Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

20k3 > Chem class 1 > Flashcards

Chem class 1 Flashcards

1
Q

Alpha Decay

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Beta- Decay

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Beta+ Emitter

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Gamma decay

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Electron capture

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

diamagnetic

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Paramagnetic

A

Is when an atoms electrons are not all spin paired.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

periodic table group 1

A

alkali metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

periodic table group 2

A

Alkaline earth metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

periodic table group 7

A

Halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

periodic table group 8

A

Noble gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Proton determines element identity, neutron, electron.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

Neutrons; protons and neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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?

A

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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

State three properties of electromagnetic radiation

A

Frequency, wavelength, energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

Alpha, beta, gamma.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are the five periodic trends?

A

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

20
Q

What are three types of covalent bonds?

A

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

21
Q

Give to other names for Lewis bases.

A

Ligand, nucleophile, or chelator

22
Q

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

A

Linear= Sp
Trigonal planar= sp2
Tetrahedral= sp3

23
Q

Name the various intermolecular forces from strongest weakest.

A

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

24
Q

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

A

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

25
Q

Which electrons do transition metal atoms lose first when ionized?

A

Valance “S” electrons

26
Q

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

A

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.

27
Q

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

A

it decreases

28
Q

Describe each kind of nuclear decay

A

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

29
Q

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

A

Radioactive elements decay exponentially with respect to time.

30
Q

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

A

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

31
Q

Define each periodic trend

A

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.

32
Q

Which three periodic trends follow the same pattern?

A

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

33
Q

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

A

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

34
Q

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

A

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

35
Q

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

A

By wavelength, gamma rays <x-rays< ultraviolet< visible light< infrared< microwaves< radio waves.

36
Q

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

A
  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
37
Q

Explain d subshell and whhy its backfilled

A

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.

38
Q

the correct electron configuration of Ge+?

A

[Ar] 4s2 3d10 4p1

39
Q

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

A

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.
40
Q

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

A

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

41
Q

The energy of excitation is equal to________________

A

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

42
Q

Visible light

A

ROYGBIV

400-700

43
Q

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

A

[Ar] 3d^9 4p^1

44
Q

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

A

Decreased atomic radius due to increased effective nuclear charge

45
Q

anhydrous means___________

A

anhydrous means in the absence of water

46
Q

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

A

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

20k3 (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions