General Chemistry I - Exam 2

Front 1

Atomic radii _______ going down a group and _________ going across a period

Back 1

Increases going down a group
Decreases going across a period.

Front 2

Within each group (vertical column) atomic radii tends to?

Back 2

Increase with the period number. Increases from top to bottom.

Front 3

Group I metals are considered the?

Back 3

Alkali metals

Front 4

Group II metals are considered the?

Back 4

Alkaline metals

Front 5

What metal has the smallest atomic radii among the Alkaline earth elements?

Back 5

Be

Front 6

Energy required to remove the highest energy electron from the neutral atom in the gaseous state is called

Back 6

Ionization energy

Front 7

Ionization energy ______ going down a group and ______ going across a period.

Back 7

Decreases going down a group and increases going across a period.

Front 8

Less negative going down a group and more negative going across a group is?

Back 8

Electron affinity.

Front 9

Metal character _______ going down a group and ________going across a period.

Back 9

Increases going down a group and decreases going across a period.

Front 10

Building up principle or Aufbau principle: Name till 5f

Back 10

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f

Front 11

An orbital can hold at most two electrons, and then only if the electrons have opposite spins. What principle is this?

Back 11

Pauli exclusion principle

Front 12

The lowest energy arrangement of electrons in a subshell is obtained by putting electrons into separate orbitals of the subshell with the same spin before pairing electons. Who's rule?

Back 12

Hund's rule.

Front 13

A diamagnetic substance has...

Back 13

Paired electrons

Front 14

A paramagnetic substance has....

Back 14

Unpaired electrons

Front 15

A charge that the electron feels, including both attraction to the nucleus and repulsion from the electrons.

Back 15

Effective nuclear charge.

Front 16

Explain first in first out concept for the transition metals:

Back 16

In transition metals, the s subshell is filled before the d subshell and also removed before the d subshell.

Front 17

Bonding between two oppositely charged ions.

Back 17

ionic bond. Example: NaCl

Front 18

Electron sharing between two atoms.

Back 18

covalent bond. Example: H2

Front 19

Positive metal ions held together in a lattice with a "sea of electrons"

Back 19

Metallic bonding.

Front 20

Species with the same number of electrons is called? Give example.

Back 20

Isoelectronic. Example is Li+ and He

Front 21

Which element is allowed to have only 2 bonds?

Back 21

Be (Beryllium)

Front 22

Which element is allowed to have only 3 bonds?

Back 22

B (Boron)

Front 23

Which elements are allowed to have the exceptions to the octet rule?

Back 23

Elements in period 3 and higher. Meaning periods 3, 4, 5, 6 and 7.

Front 24

As you go down a column, ions ___________ in size due to the value of _________

Back 24

Increase and N

Front 25

Ionic size ____________ with an increasing nuclear charge.

Back 25

Decreases.

Front 26

Cis means...

Back 26

next to

Front 27

Trans means....

Back 27

Across from