What is the empirical formula of H2O?

H2O

What is the empirical formula of H2O2?

HO

Rank the acid from weakest to strongest

HX,HZ,HY

Solid

Has a definite shape and volume and is not compressible to any appreciable extent

Solution

Homogeneous mixture

The law of multiple proportions

If two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ratio of small whole numbers (review)

The law of constant composition

In a given compound, the relative numbers and kinds of atoms are constant

The prefix hypo-

Indicates one O atom fewer than the oxyanion ending in -ite Ex ClO2^- chlorite ion (one O atom fewer than chlorate) Ex ClO^- hypochlorite ion (one O atom fewer than chlorite)

The prefix per-

Indicates one or more O atom than the oxyanion ending in -ate Ex ClO4^- perchlorate ion (one more O atom than chlorate) Ex ClO3^- chlorate ion

If a result contains more than the correct number of significant figures...

It must be rounded off

How was the electron discovered?

JJ Thomson completed the cathode ray experiment. Saw that the cathode had a stream of negatively charged particles by using charged plates to bend the stream. The ray avoided the negative plate. Concluded there must be a negative particle. Called it the electron.

Who discovered the neutron?

James Chadwick

Celsius to Kelvin equation

K= degreeC + 273.15

What is the SI unit used for temperature?

Kelvin (K)

What is the SI unit used for mass?

Kilogram (Kg)

The 7 SI units

Length Mass Temperature Time Amount of substance Electric current Luminous intensity

Volume of a cube

Length^3

dilution formula

M1V1=M2V2

Mega

M=10^6

How to find mass with volume and density

Mass = Volume x Density

The magnitude of kinetic energy depends on

Mass and velocity (speed)

Pure substance

Matter that has distinct properties and a composition that does not vary from sample to sample

Milikans Oil Drop Experiment

Measured the charge of the electron. Small drops of oil are allowed to fall between electrically charged plates. Millikan measured how varying the voltage between the plates affected the rate of fall. From these data he calculated the negative charge on the drops. Because the charge on any drop was always some interval multiple of 1.602 x 10^-19 C, Millikan deduced this value to be the charge of a single electron. The force of gravity pulls drops down word but is a post by the electric field that pushes the negatively charged drops upward.

The elements of the periodic table are mostly...

Metals

What is the SI unit used for length?

Meter (m)

Simple organic molecules

Meth = 1 Eth = 2 Prop = 3 But = 4 I.e. Methane Butane Propane

Column chromatography

Mixture is separated by dissolving in a solvent Put components in a pipet/buret? Components separately solvent is added throughout the process. Each component is collected as it reaches the bottom of the column

Homogeneous

Mixtures that are uniform throughout have few compounds Aka solutions

Heterogenous

Mixtures that do not have the same composition and properties or appearance throughout In general, vary in texture and appearance in one sample Have many compounds

Nuclear model

Model of the atom with a very small and extremely dense nucleus containing most of the mass (protons and neutrons) and with electrons in the space outside the nucleus. Further most of the atom is empty space with electrons moving around the nucleus

Ball and stick models

Model that depicts atoms as spheres and bonds as sticks. Accurately represents angles

Space filling models

Model that shows relative size of the atoms - smooshed balls of color coded molecules

What is the SI unit used for the amount of a substance?

Mole (Mol)

How do we find the whole-number multiple?

Molecular weight/ empirical weight

Why is density temperature dependent?

Most substances volumes change if they are heated or cooled

Nano

N= 10^-9

Weak base

NH3

Is a measurement from a pipette exact?

NO because any measurement is inexact!

Would PbI2(s) be consider an electrolyte?

NO! its not a water soluble ionic compound

Which weighs more 1 kg of air or 1 kg of iron?

Neither they both have the same MASS!

Is O^2- a polyatomic ion?

No

will a reaction occur if Ag(s) is combined with MgNO3?

No because Mg^2+ is not a very reactive ION -higher on the reactivity series

Is a weak acid a strong electrolyte?

No but a strong acid is

Gas aka vapor

No fixed volume or shape; rather, it uniformly fills its container Can be compressed into small space or expand to occupy larger one

is millimeters a derived unit?

No its just a normal measurement

Do the number of protons in atom ever differ?

No only neutrons and electrons differ

What happens if all the ions in a complete ionic equation are spectator ions?

No reaction occurred

Can theory be proven absolutely true?

No, however, we treat it as it is true until disproven

Most stable group on the periodic table is..

Noble gases

Do isomers have the same molecular formula?

