South Pasadena • Chemistry



Name ________________________________ Period ___ Date ___/___/___

Periodic Table

PROPERTIES & TRENDS

Classifying the Elements:

The elements can be classified in two ways:

▪ Metals, non-metals, and semi-metals

▪ Chemical families (groups)

Metals are good __________________ of heat and electricity. They are ______ and lustrous. They are ___________ which means they can be pounded into thin sheets. They are _________ which means they can be drawn into wires.

Metals have low ___________________ which means that they do not hold onto their valence electrons tightly. In their compounds they form ions with ___ charge.

Nonmetals are poor ____________________ of heat and electricity. An important exception is pure carbon in the form of ___________. Unlike metals, as solids they are ___________ when hit with a hammer.

All of the diatomic elements are nonmetals. Note that ___ is a nonmetal even though it is located with the metals on the periodic table. Use the Gen-U-Ine Rule to identify the 7 elements that form diatomic molecules.

____ ____ ____ ____ _____ ____ _____

Nonmetals have high ___________________ and tightly hold onto their valence electrons. In their compounds the nonmetals form ions with a ___ charge.

Semimetals have properties that are in between metals and nonmetals. They are important in the semiconductor and computer industries. The semimetals are: __ __ __ __ __ __ __.

Sketch the location of the semi-metals, metals, nonmetals and noble gases:

[pic]

Properties of the Families:

Alkali Metals (1): __ __ __ __ __ __

▪ In their compounds they always form __ ions.

▪ They react with _____ to form H2(g) and OH− ions.

Example: Na + (

▪ Their chemistry involves _________ (gaining/losing) one electron. They have one _________ electron.

▪ They are ______ metals and can be cut with a knife.

▪ They are never found uncombined in nature because they are so reactive.

▪ They are stored _________ _______.

Alkaline Earth Metals (2): __ __ __ __ __ __

▪ In their compounds they always form __ ions.

▪ They slowly react with _____ to form H2(g) and OH− ions. Example: Ca + (

▪ Their chemistry involves _________ (gaining/losing) two electrons. They have two ________ electrons.

▪ __ is a component of bones and teeth.

Noble Gases (18): __ __ __ __ __ __

▪ These elements do not easily combine with other elements. They are odorless, colorless and therefore were difficult to discover.

▪ When air is cooled, O2 liquefies first at -182(C. N2 liquefies at -195(C. About 1% of the air is still gas composed of the noble gas ________, __.

▪ One noble gas is radioactive and seeps up through basement floors and walls. It is ________, __.

▪ One noble gas is best known for its orange color in gas discharge tubes. It is used for signs that bear its name. It is _______, __.

Halogens (17): __ __ __ __ (__)

▪ In their compounds they always form __ ions.

▪ They have ___ valence electrons.

▪ They react with ________ to form salts which gives them their name of “salt formers.”

Example: 2 Na + Cl2 (

▪ Their chemistry involves _________ (gaining/losing) one electron.

▪ All of the members of this family are _________. (We assume At2 would exist if there were any.)

▪ Halogens are very _______________. The element on the table with the greatest attraction for electrons is ___________, ___ (4.0).

Hydrogen, H

▪ Hydrogen is its own family.

▪ It usually forms ___ ions.

▪ It can combine with halogens.

Example: H2 + Cl2 (

▪ In this case, H ______ (gains/loses) one electron.

▪ Hydrogen has ___ valence electron.

▪ H is located with the _________ ________ family.

▪ It has one less electron than the noble gas, ___.

▪ It can combine with alkali and other metals.

Example: 2Li + H2 (

▪ In this case, H ______ (gains/loses) one electron.

▪ In this case, H has a ___ charge (oxidation #).

▪ It is diatomic like the __________ family.

Trends in the Periodic Table:

Size of the Elements:

[pic]

(Sketch the trend in size)

The size of the atom is due to the size of the ___________ ___________. The two forces at play are __________ between the electrons and other electrons and ____________ between the electrons and protons in the nucleus.

Left to right across the table, the atoms get _________ because there are more and more _________ in the nucleus pulling on the valence electrons. In any period, the valence electrons are on the same level (floor).

Going down any group or family, the atoms get ___________ because there are more and more __________ of electrons. Each level of electrons is ____________ from the nucleus.

Ionization Energy (IE)

This is defined as the energy needed to remove an electron from an atom.

Example: Na + NRG ( Na+ + e−

It is _________ (easier/harder) to remove an electron from a larger atom. This is because the electron is _________ (closer/farther) from the nucleus and feels _______ (less/more) attraction.

[pic]

(Sketch the trend in ionization energy)

Sizes of Ions:

Each time an electron is removed, the atom/ion becomes __________ (smaller/larger) because there is ________ (more/less) e−- e− repulsion.

So… each successive electron removed has a ___________ (higher/lower) ionization energy.

(Atoms that gain electrons become ___________.)

After all the valence electrons are removed, the next electron is much __________ (closer to/farther from) the nucleus and is much more difficult to remove. There is a big jump in Ionization NRG.

ION Formation: each group on the periodic table will normally gain or lose a certain number of electrons to become an ion, Label the periodic table below with the charges usually found on the ions formed for each group (leave out the transition metals)

+1

[pic]

TAKS PRACTICE QUESTIONS:

1)According to the periodic table, which element most readily accepts electrons?

A Fluorine B Nitrogen

C Arsenic D Aluminum

2)An unidentified element has many of the same physical and chemical properties as

magnesium and strontium but has a lower atomic mass than either of these elements.

What is the most likely identity of this element?

F Sodium G Beryllium

H Calcium J Rubidium

3) The elements from which of the following groups are most likely to react with

potassium (K)?

F Group 2 G Group 7

H Group 13 J Group 17

4) The elements of which of these groups on the periodic table are most resistant to forming

compounds?

A Group 1 B Group 9

C Group 14 D Group 18

[pic]

5) The table shows the atomic radii of some elements in Periods 1 through 4 of the periodic table. Which inference can be made from this information?

F Atomic radii decrease from left to right.

G Atomic radii increase from bottom to top.

H Atomic radii decrease from right to left.

J Atomic radii double from top to bottom.

6) Which of these elements is most likely to donate one electron?

F Be G Cs

H Rn J He

7) A certain atom has a nucleus containing six protons and eight neutrons and has six

electrons orbiting the nucleus. This atom is a form of the element —

A silicon B carbon

C magnesium D calcium

8) In which model of the periodic table does the shaded area show the location of elements

that require the least energy to lose one electron?

[pic]

9) According to the periodic table, which of these

elements will form an ion with a –2 charge?

F S

G Mg

H F

J Rb

10) Calcium ions play an important role in the function of neurons in the brain. Elements

that are chemically similar to calcium can interfere with the function of neurons. Which

of the following is most likely to imitate calcium’s role in the function of neurons?

F Sodium

G Potassium

H Strontium

J Rubidium

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download