Chapters 1-4

Chemical symbol vs nuclear symbol

Cl identifies the element; ³⁷₁₇Cl identifies a specific isotope

Top number in nuclear symbol

Mass number

Bottom number in nuclear symbol

Atomic number

How many neutrons are in ⁶⁵₃₀Zn?

35

How many neutrons are in ⁸⁰₃₅Br?

45

How many neutrons are in ⁷⁹₃₄Se?

45

How many neutrons are in ³¹₁₅P?

16

How many neutrons are in ¹⁸₈O?

10

How many protons, neutrons, and electrons are in ⁸⁰₃₅Br⁻?

35 p, 45 n, 36 e

How many protons, neutrons, and electrons are in ³¹₁₅P³⁻?

15 p, 16 n, 18 e

How many protons, neutrons, and electrons are in ²⁴₁₂Mg²⁺?

12 p, 12 n, 10 e

What determines element identity?

Number of protons

What determines isotope identity?

Number of neutrons

What determines ionic charge?

Difference between protons and electrons

Average atomic mass formula

Σ(isotope mass × fractional abundance)

Convert 24.78% abundance into decimal

0.2478

Convert 75.22% abundance into decimal

0.7522

If average atomic mass is closer to one isotope

That isotope is more abundant

Chlorine average atomic mass is 35.45 amu. Which isotope is more abundant?

Cl-35

Bromine average atomic mass is 79.90 amu. Which isotope is more abundant, Br-79 or Br-81?

Br-79

An element has isotopes 20 amu (90%) and 22 amu (10%). Average mass?

20.2 amu

An element has isotopes 35 amu (75%) and 37 amu (25%). Average mass?

35.5 amu

What does a weighted average account for?

Different abundances of isotopes

Group 1 name

Alkali metals

Group 2 name

Alkaline earth metals

Group 17 name

Halogens

Group 18 name

Noble gases

Most reactive nonmetals

Halogens

Least reactive elements

Noble gases

Metalloids

B, Si, Ge, As, Sb, Te

Location of metals

Left side of periodic table

Location of nonmetals

Right side of periodic table

Location of metalloids

Along staircase

Group 1 valence electrons

1

Group 2 valence electrons

2

Group 13 valence electrons

3

Group 14 valence electrons

4

Group 15 valence electrons

5

Group 16 valence electrons

6

Group 17 valence electrons

7

Group 18 valence electrons

8

Which group has 5 valence electrons?

Group 15

Which group has 6 valence electrons?

Group 16

Which group has 7 valence electrons?

Group 17

Which group has 1 valence electron?

Group 1

Which group has 2 valence electrons?

Group 2

Atomic radius trend

Increases down and left

Ionization energy trend

Increases up and right

Metallic character trend

Increases down and left

Which trend is opposite atomic radius?

Ionization energy

Which trend follows atomic radius?

Metallic character

Largest atom on periodic table

Francium

Smallest atom on periodic table

Helium

Highest ionization energy

Helium

Lowest ionization energy

Francium

Most metallic element

Francium

Least metallic element

Helium

Arrange by increasing atomic radius

Na, Mg, Al, Si

Arrange by increasing atomic radius

F, Cl, Br, I

Arrange by increasing atomic radius

N, P, As, Sb

Arrange by increasing atomic radius

Ar, Cl, S, P

Arrange by increasing atomic radius

K, Ca, Ga, Br

Arrange by increasing ionization energy

K, Ca, Ga, Br

Arrange by increasing ionization energy

Na, Mg, Al, Si

Arrange by increasing ionization energy

I, Br, Cl, F

Arrange by decreasing ionization energy

F, O, N, C

Arrange by decreasing ionization energy

Ar, Cl, Br, K

Arrange by increasing metallic character

Br, Ga, Ca, K

Arrange by increasing metallic character

F, Cl, Br, I

Why does atomic radius decrease across a period?

Increasing nuclear charge

Why does ionization energy increase across a period?

Stronger attraction between nucleus and electrons

Why does atomic radius increase down a group?

Additional occupied energy levels

Why does ionization energy decrease down a group?

Valence electrons farther from nucleus

Cation compared to parent atom

Smaller

Anion compared to parent atom

Larger

Why are cations smaller?

Fewer electrons and reduced repulsion

Why are anions larger?

Increased electron repulsion

Which is larger, K or K⁺?

K

Which is larger, Ca or Ca²⁺?

Ca

Which is larger, O or O²⁻?

O²⁻

Which is larger, F or F⁻?

F⁻

Which is larger, Cl or Cl⁻?

Cl⁻

Which is larger, Na or Na⁺?

Na

Isoelectronic species

Species with same number of electrons

What determines size among isoelectronic species?

Atomic number

For isoelectronic species, largest atomic number gives what radius?

Smallest

Arrange in increasing radius

Mg²⁺, Na⁺, Ne

Arrange in increasing radius

Al³⁺, Mg²⁺, Na⁺, Ne

Arrange in increasing radius

O²⁻, F⁻, Ne

Arrange in increasing radius

O²⁻, F⁻, N³⁻

Arrange in increasing radius

Ca²⁺, K⁺, Ar, Cl⁻, S²⁻

How many orbitals are in an s sublevel?

1

How many orbitals are in a p sublevel?

3

How many orbitals are in a d sublevel?

5

How many orbitals are in an f sublevel?

7

How many electrons fit in an s sublevel?

2

How many electrons fit in a p sublevel?

6

How many electrons fit in a d sublevel?

10

How many electrons fit in an f sublevel?

14

How many orbitals are in n=3?

9