Chemistry Chapter 6

Family Names

-Alkali metals (most reactive) -Alkaline earth metals -Halogens -Noble gases

Sodium

-Bluish-white, shiny metal -Unworkable -Can't be melted and isn't like other metals

Metals

-Higher melting & boiling points-mainly solids -Lustrous (shiny and smooth) -Good conductors of energy -Malleable (can be hammered into sheets) -Ductile (can be pulled or squeezed into wires)

Chlorine

-Highly reactive element -It undergoes reaction with a wide variety of elements and compounds -Gas -Greenish yellow -Very toxic -Suffocating smell

Non-Metals

-Lower melting & boiling points for all states of matter -Dull -Poor conductors of heat & electricity -Brittle (not malleable or ductile)

Sulfur

-Pale yellow -Solid -Odorless -Tasteless -Very chemically reactive when heated

Uranium

-Silvery, shiny metal -Ductile -Malleable -Highly reactive

Osmium

-Silvery-white metal -Waxy -Soft enough to be cut by a knife -High reactivity

Barium

-Solid -Alkali Earth Metal -When pure, it is silvery white like lead -Never found free in nature, found only in combination with other elements because it reacts with Oxygen in the air

Calcium

-Solid -Hard -Silver/ White/ Gray -Burns in oxygen with strong heating -Reacts with dilute hydrochloride acid to give hydrogen -Reactions with dilute calcium and acids forms calcium chloride -Does not react in water

Ionization energy

-Within a family, the trend is decreasing (because less energy is required to remove electrons from the larger atoms) -Across a period, the trend is increasing (because more energy is required to overcome the stronger nuclear forces on electrons in the smaller atoms)

Electronegativity

-Within a family, the trend is decreasing (because weaker nuclear pull on electron in larger atoms making it difficult to attract other electrons in a chemical bond) -Across a period, the trend is increasing (because stronger nuclear pull on electron in smaller atoms makes it easier to attract other electrons in a chemical bond)

Electron affinity

-Within a family, the trend is decreasing (because weaker nuclear pull on electron in larger atoms making it difficult to attract other electrons) -Across a period, the trend is increasing (because stronger nuclear pull on electron in smaller atoms makes it easier to attract other electrons)

Atomic radius

-Within a family, the trend is increasing (because the valence shell is farther from the nucleus) -Across a period, the trend is decreasing (because its adding electrons to the valence shell)

Nitrogen

-colorless -odorless -tasteless -can also turn in to a liquid -Doesn't react with anything under normal conditions

Nickel

-silver color -magnetic metal -hard -malleable -ductile -conducts electricity -not very reactive

How many groups are there?

3; Metals, Non-Metals, & Metalloids

Where are the alkali metals, the alkaline earth metals, the halogens, and the noble gases located in the periodic table?

Alkali metals: Group 1A Alkaline earth metals: Group 2A Halogens: Group 7A Nobles Gases: Group 8A

Which of these metals isn't a transition metal? a. aluminum b. silver c. iron d. zirconium

Aluminum

How can you tell how many valence electrons there are for the elements

By the group number, except for transitional metals. With nonmetals, ignore the first number- ex: 17 -> 7 valence electrons

Columns #1-18

Families

Why does the ionic radius always become larger?

Filling energy levels increases the shielding effect.

Explain why fluorine has a smaller atomic radius than both oxygen and chlorine.

Fluorine is keeping it's electron very close to the nucleus. Making the atomic radius smaller. Atomic radius trend goes from left to right that atomic radius decreases. The atomic radius increases from top to bottom.

Losing weight

Getting smaller waist--> pull that belt tighter

Why does the ionic radius always become smaller?

Losing electrons could sometimes lose an energy level.

Mendeleev

Made the 1st useful periodic table by using atomic mass to place the elements horizontally & similar chemical reactivity to place them vertically

Halogen family

Most reactive nonmetal family

What element makes itself bigger than it is?

Na (sodium)

Anion

Negatively charged ion formed through the gaining of electrons. Always nonmetals.

John Newlands

Noticed that elements were arranged by increasing atomic mass, their properties repeated every eighth element; known as the Law of Octaves

Atomic Mass

Number of protons and neutrons in an atom

Atomic Number

Number of protons in an atom

Atomic radius

One-half the distance between the nuclei of identical atoms that are bonded together

Rows #1-7

Periods

Mosley

Placed the elements horizontally by atomic number & vertically by similar chemical reactivity

Cation

Positively charged ion formed through the loss of electrons. They are always metals.

Law of Octaves

The 1st and 8th elements had similar properties

Shielding effect

The effect of inner electrons in decreasing the nuclear charge experienced by outer electrons

Electronegativity

The element's atom ability to attract electrons in a chemical bond

Electron affinity

The energy change that occurs when are electron is added to an atom and an ion

Ionization energy

The energy required to remove an electron from an atom is in its ground state

Noble gases

Very stable; have a full octet of electrons

a. In which 50-year period were the most elements discovered? b. How did Mendeleev's work contribute to the discovery of elements? c. What percent of these elements were discovered by 1900?

a. 1801-1850 b. Many elements were founded after his work c. 50%

Use the figure to write the electron configurations of these elements. a. boron b. arsenic c. fluorine d. zinc e. aluminum

a. Boron: 1s2 2s2 2p1 b. Arsenic: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 c. Fluorine: 1s2 2s2 2p5 d. Zinc: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 e. Aluminum: 1s2 2s2 2p6 3s2 3p1

Locate each of the following elements in the periodic table and decide whether its atoms are likely to form anions or cations. a. sodium b. fluorine c. calcium d. potassium e. iodine f. beryllium g. oxygen h. lithium

a. Cation b. Anion c. Cation d. Cation e. Anion f. Cation g. Anion h. Cation

Which element in each pair has a higher electronegativity value? a. Cl, F b. C, N c. Mg, Ne d. As, Ca

a. F b. N c. Mg d. As

Which particle has the larger radius in each atom/ion pair? a. Na, Na^+ b. S, S^2- c. I, I^- d. Al, Al^3-

a. Na b. S^2- c. I^- d. Al^3-

Identify each property below as more characteristic of a metal or a nonmetal. a. a gas at room temperature b. brittle c. malleable d. poor conductor of electric current e. shiny

a. Nonmetal b. Nonmetal c. Metal d. Nonmetal e. Metal

Arrange the following groups of elements in order of increasing ionization energy: a. Be, Mg, Sr b. Bi, Cs, Ba c. Na, Al, S

a. Sr, Mg, Be b. Cs, Ba, Bi c. Na, Al, S

Which element in each pair has a greater first ionization energy? a. lithium, boron b. magnesium, strontium c. cesium, aluminum

a. boron b. magnesium c. aluminum

Which element in each pair has atoms with a larger atomic radius? a. sodium, lithium b. strontium, magnesium c. carbon, germanium d. selenium, oxygen

a. sodium b. strontium c. germanium d. selenium

Gaining weight

getting larger waist--> loosen the belt

Arsenic

• Two forms • Brittle, gray, metallic (stable) • Yellow, non-metallic solid (reactive) • Both are odorless, tasteless, solid at room temperature, and are hexagonal/rhombic crystals

Iodine

•Resembles chlorine and bromine, but it is much less reactive •Reacts quantitatively with sodium thiosulfate •Combines directly with many elements, although it is usually necessary to provide heat and/or a catalyst •A black, shiny, crystalline solid •When heated, it sublimes to form a purple vapor •Non-metal, but has some metallic properties