Chem class 1

Question 1

Alpha Decay

Answer 1

Subtracts 4 from the mass number and subtracts 2 from the atomic number

Question 2

Beta- Decay

Answer 2

Will always change the identity of an element. Adds 1 to the atomic number.

Question 3

Beta+ Emitter

Answer 3

Subtracts 1 from the atomic number. All types of beta+ emitter decay leave the mass of the daughter and parent elements the same.

Question 4

Gamma decay

Answer 4

Brings an excited nucleus to a lower energy state. Doesn’t change mass number or atomic number.

Question 5

Electron capture

Answer 5

Causes the atomic number to be reduced by 1 while the mass number remains the same.

Question 6

diamagnetic

Answer 6

An atom that has all of its electron spin-paired.

Question 7

Paramagnetic

Answer 7

Is when an atoms electrons are not all spin paired.

Question 8

periodic table group 1

Answer 8

alkali metals

Question 9

periodic table group 2

Answer 9

Alkaline earth metals

Question 10

periodic table group 7

Answer 10

Halogens

Question 11

periodic table group 8

Answer 11

Noble gases

Question 12

What are the three fundamental particles of matter and which determines the identity of the element?

Answer 12

Proton determines element identity, neutron, electron.

Question 13

Isotopes differ by number of which fundamental particle? The mass number of an element is determined by which two particles?

Answer 13

Neutrons; protons and neutrons.

Question 14

There are two types of ions. Identify them by name and their type of charge.

Answer 14

cations **+ **(positive) , anions are - (negative)

Question 15

The ground state electron configuration of any element can be determined by following three rules of electron filling. What are they and how do they determine the location of electrons in an atom?

Answer 15

Aufbau principle fill lower energy levels in sub levels before adding electrons to higher energy sublevels.

**Pauli exclusion **principle there is a maximum of two electrons per orbital, and they must have opposite spins.

**Huns rule **half filled orbitals of equal energy before pairing electrons in any one orbital in a given sub shell.

Question 16

State three properties of electromagnetic radiation

Answer 16

Frequency, wavelength, energy

Question 17

Name the three types of nuclear decay from least to most damaging to living tissues

Answer 17

Alpha, beta, gamma.

Question 18

One type of nuclear decay has three different modes. What are they?

Answer 18

Beta colon B- (normal beta decay), B+ positron emission, and EC electron capture

Question 19

What are the five periodic trends?

Answer 19

Atomic size, first ionization energy, electron affinity, electronegativity, acidity/basicity.

Question 20

What are three types of covalent bonds?

Answer 20

Normal (which can be polar or nonpolar), metallic, and coordinate covalent bonds.

Question 21

Give to other names for Lewis bases.

Answer 21

Ligand, nucleophile, or chelator

Question 22

What three geometric family names are associated with each type of hybridized orbitals?

Answer 22

Linear= Sp
Trigonal planar= sp2
Tetrahedral= sp3

Question 23

Name the various intermolecular forces from strongest weakest.

Answer 23

Hydrogen bonds > dipole-dipole forces > London dispersion forces.

Question 24

Give two examples of elements that do not obey the Aufbau principle.

Answer 24

Chromium (Cr) and it’s family members or copper (Cu) and it’s family members.

Question 25

Which electrons do transition metal atoms lose first when ionized?

Answer 25

Valance "S" electrons

Question 26

Explain the difference between paramagnetic and diamagnetic elements, and give an example of each.

Answer 26

**Paramagnetic** elements have unpaired electrons like nitrogen (N). **Diamagnetic **elements have all their electrons paired like Ne or any element with a field orbital sub shell.

Question 27

What happens to the spacing between successively higher energy levels in an atom as you move farther from the nucleus?

Answer 27

it decreases

Question 28

Describe each kind of nuclear decay

Answer 28

**A=** nucleus emits helium nucleus (two protons and two neutrons) **B- = **a neutron converts into a proton and the electron, e- which is emitted **B+ =** a proton converts into a neutron in the pro positron, e+ which is emitted **EC= **a proton in the nucleus captures an inner shell electron and converts it into a neutron. **gamma**= excited nucleus drops to a lower energy state by admitting a gamma photon

Question 29

What type of mathematical relationship is associated with all radioactive decay?

Answer 29

Radioactive elements decay exponentially with respect to time.

Question 30

Why is the mass of a nucleus not equal to the mass of the individual protons and neutrons that comprise it?

Answer 30

The binding energy that is released when the nucleons are bound together in the nucleus comes from the mass defect according to E=mc2

Question 31

Define each periodic trend

Answer 31

**Atomic radius**: extent of the valence electrons of an atom. **Ionization energy**: energy required to remove a mole of valence electrons from a mole of gaseous atoms of a given element. **Electron affinity: **Energy associated with adding a mole of electrons to the valence shell of a mole of gaseous atoms of a given element. **Electronegativity:** a measure of the amount of pull an atom has on shared valence electrons in a bond. **Acidity:** the tendency for a molecule to give up a hydrogen ion.

Question 32

Which three periodic trends follow the same pattern?

Answer 32

First ionization energy, electron affinity, and electronegativity. They are all inversely related to atomic size.

Question 33

What charge is generally associated with larger ions? And with smaller ions?

Answer 33

Generally, negative ions are larger and positive ions are smaller (than a neutral atom)

Question 34

Rank the colors of visible light in order from lowest frequency to highest.

Answer 34

By frequency Red< orange< yellow< green< blue< violet

Question 35

Rank in order of wave length, from shortest to longest, the regions of the EM spectrum.

Answer 35

By wavelength, gamma rays

Question 36

What are the key characteristics about photons an electron energy levels?

Answer 36

1. A product of the wavelength and frequency of a photon is equal to 3.0 x 10^8 m/s 2. The difference in energy between adjacent energy levels decreases as the energy level increase 3. Energy of a photon is directly proportional to its frequency

Question 37

Explain d subshell and whhy its backfilled

Answer 37

For an atom in the d block of period n, the d sub shell will have a principal quantum number of n-1. Transition metals ionize from their valence s sub shell before the d of shells. d5 and d10 subshell are stable.

Question 38

the correct electron configuration of Ge+?

Answer 38

[Ar] 4s2 3d10 4p1

Question 39

An excited electron drops down to its initial energy level within an atom and a photon is emitted. List characteristics about photons and electron energy levels

Answer 39

the product of the wavelength and frequency of a photon is equal to 3.0 × 10^8 m/s. the difference in energy between adjacent energy levels decreases as the energy levels increase. the energy of a photon is directly proportional to its frequency.

Question 40

In the ionization of titanium, which subshell will lose its electrons first and why?

Answer 40

The 4s subshell because it has the least stable orbitals.

Question 41

The energy of excitation is equal to________________

Answer 41

The energy of excitation is equal to the **energy of the emitted photon**

Question 42

Visible light

Answer 42

ROYGBIV 400-700

Question 43

What is a possible electronic structure for an excited Cu(I) ion?

Answer 43

[Ar] 3d^9 4p^1

Question 44

Beta decay is most likely to have what effect on atomic radius?

Answer 44

Decreased atomic radius due to increased effective nuclear charge

Question 45

anhydrous means___________

Answer 45

anhydrous means in the absence of water

Question 46

What happens to the electronic transition energy of the atoms as one moves down a family in the periodic table?

Answer 46

The first electronic transition energy of the atoms **decreases **as one moves down a family in the periodic table