Unit 3 Review!

Section 6.1

_________________created the first periodic table which was arranged according to atomic ___________. Dmitri Mendeleev Mass Pudding

In the modern periodic table, elements are ordered by atomic __________. ______________ was the first scientist to order them this way. Number Henry Moseley Wedding cake

______________ law says that when the elements are placed in order by atomic number there is a periodic repetition of their chemical and physical properties. Periodic HUGE PIZZA!!!!!

_______________ determine the identity of an element and the atomic number. However, _______________ determine the chemical behavior. Protons Electrons

Chapter 7 Study your notes for metals, nonmetals, and metalloids. Be sure you could identify elements of these regions and describe the properties of these regions.

Groups _____________________ are known as the representative elements because… 1A-8A They possess a wide range of properties

The valence electrons of representative elements are in the ____ and ____ orbitals

Group 1 elements Group 1: called the _____________ metals. They have electron configurations ending in ________. Alkali s1

Properties of Group 1 elements include: Stored in _________ due to extreme reactivity with oxygen (contains the most reactive metal) Form __________ (charge) ions. Consistency is ________. Good conductors of _____ and _______ oil 1+ Cold Butter Heat Electricity

Group 2 elements Group 2: called the ________metals. Their electron configurations end in ______________. Alkaline Earth s2

Properties of Group 2 elements include: Shiny generally _____________ solids. ________and denser than alkali metals Less ______________ than alkali metals. Form __________________ (charge) ions. Harder reactive 2+

Transition The ____________________ metals are a large group of elements in the middle of the periodic table. Properties of these elements include:

Properties of Transition metals include: Transition metals are also known as the _____-block elements General properties (similar to other metals) are… Most transition metals are _______ solids with ________ melting points. Transition metal unpaired d-electrons have the ability to move into the ________ level. Because of this, many transition metals can form several different charged ions. Transition metals contain the ________________ metals (like gold & silver) The more unpaired electrons in the d-level, the ….. Electrical conductivity, lustrous, malleable Hard High valence precious The greater the hardness and the higher the melting and boiling point

Inner Transition The _______________________ metals are also known as the f-block. The top row is called the _____________ and the bottom row the ________________. This group contains synthetic and radioactive metals. Lanthanides Actinides

Group 17 Group 17 is the ______________________ family. Their electron configurations end in _________. Halogen P5

Properties of elements in group 17: Very ___________ nonmetals – they are always in compounds, never alone. Halogens tend to gain or share 1 electron because they have ________ valence electrons. Form ________ (charge) ions. The most reactive nonmetal, __________________, is in this family. Exist in all 3 ____________ of matter (s, l, g) React readily with ____________, especially alkali, to produce salts. (halogen = salt former) reactive 7 1- Fluorine States Metals

Group 18 elements Group 18 elements are the _______ gases. Their electron configurations end in _______. Noble P6

Properties of group 18 elements include: Inert or _________ gases because…. Do not form ions or bonds. Noble Full outer shell of e-

The reason any group has similar properties is because they have the same number of __________. Valence e-

Hydrogen: only element considered to be a chemical family all by itself. Hydrogen is placed in group 1 because it has _________ valence electron. Hydrogen has properties of group 1 and group ___________. The universe is _____% hydrogen by mass. 1 7a 90

Hydrogen acts like a metal when….. Hydrogen acts like a nonmetal when… It loses an electron It gains an electron

Match the family name to the location: d b ______ lanthanides and actinides (inner transition metals) _______alkali and alkaline earth metals _______halogen _______noble gases _______transition metals C A D E B Label the s, p, d and f blocks on the periodic table above c

An element has the electron configuration [Ne]3s23p5 An element has the electron configuration [Ne]3s23p5. What family is this element in? _______ What group? ________ What period? ____________ What is this element? _______ Halogens Halogens 3 Chlorine

Match the element with the family to which it belongs: Neon Magnesium Fluorine Silver Potassium Iron a=Alkaline Metals b=Alkaline Earth Metals c=Transition Metals d=Halogens e=Noble Gasses

A = alkali metals B = alkaline-earth metals C = transition metals D = halogens E = noble gases The __________________ have electron configurations that end in s2. The _______________________ are soft enough to cut with a knife. The ______________________ contain the precious metals. The ______________________ are the most reactive nonmetals. The _______________ are stable and unreactive due to their full s and p orbitals. The ___________________ have a name that means salt-former. B A C D E D

Review your notes and know why! As you move down a group on the periodic table, atomic radii generally ____________ and across a period it generally _______________. Review your notes and know why! Increases Decreases

Define ionization energy. Energy needed to remove an e- from an atom What did one ion say to the other ion? I got my ion you!

Review your notes to explain why. Ionization energy generally __________ across a period and ______________ down a group. Review your notes to explain why. Increases Decreases A small furry mammal walks into a bar and orders a drink. The bartender says, "Sorry, our maximum occupancy is only 6.00 x 1023. We can't serve a mole."

Which family of elements has the highest ionization energy Noble Gases

Know Why! Review your notes. The tendency for an atom to attract electrons of another atom is called ______________. It generally ____________ as you move left to right across a period and _____________ down a group. Know Why! Review your notes. Electronegativity Increases Decreases

Circle the atom with the LARGER atomic radius cesium potassium sodium aluminum cesium helium

Circle the atom with the LARGER ionization energy Boron oxygen nitrogen phosphorous Chlorine selenium

Circle the atom with the LARGER electronegativity calcium potassium fluorine bromine phosphorus oxygen