11th Chemistry- Fall final review Flashcards by Carson Daniel

What are scientific notation rules?

• Know how to round-off to 2 decimals.

10^x (?). SCI display mode on the calculator

6,720,000,000. = 6.72x10^9. moved decimal point 9 to left

0.25 = 25x10^-2. moved decimal point 2 to right

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Define mass and volume?

What units are they measured in?

Mass - Density * Volume. M=D*V. also called weight
measured in grams (g). measure of matter & gravity force

Volume - Mass/Density. V=M/D. space occupied by matter
measured in cm3 or mL

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How would you calculate density?

D=m/V

Compute volume if needed. cm3 or mL.
ensure you are using mass(m) in grams (g)

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Indicate whether the following properties increase or decrease from left to right across the periodic table

atomic radius (excluding noble gases)
first ionization energy
electronegativity.

Decreases. - atomic radius (excluding noble gases)
Increases. - first ionization energy
Increases. - electronegativity.

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What is density?

D=m/V. Mass/Volume

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Definitions of: kilo-, centi-, milli-

kilo- 1,000. Ex. kilometer. 1,000 meters
10^3
centi-1/100th. Ex. centimeter. 1/100th meter
10^-2
milli- 1/1000th. Ex. millimeter. 1/1000th meter
10^-3

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If doing a density calculation and given a liter of water or a block measuring 0.5 meters per side, what must you first do?

Convert liter to 1000mL
or
compute volume. —> convert to 5cm then—> 555 = 125cm3

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What is another name for mass?

Mass = weight. or force of gravity on matter

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What is the difference between carbon 12 and carbon 13 if all carbon atoms have an atomic number of 6?

C12 has 6 neutrons

C13 has 7 neutrons

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How many electrons, neutrons, and protons does Chromium-58 have if the element has an atomic number of 24?

Protons - 24
Electrons - 24
Neutrons - 34

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What does the number next to the isotope signify?
A. Atomic number
B. Atomic mass
C. Place on the periodic chart
D. Number of electrons

B. Atomic mass. Protons + neutrons

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Atomic mass consists of 
A. Protons and electrons
B. Protons and neutrons
C. Electrons and neutrons
D. Protons, electrons and neutrons

B. Protons and neutrons

Electrons are practically without mass

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How many electrons, neutrons, and protons does Nitrogen-20 have if the isotope has an atomic mass of 20?
A. 5 electrons, 10 neutrons and 5 protons
B. 4 electrons, 8 neutrons and 8 protons
C. 7 electrons, 6 neutrons, and 7 protons
D. 7 electrons, 13 neutrons, and 7 protons

D. 7 electrons, 13 neutrons, and 7 protons

Remember — Only neutrons and protons = atomic mass
13. +. 7. =. 20

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If boron-10 and boron-11 both have an atomic number of 5 how many electrons, neutrons, and protons does the isotope have?

5 protons - atomic #
5 electrons also
Boron-11 has 6 neutrons
Boron-10 has 5 neutrons

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T/F

If an element were to add an extra proton it would become an entirely new element.

True.

As atomic number changes, the element moves on the periodic table of elements.

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Naturally occurring Europium (Eu) consists of two isotopes with a mass of 151 and 153. Europium 151 has an abundance of 48.03% and Europium -153 has an abundance of 51.97%. What is the atomic mass of Europium?

151 * .4803 + 153 * .5197 = 152.04

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Boron exists in two isotopes, boron-10 and boron-11. Based on the atomic mass, which isotope should be more abundant?

Boron because the mass number is closer to the atomic mass listed on the periodic table

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Which of the following are true of isotopes?
A. Isotopes are different versions of the same element
B. Same number of protons for isotopes of the same elements
C. Different number of neutrons between isotopes of the same element
D. All of the above are true

D. All of the above are true

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Titanium has five common isotopes. Ti46 (8.0%), Ti47(7.8%), Ti48 (73.4%), Ti49(5.5%), and Ti50(5.3%). What is the average atomic mass of titanium?

2.65

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T/F

Isotopes of a given element have the same atomic mass but a different atomic number

False. Same atomic number.

Atomic mass differs based on # of neutrons.

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If carbon has six protons how many electrons does it have?

Six also.

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T/F

If an extra neutron were added to an element, it would become an entirely new element.

False.