Not always

Physical properties

Observed without changing the identity and composition of the substance Ex: color, odor, density, melting point, boiling point, and hardness

Oil floats on water because

Oil is less dense than water because the molecules that make up oil are larger so they can not pack together as tightly as water so they take up more space and are more dense

Macroscopic

Ordinary sized objects

Functional groups

Other classes of organic compounds that are obtained when one or more hydrogen atoms in an alkanes is replaced with a specific group of atoms Ex alcohol

Pico

P= 10^-12

Subatomic particles

Particles such as protons neutrons and electrons that are smaller than an atom

is temperature chemical or physical property?

Physical property

Matter is classified by

Physical state and composition

Radioactivity

Possessing radioactivity; the spontaneous disintegration of an unstable atomic nucleus with accompanying emission of radiation

what are examples of metathesis reactions?

Precipitate reactions and acid-base neutralization reactions

Compounds

Pure substances that are the chemical bond of two or more elements.

precipitate reaction

Reactions that result in the formation of an insoluble product

Accuracy

Refers to how closely individual measurements agree with the correct or true value

What is the fifth step of the scientific method?

Repeatedly test theory and modify as needed to match experimental results or reject

Who discovered the charge of an electron?

Robert Millikan

Who is know for the nuclear model?

Rutherford

What is the SI unit used for time?

Second (s or sec)

The denser liquid will...

Sink to the bottom and the less dense liquid will float on top

Cathode rays

Streams of electrons that are produced when a high voltage is applied to electrodes in an evacuated tube. Cathode rays are the radiation produced between electrodes. Cathode rays originate at the negative electrode and traveled to the positive electrode

Physical change

Substance changes physical appearance but not it's composition Ex changes of state

Element

Substances that can not be decomposed into smaller substances Each element is composed of only one kind of atom

Hypothesis

Tentative explanation of a series of observations First step of scientific method

What is the third step of the scientific method?

Test the hypothesis via experiments

The Kelvin scale

The SI temperature scale 0 K = -273.15 degrees C

Joule (J)

The SI unit for energy

Energy

The ability to do work or transfer heat

Solubility

The amount of a substance that dissolves in a given quantity of a solvent at given temperature to form a saturated solution

What is density?

The amount of mass in a unit volume of a substance

Periodic table

The arrangement of elements in order of increasing atomic number with elements having similar properties placed in vertical columns

Atomic weight

The average mass of the atoms of a element in atomic mass units. It is numerically equal to the mass in grams of one mole of the element *Listed on periodic table

What is solvation?

The clustering of solvent molecules around a solute particle. It prevents cation and anion from recombining and stabilize the ions

Significant figures

The digits that indicate the precision with which a measurement is made All digits of a measured quantity are significant, including the last digit, which is UNCERTAIN

Kinetic energy

The energy of motion

Work

The energy transferred when a force exerted on an object causes the displacement of that object

Heat

The energy used to cause the temperature of an object to increase

Scientific method

The general process of advancing scientific knowledge by making experimental observations and by formulating hypotheses theories and laws

Composition

The kinds of atoms the matter contains

-ide ending of anions

The names of monatomic anions are formed by replacing the ending of the name of the element with -ide Ex H^- hydride ion Ex O^2- oxide ion Ex N3^- nitride ion

Electronic charge

The negative charge carried by an electron. It has a magnitude of 1.602 x 10^-19 C

Atomic number

The number of protons in the nucleus of an atom of an element

Law of definite proportions

The observation that the elemental composition of a compound is always the same Same as law of constant composition

Law of constant composition

The observation that the elemental composition of a compound is always the same. Same as law of definite proportions

When naming a binary compound, if both elements are in the same group...

The one closer to the bottom of the periodic table is named first and the second element is given an -ide ending

SI Units

The preferred metric units for use in science. Has seven base units.

Plum pudding model

The proposition that an Adam consists of a uniform positive spirit of matter in which the mass is evenly distributed and in which the electrons are embedded like raisins in a pudding or seeds in a watermelon

Sig Fig Multiplication and Division Rule

The results contain The same number of significant figures as the measurement with the fewest SIGNIFICANT FIGURES Ex length 6.221 cm x width 5.2 cm = 32.3492 cm^2 round to fewest sig figs (2) = 32

Sig Fig Addition and Subtraction Rule

The results should have the same number of decimal places as the measurement with the fewest DECIMAL PLACES Ex 20.42 + 1.322 + 83.1 = 104.842 round to one decimal place = 104.8

Periods

The row of elements that lie in a horizontal row in the periodic table

Atom

The smallest representative particle of an element The almost infinitesimally small building block of matter

Organic chemistry

The study of carbon containing compounds, typically containing carbon-carbon bonds

Component

The substances that make up a mixture

Mass number

The sum of the number of protons and neutrons in the nucleus of a particular atom

The law of conservation of mass

The total mass of materials present after a chemical reaction is the same as the total mass present before the reaction

Metric system

The units used for scientific measurements

Chemical properties

The way a substance may change or react to form other substances Ex: flammability

What do graduated cylinders, syringes, and burettes have in common?

