Periodic Table and Trends

Question 1

What are the columns of elements in the periodic table?

Answer 1

Groups

Question 2

What are rows of elements in the periodic table?

Answer 2

Periods

Question 3

A family of elements is the same as…

Answer 3

A group

Question 4

A metal can be stretched into thin wire is…

Answer 4

Ductile

Question 5

The ability to conduct electricity is a property of…

Answer 5

Metals

Question 6

A metal that can be hammered into thin sheets because it is…

Answer 6

Malleable

Question 7

A property of metals is ____ or shininess.

Answer 7

Luster

Question 8

______ is the gradual wearing away of a metal due to a chemical reaction with water or elements in the atmosphere.

Answer 8

Corrosion

Question 9

Elements that are ______ are located to the right of the zig-zag line in the periodic table.

Answer 9

Nonmetals

Question 10

Elements that have the same properties as both, metals and nonmetals are…

Answer 10

Metalloids

Question 11

______ are elements that tend to gain electrons in chemical reactions.

Answer 11

Nonmetals

Question 12

Coulombic Attraction

Answer 12

The attraction between oppositely charged particles.

less distance, more attraction; more distance, less attraction

Question 13

Number of protons + attractive force

Answer 13

Increased protons –> increased attractive force

Question 14

Electrons are attracted to protons in a nucleus, but are repelled by electrons in the same atom.

Answer 14

Electron Repulsion

Question 15

Ion

Answer 15

An atom that is negatively/positively charged, or neutral.

Question 16

Valence electron

Answer 16

Electrons in the outermost shell of an atom.

Question 17

How is an ion formed?

Answer 17

When an atom gains/loses an electron to reach stability

Question 18

Ionization energy

Answer 18

Energy required to remove an electron

Question 19

Ionic Radius

Answer 19

The size of an ion, when it gains/loses an electron.

Question 20

Cation

Answer 20

Positively charged ion - neutral ion is larger than (>) +ion
Na+
- less electrons -> less repulsion
- # of shells dec. -> stronger attraction towards valence electrons
- less shielding effect

Question 21

Anion

Answer 21

Negatively charged ion - neutral ion is smaller than ( more electron repulsion
- same shielding effect

Question 22

Shielding Effect

Answer 22

Describes the balance between the pull of the protons on valence electrons and the repulsion forces from inner electrons

Question 23

Atomic Radius

Answer 23

The size of an atom

• The distance between the nucleus and valence electrons
• 1/2 distance between the nuclei

Question 24

Atomic Radius - across a period

Answer 24

Atomic radius DECREASES

• proton # increases, attraction increases
• distance stays the same -> same period = same # of shells
• shielding effect stays the same
• electron repulsion increases, but not as effective

Question 25

Atomic Radius - down a group

Answer 25

Down a group, atomic radius increases - distance between valence electrons and nucleus increases -> # of shells increase - shielding effect increases, attraction decreases - electron repulsion increases (makes atom larger)

Question 26

Electronegativity

Answer 26

The tendency for an atom to attract shared electrons when forming a chemical bond. - element with the highest electronegativity: F (Fluorine) (approx 3.98 or 4.0) - G18 ARE NONMETALS - DO NOT ATTRACT

Question 27

Electronegativity - across a period

Answer 27

- Across a period, increases - Atoms get smaller - Proton # increases, distance stays the same - Attraction towards electrons increase - Electronegativity increases

Question 28

Electronegativity - down a group

Answer 28

- Down a group, electronegativity decreases - Atoms are getting larger - Attraction gets weaker - Less attraction, towards electrons - Electronegativity decreases

Question 29

Reactivity

Answer 29

A measure of how readily a substance undergoes a chemical reaction

Question 30

Reactivity: Metals - down a group

Answer 30

- Down a groups, reactivity increases for metals. - Starts to form positive ions - Wants to lose electrons - Less force of attraction - valence electrons - Less ionization energy -> easier to remove an electron - Easier to react to other elements

Question 31

Reactivity: Metals - across a period

Answer 31

- Across a period, reactivity decreases for metals. - More attraction for valence electron - More ionization energy -> harder to remove an electron - Harder to react with other elements - Most reactive metal: Francium

Question 32

Reactivity: Nonmetals - down a group

Answer 32

- Down a group, reactivity decreases for nonmetals. - Forms negative ions - Wants to gain electrons - Less attractions - valence electrons - Less electronegativity - Lower reactivity

Question 33

Reactivity: Nonmetals - across a period

Answer 33

- Across a period, reactivity increases in nonmetals. - More attraction for valence electrons - More electronegativity - Higher reactivity - Most reactive NM: Chlorine

Question 34

Alkali Metals

Answer 34

- GROUP 1, does not include hydrogen - Shiny, soft, highly reactive metals - DO NOT OCCUR NATURALLY - Only have 1 valence electron - Reactivity increases down the group

Question 35

Alkaline Earth Metals

Answer 35

- GROUP 2 - Has 2 valence electrons - Somewhat reactive metals, some of which occur naturally as free elements - Reactivity increases down the group

Question 36

Icosagens

Answer 36

- GROUP 3 - All have 3 valence electrons - Called "poor metals" due to their low melting points + hardness - Liquid at a larger range of temperature than any other element

Question 37

Crystallogens

Answer 37

- GROUP 4 - A mix of metals, nometals, and metalloids - All have 4 valence electrons

Question 38

Pnictogens

Answer 38

- GROUP 5 - All have 5 valence electrons - All solids, apart from nitrogen, are a mix of nonmetals, metalloids and metals

Question 39

Chalcogens

Answer 39

- GROUP 6 - All have 6 valence electrons - Form -2 ions when reacting w/ electropositive metals

Question 40

Halogens

Answer 40

- GROUP 7 - Contains elements in all 3 states of matter - All reactive nonmetals - All form diatomic molecules - Reactivity decreases down the group

Question 41

Noble Gases

Answer 41

- All monoatomic, rarely form compounds | - Not very reactive -> already have a full valence electron shell