Adding a neutron increases only the atomic weight and makes it an isotope of the element. ( i.e. C12 becomes C13)

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How can you tell isotopes of the same element apart?
A. Compare atomic number
B. Compare atomic mass
C. Look them up on the periodic chart
D. Count the number of electrons

B. Compare atomic mass

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Which of the following are elements and which are compounds?
Ice. Sodium Chloride
Nickel. Silicon. Francium

Elements - Nickel. Silicon. Francium

Compounds - Ice. Sodium Chloride

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``` Which of the following is an example of a compound? A. gold B. Silver C. Aspirin D. Copper ```

C. Aspirin

Iced tea with ice cubes in it would be a homogenous/heterogenous mixture?

With ice cubes - heterogenous Without ice cubes - homogenous. Tea fully dissolved into water

A ______________ is a form of matter with a uniform and unchanging composition

Substance.

What separates substances based on their movement through a special paper?

Chromatography

``` What are the vertical columns in the periodic table called? A. Block elements B. Groups or families C. Grids D. Periods ```

B. Groups or families

T/F | The words gas and vapor can be used interchangeably

True.

______________ properties can be measured without altering the chemical properties of the substance.

Physical

T/F | A liquid has a definite shape and takes on the volume of its container

False. | Definite VOLUME and takes on the shape of its container

T/F | A solid has a definite shape and volume

True

Which of the following are pure substances, homogenous mixtures, and heterogenous mixtures? Salt water. Water Water & sand mix. Solutions

Pure substance - water. All H2O Homogenous mixture - Solution or Salt water Heterogenous mixture - water & sand mix

Matter is anything with __________ and ____________.

Mass. Volume

T/F | Liquids tend to contract when heated

False. Contract when cooled - Ice | Expand when heated - water boiling over in a pan

Indicate whether the following properties increase or decrease from top to bottom down the periodic table - atomic radius (excluding noble gases) - first ionization energy - electronegativity.

Increases. - atomic radius (excluding noble gases) Decreases - first ionization energy Decreases - electronegativity.

What separates solids from liquids using a porous barrier?

Filtration

What is an element? What is a compound? How can elements be separated out?

Element - pure substance such as oxygen, nickel or gold Compound - combination of substances such as water (H2O) or salt (sodium Chloride) Elements separated out through a chemical process??????

What trend in ionization energy occurs across a period on the periodic table? Why?

Ionization energy INCREASES as you move right in the period. Less metallic. Requires more energy to remove a valence electron

How is mass different than weight?

Mass remains the same despite gravity. Weight differs based on the gravitational force. Ex - your mass is the same on earth and on the moon. Your weight on the moon would be much less than on earth due to less pull of gravity.

``` The density of gold is 19.3 g/ml. What is the volume of a piece of gold that weighs 63.3g? A. 5.623 ml B. 3.28 ml C. -33.68 ml D. 35.2 ml E. 67.243 ml ```

B. 3.28 ml

What shows the relationship between the reactants and products in a chemical reaction?

Chemical equation

T/F | The particles in a gas cannot be compressed into a smaller volume.

False. Think compressed air/CO2 cartridge/bicycle tire

``` As you travel down a group or family on the periodic chart, which is true? A. Atomic radius increases B. Atomic number decreases C. Ionization energy increases D. Electronegativity increases ```

A. Atomic radius increases. <- - - - | increases |

Substances have specific, unchanging ___________ which can be measured.

Properties

``` A substance that cannot be separated into simpler substances by either physical or chemical means is a A. Compound B. Mixture C. Element D. Period ```

C. Element

The starting substances in a chemical reaction are called what?

Reactants

Substances have both ____________ and ___________ properties

Physical Chemical.

Which of these are physical properties? Which are chemical properties? Size Weight. Mass. Color. Boiling/Melting point Solid/Liquid/Gas at normal temps/pressures. Conducts electricity. Chemical composition (H2O) Combines with another substance

Physical. - size, weight/mass, color, Chemical properties - combines with another substance

``` Which of the following is an example of an element? A. Air B. Water C. Sugar D. Oxygen ```

D. Oxygen

How can a homogenous mixture be separated out to the substances that make them up? How can a heterogenous mixture be separated out to the substances that make them up?

Homogenous - such as salt Crystallization. Distillation. Chromatography????? Heterogenous - such as sand and water Filtration.

``` Convert 9,830 grams to pounds (1 lb = 453.6g) A. 2.17 x 10^-2 lb B. 4.46 x 10^3 lb C. 21.7 lb D. 4.46 x 10^6 lb E. 4.46 lb ```

C. 21.7 lb

____________ properties CANNOT be observed without changing the composition of a substance.

Chemical

What method separates substances by formation of solid, pure particles from a solution?