They are used to deliver VARIABLE volumes

Exact number

Those whose values are known exactly Can result from counting objects

Inexact numbers

Those whose values have some uncertainty Any number obtained by measurement is inexact

What is a pipette used for?

To deliver a SPECIFIC volume

What is a volumetric flask used for

To hold a SPECIFIC volume

Transfer of heat is simply

Transfer of kinetic energy at the molecular level bc atoms and molecules gain kinetic energy and average speed increases when they are heated

Chemical change

Transformed into a substance that is chemically different from the original substance

Is this statement true or false: Whenever one substance is oxidized, another substance must be reduced.

True

What is a molecule?

Two or more atoms joined in specific shapes (can be a compound).

The last digit reported for any measured quantity is always...

Uncertain

Liter

Unit of volume 1000 mL= 1 L

Sig Fig Exponential notation

Used to indicate which zeros are insignificant 1.03 x 10^4 g has 3 sig Fig 1.030 x 10^4 g has 4 sig Fig 1.0300 x 10^4 g has 5 sig Fig

Nucleus

Very small very dense positively charged portion of an atom composed of protons and neutrons

Formula of work

W= F x d Where F is force and D is the distance that it moves

How do we know if metal will be oxidized?

We use the activity series

Rutherford scattering experiment

When alpha particles pass through a gold foil most pass-through undeflected but some are scattered, a few at very large angles. This contradicted the plum pudding model which said particles should experience only very minor deflections. The nuclear model of the atom explains why a few particles are deflected at large angles. Most of the space around the nucleus contains only low mass electrons

When is oxygen written last

When you are naming a two-element compound that contains oxygen and chlorine, bromine, or iodine (any Halogen except fluorine)

Is a joule a derived unit?

YEAH, 1 J = 1 kg-m^2/s^2 this can be seen from kinetic energy equation which is KE= 1/2 mv^2 m= kg v^2= (m/s)^2

is the actual yield always less than the theoretical?

YES

Are potential energy and kinetic energy interconveritable?

Yes

Is SO4^2- a polyatomic ion?

Yes

Is a strong base a strong electrolyte?

Yes

will a reaction occur if Mg(s) is combined with AgNO3?

Yes because Ag^+ is a very reactive ion -lower on the reactivity series

Is density a derived unit?

Yes because of its formula mass/volume= density

Are all water solube ionic compounds strong electrolytes?

Yes because they always dissociate if they are aqueous

Are most molecular compounds nonelectrolytes?

Yes but acids are an exception

Can empirical and molecular formulas be the same

Yes if the formula is already in it's simplest form

Do most elements occur in nature as a mixture of isotopes?

Yes to find there mass we use the atomic weight formula

Are spectator ion cancelled out in net ionic equations?

Yes!

Are strong bases water soluble ionic compounds?

Yes!

Sig Fig Zero Rule 2

Zeros at the beginning of a number are never significant - they merely indicate the position of the decimal point Ex 0.02 g has 1 sig Fig Ex 0.0026 cm has 2 sig Fig

Sig Fig Zero Rule 3

Zeros at the end of a number are significant if the number contains a decimal point Ex 0.0200 g has 3 sig Fig Ex 3.0 has 2 sig Fig

Sig Fig Zero Rule 1

Zeros between nonzero digits are always significant Ex 1005 kg has 4 sig figs Ex 7.03 cm has 3 sig figs

combination reaction

a chemical change in which two or more substances react to form a single new substance

combustion reaction

a chemical reaction that occurs when a substance reacts with OXYGEN, releasing energy in the form of heat and light

combustion analysis

a method of obtaining empirical formulas for unknown compounds, especially those containing carbon and hydrogen, by burning a sample of the compound in pure oxygen and analyzing the products of the combustion reaction

decomposition reaction

a reaction in which a single compound breaks down to form two or more simpler substances -heating can cause this

neutralization reaction

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

Base

a substance that accept (react with)H+ ions.

strong electrolyte

a substance that completely ionizes in a solution

weak electrolyte

a substance that only partly dissociates into ions when it dissolves in water

percent yield

actual yield/theoretical yield x 100

The oxidation number of fluorine is −1 in _____________

all compounds.

