Chemistry Ch. 5

by increasing atomic numbers

After many years of study and revisions, how is the periodic table arranged today?

Cations (less electrons) tend to be smaller than anions (more electrons) tend to be larger

Are cations or anions smaller than neutral atoms?

Ne

Neon

1. metallic luster 2. crumbly, brittle solids 3. conduct electricity better than nonmetals but not as well as metals

What are some characteristics of metalloids?

1.generally gases or soft, crumbly solids 2. Bromine is a liquid 3. Diamond is the hardest known natural substance 4. generally poor conductors of thermal energy and electrical current

What are some characteristics of nonmetals?

Group 7A, because it will add one electron instead of loosing 7 electrons

Which group 1A or 7A has a higher electron affinity?

Group 7A

Which group 1A or 7A has a higher ionization energy?

because the strength with which protons in the nucleus attract the outer-shell electrons increases

Why does the ionization energies generally increase from left to right across a period?

Antoine Lavoisier

a French chemist that used the word "element"

Dmitri Mendeleev

a Russian chemist who established the structure of the modern periodic table, but arranged the elements by their atomic mass and left blanks for elements he believed were not yet discovered; he also included transition elements

International Union of Pure and Applied Chemistry (IUPAC)

a convention of numbering the columns from 1 through 18; each family is uniquely identified

periodic table

a description of how elements differ from one another

paramagnetic

a property of materials that are weakly attracted by a magnetic field because of unpaired electrons

Al

aluminum

Henry Moseley

an English physicist who found the elements are related to the number of protons in the nucleus (atomic number)

B

boron

F

fluorine

Hg

mercury

Mo

molybdenum

Ni

nickel

N

nitrogen

atomic number

the number of protons

it decreases

Does the atomic radius increase or decrease as you move across the periodic table from left to right?

it increases, because another principal energy level is added

Does the atomic radius increase or decrease as you move down a column in the periodic table?

left to right

Does the electronegativity of the elements increase as you move from left to right on the periodic table or right to left?

1. element's atomic number 2. element's name 3. element's symbol 4. element's atomic mass 5. element's electron configuration 6. element's physical properties

On the periodic table, for each element, what information is given?

1. has one electron 2. reacts like other Group IA elements 3. also similar to Group 7A elements because it only needs one more electron to fill its outer shell 4. combines with many elements to form compounds 5. forms, with carbon, hydrocarbons

What are some chemical properties of Hydrogen?

1. colorless, odorless, tasteless 2. diatomic molecule

What are some physical properties of Hydrogen?

1. very reactive 2. typically form cations (+1) 3. conduct heat and electricity well 4. metallic luster 5. low densities and soft 6. must be stored in oil

What are some properties of alkali metals?

1. metallic luster 2. crystalline and brittle 3. lower ductility and malleability than metals 4. semiconductors

What are some properties of metalloids?

1. solid at room temperature 2. denser, harder, and have higher melting points than the alkali metals 3. form cations (+2) 4. malleable 5. typically donate their 2 valence electrons

What are some properties of the alkaline-earth metals?

1. paramagnetic 2. when cut, bright and silvery 3. usually give up their 2 valence electrons 4. actinide series are radioactive and used in nuclear power plants

What are some properties of the inner transition metals?

1. high densities 2. hard, tough, and strong 3. shiny luster 4. conduct heat and electricity well 5. ductile and malleable 6. 2/3 are native minerals

What are some properties of the transition metals?

1. used to manufacture ammonia used in crop fertilizers 2. the space program for rocket fuel 3. hydrogenation (forms semi solid fats) 4. in the future, fuel cell technology

What are some uses of hydrogen?

1. solid 2. lustrous (shiny) 3. malleable (shapeable) 4. ductile 5. good conductors of heat and electricity (some exceptions: mercury is a liquid and manganese is a brittle solid)

What are the characteristics of most metals?

post-transition metals

What are the metals in Groups 13-16?

transition metals

What are the metals in groups 3-12?

oxygen

What element is a member of both Period 2 and Group 16 (6A)?

calcium

What element is a member of both Period 4 and Group 2 (2A)?

indium

What element is a member of both Period 5 and Group 13 (3A)? use pgs. 108-109

The Boron Family (3 valence electrons)

What is the name of Group 13 (3A)?

The Carbon Family (4 valence electrons)

What is the name of Group 14 (4A)?

The Nitrogen Family (5 valence electrons)

What is the name of Group 15 (5A)?

The Oxygen Family (6 valence electrons)

What is the name of Group 16 (6A)?

The Halogen Family (7 valence electrons)

What is the name of Group 17 (7A)?

