Chapter 10 (periodic Trends)

Question 1

Atoms get smaller as you move across (—->) a period (row) becuase

Answer 1

Protons are being added

Question 2

Ionization energy

Answer 2

The minimum amount of energy required in order to remove an electron from the atom

Question 3

Larger atoms are easier to remove an electron because

Answer 3

It is further alway from the nucleus and isn’t held as tightly together

Question 4

Atoms get larger as you move down the group, why?

Answer 4

As you add energy levels, you are adding e’ at a quarter distance from the nucleus.

Question 5

Smaller atoms _______ to the nucleus better.

Answer 5

Attract,
Big ones can get through cloud
(Noble gases not included in trend)

Question 6

When a neutral atom loses an electron it’s called

Answer 6

A cation

Question 7

What types of atoms tend tot lose electrons

Answer 7

Metals

Question 8

When a neutral atom gains an electron it’s called

Answer 8

Anion

Question 9

What types of atoms tend to gain electrons

Answer 9

Nonmetals

Question 10

Periodic law

Answer 10

If elements arranged in order of increasing atomic mass, a pattern can be seen in which similar properties recur on a regular or periodic basis

Question 11

Metals

Answer 11

Solid at room temp 
Shiny, lustrous
Good conductors of heat and electricity 
Malleable 
Flexible 
Gives up electrons easily to form cations

Question 12

Non metals

Answer 12

Gases or brittle solids at room temp
Dull to translucent opaque
Poor conductors of heat and electricity

Question 13

Alkali metals

Answer 13

• located far left of periodic table (lithium, sodium, potassium..)
• soft, silvery, solids
• most reactive of all metals
• react vigorously with water to produce hydrogen gas
• one valence electrons
  Group 1

Question 14

Alkaline earth metals

Answer 14

• silver colored reactive metals
• readily form compounds with non metals
• low solubility in water
• two valence electrons
• group 2

Question 15

Periodic trends

Answer 15

Consistent and predictable changes in elemental properties

Question 16

Atomic radius

Answer 16

Distance from the nucleus to the boundary of the surrounding cloud of electrons

Question 17

Two periodic trends

Answer 17

• As we move down a family, the sizes of atoms increase

- Across a period sizes decrease

Question 18

Ionization energy

Answer 18

Minimum energy required to remove an electron from a gaseous atom or ion.

• tells us how strongly an atom holds on to its outermost electrons
• ion with low IE is more likely to lose electrons and form cations during chemical changes
• a high IE ion tendency to gain electrons and from anions or no ions

Question 19

Size of atoms and IE

Answer 19

Larger atoms (outer electrons are held less tightly together) = lower IE

The smaller the atom (held tightly together) = higher IE

**as atomic size increases, IE decreases

Question 20

Alkali metals and IE

Answer 20

Alkalis have the lowest IE

Question 21

Electronegativity

Answer 21

Relative ability of a bonded atom to attract shared electrons to itself.
- atoms with higher EN tend to pull bonded electrons closer to nucleus

Question 22

EN and atomic size

Answer 22

Smaller atoms have higher EN

Larger atoms, lower EN

Question 23

PES

Answer 23

-energy measurement of electrons emitted from solids, gases or liquids by the photoelectric effect

Question 24

Ionic bonding

Answer 24

Electrostatic attractive force bw oppositely charged ions produced when a metal atom transfers one or more electrons to a non-metal atom.

Question 25

Covenant bonds

Answer 25

The term covalent bond is used to describe the bonds in compounds that result from the sharing of one or more pairs of electrons.

Ex) h2

Question 26

Polar covenant bond

Answer 26

Where a bond “dipole” is said to exist

Caused by an unequal distribution of electron density will give that end of the bond a partially negative “pole”

Question 27

Network covalent solids

Answer 27

The strength of covenant bonds can be seen through studying this

Question 28

Ionic bond properties

Answer 28

High melting point
Brittle
Hard

Question 29

Molecular bond properties (intermolecular forces)

Answer 29

Low melting point, nonconducting

Question 30

Network bond properties

-covelant

Answer 30

High melting point
Hard
Nonconducting

Question 31

Network bond

Answer 31

Chemical compound in which the atoms are bonded by covalent bonds in a continuous network extending throughout (no individual molecules)

Question 32

Covalent bonds (NM+NM)

Answer 32

Occur when a pair of electrons are shared by atoms

• stable
• unshared
• liquid/gas at room temp
• low polarity
• formed by two non metals
• definite shape
• low boiling point

Question 33

Ionic bonds are….

Answer 33

• unstable
• solid at room temp
• high polarity
• no definite shape
• M + NM

Question 34

Lewis structures: which are written with brackets

Answer 34

Metals in group 1,2,13

Question 35

Lone pairs are on….?

Answer 35

The central atom

Question 36

Intermolecular forces

Answer 36

Make molecules attracted to one another 
 Includes:
London dispersion
Dipole-dipole
Hydrogen

Question 37

London dispersion

Answer 37

Forces that hold molecules together in a liquid, solid, and solution phase
Weakest

Question 38

Dipole-dipole bonding

Answer 38

Only with polar molecules

Bw ionic and covalent bonds

Question 39

Hydrogen bond

Answer 39

Hydrogen has to be bonded with a highly EN atom (N O F)