Crystallization

Anything that has mass and takes up space is called A. weight B. matter C. volume D. weight

B. matter

``` Classify each of the following as a physical or chemical property A. Iron and oxygen form rust B. Iron is more dense than aluminum C. Magnesium burns brightly when ignited D. Oil and water do not mix E. Mercury melts at -39° Celsius ```

A. Iron and oxygen form rust- chemical B. Iron is denser than aluminum- physical C. Magnesium burns brightly if ignited- chemical D. Oil and water do not mix- chemical E. Mercury melts at -39° Celsius- physical

A chemical reaction that involves one or more substances changing into new substances is called _________________?

Chemical change

T/F | The particles in a solid are spaced far apart

False. Closely packed. Touching.

``` What are the horizontal rows in the periodic table called? A. Block elements B. Groups or families C. Grids D. Periods ```

D. Periods

178g of water is separated into hydrogen gas and oxygen. If the hydrogen gas has a mass of 20g. What is the mass of the oxygen?

158g. Conservation of mass

T/F | An element is a combination of two or more compounds.

False. A single homogenous substance

T/F | When a small amount of sugar is completely dissolved in water, a heterogeneous solution is formed

False. Homogenous

Describe the differences in atom spacing within a solid, liquid and gas. How would the appear differently in these different states?

Solid - atoms packed together, touching. Defined shape Liquid - atoms farther apart and sliding past each other. Shape defined by what contains liquid (i.e. Pitcher, shoreline, etc) Gas - Atoms moving rapidly and far apart. Continue to expand apart unless contained.

Why must a measurement include both a number and units?

number gives you quantity. Unit gives you comparable units

What separates substances based on their boiling points?

Distillation.

``` The density of copper is 8.92 g/ml. The mass of a piece of copper that has a 10 ml volume is A. 89.2 g B. 892 g C. 8.9 x10^2 g D. .892 g E. None of the above ```

A. 89.2 g

``` A chemical combination of two or more elements is called a(n) A. Solution B. Compound C. Element D. Period ```

B. Compound

T/F | A gas takes on both the shape and volume of its container

True. Think balloon.

The formula for density is D=M/V ``` If a 100g sample of metal has a volume of 5.18ml what is the density of the metal? A. 5 g/ml B. 0.518 g/ml C. 19.3 g/ml D. 1.93 g/ml E. None of the above ```

C. 19.3 g/ml

The new substances produced in a chemical reaction are called ______________?

Products

T/F | All matter that we encounter in everyday life exists in one of three physical forms

True. Solid - liquid - gas

Which of these are physical changes and which are chemical changes? Boil. Burn. Condense. Corrode. Crumple. Crush. Explode Ferment. Freeze. Grind. Melt. Oxidize. Rot. Rust. Tarnish. Vaporize.

Physical. - Boil, Condense, Crush, Crumple, Freeze, Grind, Melt, and Vaporize Chemical. - Burn, Corrode, Explode, Ferment, Oxidize, Rot, Rust, Tarnish

``` Which of the following is an ion? A. O2- B. C C HCI D. LI-3 ```

A. O2

``` Which property describes h how much energy must be added to an atom to remove an outermost electron? A. Atomic radius B. Electronegativity C. Ionic radius D. Ionization energy ```

D. Ionization energy

How do you count valence electrons? | What impact does it have on Bohr diagrams?

2/8/18. =2n^2 | Determines how many electrons are in the outer ring

Define group/family/column

Group/ Family - 18 columns of elements in periodic table

T/F | Ionic radius of both positive and negative ions gets larger as you move down a group

True.

T/F | The noble gases possess very high ionization energies because of their full valence shells.

True. All group 18 elements have full valence shells. 2/10/18/26/34/42 etc helium has the highest ionization energy of all the elements. Shell of 2 electrons

What are the noble gases?

- group.18 | - Extremely unreactice

Define period and row

Period/Row. - 7 rows of elements in periodic table

Why are ionic radii generally larger for group 15 than for group 17? A. Atoms in group 15 are larger than atoms in group 17 B. Atoms in group 15 have more protons than atoms in group 17 C. Ions of group 15 have greater negative charge than ions of group 17 atoms D. Atoms in group 15 are generally more electronegative than atoms in group 17

