Chapter 4 Test

Lanthanides ●They form a ___ oxidation number in compounds as they tend to lose the ___ electrons ●Lanthanides are about as reactive as ___ . ●used in TV phosphors ●used in microwave technology ●used in high-strength permanent magnets ●used in improved types of lasers.

+3 6s² 5d¹ Alkaline earth metals

alkali metals ●group ___ ●___valence electron ●most reactive metal family ●react with ___ to form alkaline (basic) solutions ●soft metals ●lower in density which generally ___ as you go down a group ●lose ___ e- to form ions with a ___ charge

1 1 water increases 1 +1

Noble Gases ●group ___ ●___ valence electrons except ___ ●do not form ions ●are very stable because they have a full valence level of electrons ●The noble gases were once called ___ gases because they were thought to be completely ___ . But in 1962, chemists were able to get xenon to react, making the compound XePtF₆. In 1979, chemists were able to form the first xenon-carbon bonds. ●Helium only has ___ valence electrons but it is very stable because those valence electrons fill up the entire first energy level.

18 8 helium inert unreactive 2

Alkaline Earth Metals ●group ___ ●___ valence electrons ●also react with water to form an ___ solution. ●They are pretty reactive though not as reactive as alkali metals. ●They are ___ and have ___ melting points than alkali metals. ●lose ___ electrons when forming compounds to form ions with a ___ charge

2 2 Alkaline Harder higher 2 +2

Rank the following in order of increasing atomic radii. Ca Ca⁺² I I⁻ Ar Xe

3 1 5 6 2 4

How many valence electrons do the following atoms have? Br Sr Pb Te Ag He Xe What oxidation number (charge associated with an atom in a compound) would the following atoms be expected to have? Br Sr Pb S Al Li N

7 2 4 6 2 2 8 -1 +2 +4 -2 +3 +1 -3

Actinides ●elements ___ to ___ ●___ sublevel filling ●tend to lose ___ electrons when forming compounds to form ions with a ___ charge. ●The actinides are unique in that their nuclear structures are more important than their electron configurations because their nuclei are unstable and spontaneously break apart. All are ___ . ●The best-known member of this family is ___ .

90 to 103 5f 3 +3 Radioactive Uranium

Label the following elements as member of the following families. Chlorine Radon Selenium Iron Calcium Potassium Mendelevium Promethium

Halogens Noble gases Chalcogens Transition metals Alkaline earth metals Alkali metals Actinides Lanthanides

Helium and beryllium both have two electrons in their valence shell. Why are their properties so different?

Helium's valence shell is full with two electrons and beryllium's is not.

THINK ABOUT WHAT GROUPING THE ELEMENTS ARE AND THEN FILL IN THE LETTER! Do problem 1 on 4-2.

THINK ABOUT WHAT GROUPING THE ELEMENTS ARE AND THEN FILL IN THE LETTER! Do problem 1 on 4-2.

What electrons do you lose in a compound? Write the short form electron configuration of: Al Al⁺³ Cl Cl⁻ Zn Zn⁺²

Valence electrons. [Ne]3s²3p¹ [He]2s²2p⁶ [Ne]3s²3p⁵ [Ne]3s²3p⁶ [Ar]4s²3d¹⁰ [Ar]3d¹⁰

Write the electron configurations for the following elements. Use the shortcut. How many dots in the dot diagram for each element? Indium rhenium samarium argon

[Kr]5s²4d¹⁰5p¹ [Xe]6s²5d¹4f¹⁴5d⁴ [Xe]6s²5d¹4f⁵ [Ne]3s²3p⁶ 3 2 2 8

As you move from top to bottom in a group on the periodic table the number of occupied energy levels As you move from top to bottom in a group on the periodic table the electron shielding effect As you move from top to bottom in a group on the periodic table the effective nuclear charge As you move from top to bottom in a group on the periodic table the electron affinity As you move from top to bottom in a group on the periodic table the ionization energy As you move from top to bottom in a group on the periodic table the atomic radii

increases. increases remains about the same. decreases. decreases. increases.

Given each of the following properties, label the property as that of a a. metal, b. nonmetal, or c. metalloid Lustrous Left side of the periodic table Semiconductors Right side of the stair-step line Brittle solids Malleable Insulators Conductors Along the staircase most elements belong to this category

metal metal metalloid nonmetal nonmetal metal nonmetal metal metalloid metal

fill in the blanks below. The ___ are the most unreactive because they have a ___ ___ ___ of electrons. Groups among the main-group elements display similar chemical behavior because they have the same number of ___ ___ . A mixture of a metal and one or more other elements that can be separated by physical means is called a(n) ___ . ___ is the most common element in the universe. Because it consists of just one proton and one electron, it behaves unlike any other element. If an element can be found in nature in its elemental form you can be sure it is ___ and less ___ . Elements that are too Elements that are too ___ are only found in nature in compounds. When an atom gains or loses electrons it becomes ___ . The main-group elements form ions that are ___ with a noble gas.

noble gases full valence level valence electrons alloy hydrogen stable reactive reactive charged isoelectric

___ : A predictable change in a particular direction. ___: A vague, relative distance that is about the distance from the nucleus to the densest part of the outer layer in the cloud. There is no clear cut edge in the cloud and the cloud fluctuates with chemical and physical state making measurement difficult. ___ : The reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons. ___ : The net positive charge that the outer valence electrons experience from the nucleus which is affected by the number of shielding electrons that surround the nucleus. ___ : The energy required to remove an electron from an atom or ion. ___ : half the distance from center to center of two like atoms that are bonded together which can change slightly depending on what atoms are involved. ___ : The energy released when a neutral atom gains an electron. ___ : A measure of the ability of an atom in a chemical compound to attract electrons ___ : The force of attraction between opposite charges or repulsion between like charges.

trend atomic radius electron shielding effective nuclear charge ionization energy bond radius electron affinity electronegativity electrostatic force