What does 0 K mean?

all thermal motion ceases (absolute zero)

stoichiometric equivalence

allows the conversion of moles of reactant to moles of a product and vice versa

What is the name of Al^3+?

aluminum ion

For an atom in its elemental form, the oxidation number is...

always ZERO Ex: H and H2

net ionic equation

an equation that includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution (form a precipitate)

complete ionic equation

an equation that shows dissolved ionic compounds as dissociated free ions

precipitate

an insoluble solid formed by a reaction in solution

displacement reaction

an ion (or atom) in a compound is replaced by an ion (or atom) of another element

spectator ion

an ion that appears on both sides of a complete ionic equation unchanged

Are non-metals cations or anions?

anions

Weak acids

any other acid that is not considered strong

Centi

c= 10^-2

Are metals cations or anions?

cations

Name the acid HClO3

chloric acid

Molecular compounds

compounds composed of different nonmetal atoms

What is the name of Cu^+ and Cu^2+?

copper (I) ion and copper (II) ion

According to Rutherford beta particles are equivalent to which subatomic particle?

electrons

What is the units used for density

g/cm^3 aka g/mL

reduction

gain of electrons Ex: H is reduced (blue)

Liquid

has a definite volume but takes the shape of its container. Is not compressible to any appreciable extent

What is standard deviation?

how much the individual measurements differ from the average

chemical equilibrium

in which the relative numbers of each type of ion or molecule in the reaction are constant over time. Chemists use half-arrows pointing in opposite directions to represent reactions that go both forward and backward to achieve equilibrium, such as the ionization of weak electrolytes

The combination of nonmetals and metal is what type of compound?

ionic compound

What is the name of Fe^2+ and Fe^3+?

iron(II) ion and iron(III) ion

An explanation for what happens...

is a theory

what happens to an aqueous ionic solid when it is put in water?

it dissociates (ion separate and disperse throughout the solution)

A substance has a solubility of .009 mol/L, is it soluble or insoluble

it is INSOLUBLE because it has a solubility of less than .01 mol/L

A substance has a solubility of .011 mol/L, is it soluble or insoluble

it is SOLUBLE because it has a solubility of greater than .01 mol/L

What is special about the acid H2SO4?

it requires two steps and only the first complete ionizes and the second only partially but it is still considered a strong electrolyte

How is matter classified?

its physical state and composition

Kilo

k=10^3

When calculating the number of atoms the number will be usually...

larger

Oxidation

loss of electrons Ex: Mg is oxidized (red)

Milli

m= 10^-3

Most matter is found as a...or...

molecule, ion (except noble gases bcuz they are stable)

Molarity equation

moles of solute/liters of solution

The oxidation number of hydrogen is usually +1 when bonded to _____________ and −1 when bonded to ______________

nonmetals, metals

How to determine the number of oxygen in an alkane

number of carbon times 2 plus 2= # of oxygen in alkane Ex: methane CH4 (1*2)+2=4

monoprotic acids yield how many H+?

one

Are molecular weight and molar mass the same thing?

pretty much

Titration

process in which a solution of known concentration is used to determine the concentration of another solution

Acid are...

proton donors (H+)

In a normal atom the number of...and... are... equal

protons and electrons

molecular equation

shows the complete formulas of all reactants and products and includes it state (s, l, g, or aq)

When calculating the number of moles the number will be usually...

small (less than 1)

What is the name of Na^+?

sodium ion

Is salt a solvent or solute?

solute

Is water a solvent or solute?

solvent

Density is dependent on...

temperature

Concentration

the amount of solute present in a given quantity of solvent or solution

The greater the amount of sig figs...

the greater the precision of the measurement

For any monatomic ion, the oxidation number equals...

the ionic charge Ex:K^+ has a +1 charge

molar mass

the mass of one mole of a substance in grams

where does most of mass of atom come from?

the nucleus (protons and neutrons)

elemental composition

the percentage composition of any element in a substance

equivalence point

the point in a titration at which the added solute reacts completely with the solute present in the solution

theoretical yield

the quantity of product that is calculated to form when all of the limiting reagent is used

limiting reactant

the substance that controls the quantity of product that can form in a chemical reaction

excess reactant

the substance that is not used up completely in a reaction

molecular weight

the sum of the atomic weights of all the atoms in a molecule -used in MOLECULAR formula

formula weight

the sum of the atomic weights of the atoms in the chemical formula of the substance -used in EMPIRICAL formula

strong bases and strong acids are similar in that....

they both completely ionize in a solution and are considered strong electrolytes

weak bases and weak acids are similar in that...

they both only partially ionize in a solution and are considered weak electrolytes

diprotic acid yield how many H+?

two

Micro

u= 10^-6

What are examples of weak electrolytes?

weak acids and weak bases

The molecular formula can be found by multiplying the empirical formula by the...

whole-number multiple

Forms of energy

work and heat

The sum of the oxidation numbers of all atoms in a neutral compound is __________. The sum of the oxidation numbers in a polyatomic ion equals _____________________

zero, the charge of the ion

What is the name of Zn^2+?

zinc ion


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