Hnrs Chem Unit 1 Part 2

How is the modern periodic table arranged?

Atomic number

Where are metals located?

Left of the stair-step line

Where are nonmetals located?

Right of the stair-step line

Where are metalloids/semimetals located?

along the stair-step line, except for Al

What do the horizontal rows on a periodic table represent?

Periods

What are the groups/families on the period table?

Alkali metals, alkaline earth metals, halogens, noble gases, and transition metals.

What are the two types of Inner transition metals?

Lanthanide series and actinide series

What column(s) are alkali metals found?

1

What column(s) are alkaline earth metals found?

2

What column(s) are transition metals found?

3-13

What column(s) are halogens metals found?

17

What column(s) are noble gases found?

18

What are the natural stages of elements (at room temperature)?

solids, liquids, gases, man-made

What column of elements form an 1+ ion?

1st

What column of elements form an 2+ ion?

2nd

What column of elements form an 3+ ion?

13th

What column of elements form an + or - 4 ion?

14th

What column of elements form an 3- ion?

15th

What column of elements form an 2- ion?

16th

What column of elements form an 1- ion?

17th

What is electromagnetic radiation?

Type of energy that travels space through waves. Has both wave and particle properties.

What are the types of electromagnetic radiation? (in order)

Radio waves, radar, microwaves, infared light, ultraviolet light, x-rays, and gamma rays.

How are different types of electromagnetic radiation similar?

All electromagnetic radiation travels at the speed of light (3 × 10^8 m/s)

How are different types of electromagnetic radiation different?

They differ in wavelength, frequency, and energy levels.

What are wavelengths?

The distance between two consecutive crests.

What is frequency?

The # of wave cycles to pass a given point per unit of time

How are wavelength and frequency mathematically related?

They are inversely proportional

How are energy and frequency mathematically related?

They are directly proportional

How are energy and wavelength mathematically related?

They are inversely proportional

What are the colors of visible light from lowest energy to highest energy?

Red, Orange, Yellow, Green, Blue, Indigo, and Violet (ROYGBIV)

What is a “packet” of electromagnetic energy called?

photon or quanta

What happens when electricity is passed through an element in the gaseous state? (what causes the atomic emission spectra?)

When atoms absorb energy, their electrons move to higher energy levels. They loose energy by emitting light when they return to lower energy levels.

What is an energy level?

The areas of fixed energy where electrons can be found.

What is a quantum?

The amount of energy required to move an electron from one energy level to another energy level

What is the Bohr model?

Neils Bohr proposed that an electron is found only in specific orbits around the nucleus.

Why do atoms produce a bright line spectrum or flame test with specific colors? (Using Bohr’s theory)

Each energy level in the electron cloud has a particular amount of energy.

When electrons fall from a higher energy level to a lower energy level, light is released.

The colors are due to the atom releasing certain photons of energy (different amounts of energy) as the electrons fall from certain energy levels.

What does the Quantum mechanical Model do?

It designates the amount of energy the electron possesses and it’s approximate location.

What is an atomic orbital?

The allowed energies an electron can have and the various locations around the nucleus of the atom

What are the type of orbitals?

s, p, d, f

What does the s orbital look like?

Spherical shape

Where is the s orbital located?

It’s present in every energy level because the 1st orbital is filled with e- in each energy level.

What does the p orbital look like?

dumbbell shaped, group of 3 orbitals.

Where is the p orbital located?

Present in the 2nd energy level and beyond

What does the d orbital look like?

group of 5 orbitals

Where is the d orbital located?

Present in the 3rd energy level and beyond

What does the f orbital look like?

group of 7 orbitals

Where is the d orbital located?

Present in the 4th energy level and beyond

What are the 3 rules for writing the electron configurations of elements?

Aufbau Principle, Pauli Exclusion Principle, Hand’s Rule

What does Aufbau Principle state?

Electrons must fill the lowest energy levels first

What does Pauli Exclusion Principle state?

An atomic orbital can hold a maximum of 2 electrons. Two electrons occupying the same orbital must have opposite spin

What does Hand’s Rule state?

There must be one electron in each orbital before they can double up.

What are valence electrons?

The e- in the outermost (highest) energy level of an atom

Why are valence e- the most important e- to chemists?

They are the ones involved when atoms form bonds

What are inner electrons known as?

Core elements

Are inner electrons involved in bonding?

No, they aren’t.

What do elements with the same valence e- show?

Very similar chemical behavior.

What happens to atomic size (radii) as you go down a group/family on the period table?

They get larger

Why do atoms get larger as you go down a group/family?

They get bigger as e- are added to larger principle energy levels (more energy levels are added)

What happens to atomic size (radii) as you go from left to right across a period?

They get smaller

Why do atoms get smaller as you go from left to right across a period?

The # of protons in the nucleus increases (increasing nuclear charge), so the e- being added to the same energy level are in tighter to the nucleus.

What are cation (negative ions) compared to neutral atom?

They tend to be smaller

Why are cations smaller than neutral atoms?

As e- are removed, the negative charge decreases while the positive charge in the nucleus remains the same → e- pulled in tighter.

What are anions (negative ions) compared to the neutral atom?

They tend to be larger.

Why are anions larger than the neutral atom?

As e- are added, the negative charges of repulsion are greater than the positive charge of attraction to the nucleus → causing the e- to spread out more.

What is electronegativity (EN)?

The ability of an atom of an electron to attract electrons when the atom is in a compound.

What happens to EN as you go down a group/family on the period table?

It tends to decrease.

Why does EN decrease as you go down a group/family?

Valence e- get further from the nucleus (larger atomic radii), so the e- have less attraction to the nucleus.

What happens to EN as you go from left to right across a period on the periodic table?

It tends to increase

Why does EN decrease as you go from left to right across a period on the periodic table?

Valence e- get closer to the nucleus (smaller atomic radii), so the e- have more attraction to the nucleus

What is the ionization energy of an atom?

Energy required to remove an e- from an individual atom in the gaseous phase

What are metals’ ionization energy like?

They have relatively low ionization energies

What does the low ionization of metals indicate?

A relatively small amount of energy is needed to remove an e- from a typical metal (metals tend to LOSE e-)

What are nonmetals’ ionization energy like?

They have relatively large ionization energies

What does the high ionization of nonmetals indicate?

A relatively large amount of energy is needed to remove an e- from a typical nonmetal. (this is why nonmetals tend to GAIN e-)

What happens to ionization energies as you go down a group/family on the periodic table?

Ionization energy tends to decrease

Why does ionization energy decrease as you go down a group/family?

Valence e- get further from the nucleus (larger atomic radii), so less energy would be needed to remove an e-

What happens to ionization energies as you go from left to right across a period on the periodic table?

Ionization energy tends to increase

Why does ionization energy decrease as you go from left to right across a period?

Valence e- get closer to the nucleus (smaller radii), so more energy would be needed to remove an e-

What happens to successive ionization energies in an atom?

Successive ionization energies tend to increase

Why do successive ionization energies tend to increase in an atom?

The nuclear charge stays the same but as the e- are removed, the neg. charge decreases (less repulsion between the e-), & remaining e- get pulled in tighter → so more energy is required to remove additional e-