C. Ions of group 15 have greater negative charge than ions of group 17 atoms

``` Elements with the physical and chemical properties of both metals and non-metals are A. Radioactive metals B. Transition metals C. Metals or semi-metals D. Gaseous metals ```

C. Metals or semi-metals

What are the properties of halogens?

- group 17 | - Usually found in compounds

What is the atomic radius?

atomic radius is one-half the distance between the nuclei of two atoms - decreases from left to right within a period. increase in the number of protons draws electrons in - increases from top to bottom within a group

What is the ionic radius?

Positive ions (missing electron) - smaller. Drawn into + center Negative ions (added electron) - larger. Push away from + center

Which correctly describes elements in the same family? A. Same number of valence electrons B. Electrons in the same outermost energy level C. Same atomic radius D. Must be in same state of matter

A. Same number of valence electrons

T/F | The periodic table organizes the elements by atomic mass

False | By atomic number

What are the properties of alkali metals?

- group 1 - very reactive - usually found in compounds (i.e. Table salt,)

T/F | The periodic table organizes elements into periods(columns) and groups our families (rows)

False periods - rows groups or families- columns

What are periodic trends? | Electronic summary assignment & PP notes

Period and group trends in atomic radii are related to electron configuration ??? As atomic radius grows - # protons grows - # electrons grows - so more rings 2/10/18/26 etc

What is ionization energy?

Energy used to hold onto electrons -higher ionization energy holds electrons more tightly - higher ionization energy less likely to lose an electron and develop (+) charge - ionization energy generally increases from left to right. This is due to valence shell stability. - ionization energy within a group generally decreases from top to bottom. - noble gases possess very high ionization energies because of their full valence shells - helium has the highest ionization energy

What is the Octet Rule?

Elements will try to stabilize by getting 8 electrons in the outer ring Elements on right side of periodic table tend to gain electrons and form (-) electrons - anions Elements on left side of periodic table tend to lose electrons and form (+) ions- cations

What are Lewis structures?

Dots around element symbol show number of valence electrons. Max of 8

In the periodic table what is the general location of the Metals Metalloids Non-metals

Metals - left side Metalloids - middle diagonal Non-metals - upper right

``` Which family contains the halogen family of elements? A. 1 B. 2 C. 17 D. 18 ```

C. 17

The correct match of elements to group is: A-alkali metals B-halogens 1- group 18. 2- group 1 C-alkaline earth metals D- noble gases. 3- group 2. 4- group 17 A. A-1. B-3. C-2. D-4 B. A-3 B-2. C-1. D-4 C. A-2 B-4. C-3. D-1 D. A-4. B-1. C-2. D-3

C. A-2 B-4. C-3. D-1

``` Most atoms that form ions become more stable by following the___________ rule, which means there will be _____ electrons in its outermost layer A. Triplet- 3 B. Octet- 4 C. Duet - 2 D. Octet - 8 ```

D. Octet - 8

``` Elements in the same group of the periodic table have the same_______? A. Number of valence electrons B. Physical properties C. Number of electrons D. Electron configuration ```

A. Number of valence electrons

How is the periodic table organized? | How does atomic number change as you move around in the table (L/R and up/down)?

Rows - increasing atomic number as you move left to right Columns - increasing atomic number as you move down

``` Which group is composed entirely of nonmetals? A. 1 B. 13 C. 15 D. 18 ```

D. 18. Noble gases

``` Where on the periodic table would you expect to find the smallest atoms? A. Upper left B. Upper right C. Lower left D. Lower right ```

B. Upper right

``` Which group contains the most unattractive and stable elements? A. 1 B. 2 C. 17 D. 18 ```

A cation is an element which has gained an electron?

False. Lost (-) electron and is now(+)

T/F | Generally, atomic radius gets smaller as you move right on the periodic chart

True.

T/F | Nitrogen has the highest ionization energy of all the elements.

False | helium has the highest ionization energy of all the elements.

What is electronegativity?

Indicates relative ability of element atoms to ATTRACT electrons in a chemical bond. ElectroNEGATIVITY Decreases as you go Down the table Raises as you go Right in the table Noble gases are 0

``` An atoms ability to attract electrons is its A. electronegativity B. Heat of reaction C. Ionization energy D. Heat of formation ```

A. electronegativity

Is ionic radius smaller or larger for a positive ion?

Smaller. + charge. Drawn into + center

What is an ion? When would it have a positive charge? When would it have a negative charge?

