Chemistry Chapter 6: The Periodic Table

A few elements, such as gold and copper, have been known for thousands of years- since ancient times. Yet only about ___ had been identified by the year 1700. As more were discovered, chemists realized they needed a way to _______ the elements.

13, organize

In electronegativity, they share the share, but how equally do they share it? (#3. trends in electronegativity)

An element with a big electronegativity means it pulls the electron towards itself strongly!

Russian chemist and teacher

Dmitri Mendeleev

Energy Levels and Shielding have an effect on the _______ ( ↓↑) (what do they influence)

Group

also forms bases with water; do not dissolve well, hence "earth metals" (groups of elements-- family names)

Group 2A- Alkaline Earth Metals

means "Salt-forming"

Group 7A- Halogens

forms a "base" (or alkali) when reacting with water (not just dissolved) ( groups of elements- family names)

Group IA--> Alkali Metals

(1913) British physicist, arranged elements according to increasing Atomic number, arrangement is still used today, symbol, atomic number, and mass are basic items included

Henry Moseley, created the better periodic table

Who created the better arrangement of the periodic table?

Henry Moseley.

(mid 1800s- 70 elements known to exist) arranged elements in order of increasing Atomic Mass. first "Periodic Table" He left ________ for undiscovered elements. (when they were discovered, he made good predictions) What six elements did Mendeleev have problems with?

Mendeleev's Periodic Table, blanks, Co and Ni, Ar and K, Te, and I

the elements in Group 8A (also called Group 18 or 0), previously called "inert gases" because the rarely part in a reaction; very stable= don't react have an electron configuration that has the outer "s" and "p" sub levels completely full

Noble Gases

Elements can be sorted into 4 different groupings based on their electron configurations: 1) _________ Gases 2) ___________ Elements 3) ___________ Metals 4) _____ Transition Metals

Noble, representative, Transition, Inner

in Groups 1A through 7A display wide range of properties, why a good "representative" some are metals, nonmetals, or metalloids, some are solid, others are gases, others are liquids their outer "s" and "p" electron configurations are not filled

Representative Elements

What factors determine IE? ________ effect Greater distance from the nucleus _____ IE. The greater the ______ charge, the ______ IE. Filled and half-filled orbitals have lower energy, so achieving them is easier, lower IE.

Shielding, decreases, nuclear, greater,

The periodic table displays the _______ and _______ of the elements, along with information about the structure of their atoms: Atomic _______ and Atomic _______ Black Symbol= ______ Red= _______ Blue = _______ (squares in the periodic table)

Symbols, Names, number, mass,solid, gas, liquid

How did Henry Moseley arrange elements?

according to increasing atomic number

negative ions

anions

positively charged particle

cation

more charge pulls electrons in closer. (+ and - attract each other) (all periodic table trends, factor #2)

charge on nucleus (# protons)

Chlorine will gain one ______. Protons (17) no longer equals the _____ (18), so a charge of -1. Cl¹⁻ is renamed a "________ ion"

electron, chloride

tendency for an atom to attract electrons to itself when it is chemically combined with another element (#3. trends in electronegativity)

electronegativity

higher energy levels are further away from the nucleus (all periodic table trends, factor #1)

energy level

All periodic table trends are influenced by three factors. What are those three factors

energy level, charge on nucleus (# protons), shielding effect (blocking effect?)

What is the third ionization energy required to do?

energy required to remove a third electron. greater than 1st or 2nd ionization energy.

vertical columns= Group ( or ________) What do vertical columns have?

family, similar physical and chemical properties

Nonmetals tend to _____ one or more electrons

gain

Non-metals form ions by ______ electrons to achieve noble gas configuration. They end up with the configuration of the noble gas after them (configurations of ions)

gaining

What are examples of transition metals?

gold, copper, silver

How did Dmitri Mendeleev arrange his elements?

in order of increasing atomic mass

located below the main body of the table, in 2 horizontal rows, electron configuration has the outer "s" sub level full, and is now filling the "f" sub level. formerly called "rare-earth" elements

inner transition metals

some compounds are composed of particles. atom (or groups of atoms) that has a positive or negative charge

ion

Metals are at the ___ of the table and they let their electrons ___ easily. Metals have ____ electronegativity. At the __ end are the nonmetals, and they want ____ electrons and they try to take away from others. Nonmetals have ____ electronegativity. (electronegativity period trend)

left, go, low, right, more, high

Metals tend to ____ electrons from their outer energy level. (ions)

lose

heavy, stair-step line, border the line- 2 sides, properties are intermediate between metals and nonmetals

metalloids

electrical conductors, have luster, ductile, malleable

metals

What are three classes of elements? (areas of the periodic table)

metals, nonmetals, metalloids

Atoms are ____ because the number of protons equals electrons. Positive and negative ions are formed when electrons are ___________ (lost or gained) between atoms (ions)

neutral, transferred

generally brittle and non-lustrous, poor conductors of heat and electricity. Some _____ are gases (O2, N2, Cl2); some are brittle solids (S); one is a fuming dark red liquid (Br)

nonmetals

Nuclear charge has an effect on a _________ (↔) (what do they influence)

period

when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

periodic law

Horizontal rows= _______ 7 ___________ (periodic laws)

periods

Chemists used the _____ of elements to sort them into groups.

properties

Sodium loses one: there are now more _____ (11) than electrons (10), and a positively charged particle is formed= "______". charge is written as a number followed by a plus sign: Na¹⁺. Now named a "______ ion"

protons, cation, sodium

Elements in the 1A-7A Groups are called the __________ elements. outer "s" or "p" filling

representative elements

What is the second ionization energy required to do?

required to remove the second electron, always greater than first IE.

Iso means "the _____" Isoelectronic ions have the same _______ of electrons. Al3+ Mg2+ Na1+ Ne F1- O2- and N3- all have 10 electrons all have the same configuration: 1s22s22p6 (which is the noble gas: neon) (size of isoelectronic ions)

same, number

in the "B" columns of the periodic table. electron configuration has the outer "s" sub level full and is now filling the "d" sub level "transition" between the metal area and the nonmetal area

transition metals

first problem: where do you start measuring from? What does the electron cloud not have? overcome this by measuring more than one atom at a time.

trends in atomic size, definite edge,

In 1829, J.W. Dobereiner arranged elements into ______ (groups of 3 elements with similar properties), one element in each triad had properties intermediate of the other two elements.

triads

groups of 3 elements with similar properties

triads