The Noble Gas Family (8 valence electrons)

What is the name of Group 18 (8A)?

alkali metals

What is the name of Group 1A?

alkaline-earth metals

What is the name of Group 2A?

Period 4 and Group 1 (1A)

What period and family is the element potassium found in?

Period 3 and Group 16 (6A)

What period and family is the element with the atomic mass of 32.07u found in?

Period 3 and Group 17 (7A)

What period and family is the element with the atomic number 17 in?

They do not except unless under unusual conditions of pressure and temperature.

When do noble gases react with other elements?

1. small amounts in the earth's atmosphere 2. large quantities are contained in gaseous byproducts of fuel and other refining processes, separated by electrolysis 3. from heated coke (impure carbon obtained from coal)

Where is hydrogen found?

group or family

a vertical column of elements on the periodic table; have similar physical and chemical properties due to their electron configuration

Ar

argon

metalloids

around the stair-step line between the cells in Groups 13-17

As

arsenic

Ba

barium

Be

beryllium

Br

bromine

Ca

calcium

C

carbon

Cs

cesium

Cl

chlorine

Cr

chromium

Co

cobalt

physical properties

colors and icons give information about the physical properties of he element, such as whether it is a metal or nonmetal and whether it is radioactive

hydrocarbons

compounds formed when hydrogen atoms and carbon atoms form compounds

Cu

copper

John Dalton

documented a list of sixty elements

representative groups

elements in the s and p blocks of the periodic table; designated with A suffixes in the North American Convention Periodic Table

native minerals

elements that are found as pure solids in nature

transition elements

elements that do not fit into the major families, but they all have similar chemical and physical characteristics

transuranium elements

elements with atomic numbers greater than 92 (Uranium's atomic number); except for neptunium and plutonium, all are products of artificial processes in nuclear reactors or bomb explosions

actinide series

fits into the table after actinium; placed at the bottom of the table; their interior f sublevel electrons are added with increasing atomic number

Ga

gallium

Ge

germanium

Au

gold

North American Convention Periodic Table

has a combination of Arabic numerals and letters that are placed above each column to indicate the valence electron structure of the elements in each column

symbol

has one, two, or three letters; most prominent item in the cell

He

helium

periods or series

horizontal rows of elements; indicates the highest principal energy level that electrons occupy in ground-state atoms

H

hydrogen

lanthanide and actinide series

inner transition metals

I

iodine

Fe

iron

Kr

krypton

Pb

lead

Li

lithium

Mg

magnesium

Mn

manganese

metals

on the left side and the middle of the periodic table

nonmetals

on the right side of the periodic table; separated from the metals by a stair-step line

John Newlands

organized elements by their atomic mass; used octaves, which was not well received

O

oxygen

P

phosphorous

lanthanide series

placed at the bottom of the table; their interior f sublevel electrons are added with increasing atomic number; fits in the table immediately after the element lanthanum

Pt

platinum

Pu

plutonium

K

potassium

Ra

radium

Rn

radon

Rb

rubidium

Se

selenium

Si

silicon

Ag

silver

Na

sodium

periodic law

states that the properties of elements vary with their atomic numbers in a periodic way; formulated by Mendeleev and later revised by Moseley

Sr

strontium

S

sulfur

electron affinity

the amount of energy required to "add" an electron to a neutral atom to form a negative ion, or anion; opposite of ionization energy; depends on the size of the atom and the fullness of the highest energy sublevels; the energies becomes larger from left to right along a period

atomic radius

the distance from the center of an atom's nucleus to its outermost electron; determined by the electron cloud that surrounds the atom; the measure of an atom's size

metalloids

the elements immediately adjacent to the stair-step line; share properties of metals and nonmetals

hydrogen

the lightest element and the most abundant in the entire universe; often considered a family by itself

electronegativity

the measure of the attraction between the nucleus and valence electrons; the atom's ability to attract and hold electrons in a "molecule"; plays a central role in predicting how atoms chemically combine with each other

first ionization energy

the minimum energy required to remove the first electron from its outermost shell to make a cation; how easily electrons are "taken away" from atoms to form cations; generally increases from left to right within a period and decreases from top to bottom within a group

electron configuration

the number and location of electrons in each occupied energy level in the neutral atom; listed below the atomic mass

descriptive chemistry

the study of elements and the compounds they form

atomic mass

the weighted average located under the symbol

Sn

tin

Ti

titanium

U

uranium

Johann Dobereiner

used triads (groups of three elements with similar properties); his method was a step that lead to periodicity

sulfides

when certain metals combine with sulfur to form compounds

oxides

when oxygen combines with other elements to form a compound

periodicity

when some measurable property repeats on a regular basis in a sequential list or time sequence

Xe

xenon

Zn

zinc