Ion is an atom with either one extra/one less electron than the base element? One less - positive charge- cation One more - negative charge - anion

For the elements in Period 3, as you move right in the periodic table, both atomic number and electronegativity increase. T/F

True

``` On the modern periodic table, metalloids are found only in _________. A. Groups. 3-5 B. Groups 13-17 C. Group 18 D. Groups 1-2 ```

B. Groups 13-17

Atoms with large ionization energy values are _________. A. More likely to form positive ions B. Less likely to form positive ions C. Most likely to lose their outer electrons D. Lacking valence electrons

B. Less likely to form positive ions

What did Ernest Rutherford discover? How did he make this discovery?

Rutherford - small positive nucleus in atoms - repels positive alpha particles - used gold foil and shot alpha particles at it - nuclear atomic model

What are the charges in these types of radiation? Alpha Beta Gamma

Alpha 2+ Beta. 1(-) Gamma. No charge

``` What is the primary factor in determining an atom's stability? A. neutron to proton ratio B. protron to electron ratio C. neutron to electron ratio D. alpha particle to beta particle ratio ```

A. neutron to proton ratio

What is the lowest state of an atom called? A. ground state B. excited state C. California D. state of flux

Ground state. 2n^2 or only 2 electrons

Discuss how radioactive atoms gain stability

Radioactive decay - emit alpha & beta particles until neutron to protron ratio allows stability

Explain radioactive decay

- Spontaneous process | - unstable nuclei lose energy by emitting radiation

What did John Dalton discover? How did he discover it?

Dalton - elements can only combine atomically when they are in fixed ratios - did numerous experiments to measure chemical reactions and determined mass ratios

What determines the stability of an atom?

Neutron to proton ratio

Classify each of the following as a chemical reaction, nuclear reaction or neither A. Thorium emits a beta particle B. Two atoms share electrons to form a bond C. A sample of pure sulfur emits heat energy as it slowly cools D. A piece of iron rusts

A. Beta particles - radioactive B. Ionic bond - chemical C. Neither. Change of state only D. Rust - chemical

Iodine-131 undergoes radioactive decay and forms an isotope with 54 protons and 77 neutrons. What type of decay occurs in this isotype? How can you tell?

Gamma rays?? No change in charge?

Why are some atoms radioactive?

neutron to protron ratio is either too little or too much

What is meant by nuclear stability?

Atoms with either too many or too few neutrons lose energy through decay to form a stable nucleus where neutrons = protons

What are alpha and beta decay?

``` Alpha - least harmful. Stopped by paper or clothing - 2 protons/2 neutrons. Charge of +2 - appreciable mass Beta - more harmful. Stopped by metal foil - high speed electrons - found/named by Rutherford - violates law of conservation of energy ```

What is the difference between radioactivity and nuclear reactions?

Radioactivity - substances spontaneously emit radiation Nuclear reactions - involve change in the nucleus of the atom

Draw and discuss the Bohr model

If neutral - Protons = Atomic # = Electrons Neutrons may be different. Protons & Neutrons in nucleus of picture Electrons orbit nucleus in rings. Each ring holds 2n^2. Ring 1 -2 Ring 2 - 8 Ring 3 - 18

T/F | Nuclear reactions involve changes in the electrons.

False NUCLEAR reactions involve changes in the NUCLEUS

What particles account for most of an atom's mass?

protons and neutrons

``` What is the maximum number of electrons that can be present in each principal energy level? A. n B. n^2 C. 2n D. 2n^2 ```

D. 2n^2

What is gamma radiation?

- Most harmful radiation as it can penetrate lead or concrete. - high energy radiation. Kills living cells - No mass, neutral charge

T/F | Chemical reactions involve changes in the number of electrons

True. | Pulled away and combined with other elements.

Element Q has isotopes Q248, Q252, and Q259. If the atomic mass of element Q is 258.63, which isotope is most abundant? A. Q248 B. Q252 C. Q259 D. Cannot be determined with the given information

C. Q259. skews average up

T/F | Number of protons AND number of neutrons remain the same for all isotopes of the same element

False. | Change in neutrons is what makes it an isotope

What did J.J. Thomson discover? How did he discover it?

JJ Thomson - electron. Negatively charged - used ray tubes to ID electrons. - determined ratio of electron mass to its charge - Plum pudding model

What is the basic structure of an atom? | What are the differences in a neutral atom, ion and isotope?

Atom - protons & neutrons in nucleus. Electrons orbiting nucleus Neutron - large, no charge Proton - large, positive charge Electron - small, negative charge Neutral - protons = electrons. No charge Ion = less or extra electrons resulting in + or (-) charge Isotope - extra neutron increasing atomic mass

T/F | The number of protons AND the mass number determine the type of atom

True. As # of protons change the element changes. Change in mass number indicates change in either protons or neutrons which also changes

An element has three naturally occurring isotopes. What additional information do you need to compute it's atomic mass?

The abundance of each isotope

11th Chemistry- Fall final review Flashcards

(139 cards)