unit 1: review of inorganic chem Flashcards
1
Q
involved in a variety of processes within the human body
A
metal ions
2
Q
an iron-containing metalloprotein which carries oxygen from the lungs to the various tissues around the human body
A
hemoglobin
3
Q
vital component of our bones
A
calcium
4
Q
Elements such _____, _____, _____, are essential for a variety of catalytic processes
A
- copper
- zinc
- manganese
5
Q
GROUP 1A
A
GROUP 1A - ALKALI METALS
- H
- Li
- Na
- K
- Rb
- Cs
- Fr
6
Q
GROUP IIA
A
GROUP IIA - ALKALINE EARTH METALS
- Be, Mg, Ca, Sr, Ba, Ra
7
Q
GROUP IIIA
A
GROUP IIIA - BORON FAMILY (Icosagens)
- B, Al, Ga, In, Tl
8
Q
GROUP IVA
A
GROUP IVA - CARBON FAMILY (Crystalogens)
- C, Si, Ge, Sn, Pb
9
Q
GROUP VA
A
GROUP VA (Pnictogens)
- N, P, As, Sb, Bi
10
Q
GROUP VIA
A
GROUP VIA - OXYGEN FAMILY (Chalcogens)
- O, S, Se, Te, Po
11
Q
GROUP VIIA
A
GROUP VIIA - HALOGENS (Salt-formers)
- F, Cl, Br, I, At
12
Q
GROUP VIIIA
A
GROUP VIIIA - NOBLE/INERT GASES/RARE GASES
- He, Ne, Ar, Kr, Xe, Rn
13
Q
IB
A
COINAGE METALS
- Cu, Ag, Au
14
Q
IIB
A
VOLATILE METALS
- Zn, Cd, Hg
15
Q
IIIB
A
SCANDIUM SUBGROUP
- Sc, Y, Lanthanides, Actinides
16
Q
IVB
A
TITANIUM SUBGROUP
- Ti, Zr, Hf,
17
Q
VB
A
VANADIUM SUBGROUP
- V, Nb, Ta
18
Q
VIB
A
CHROMIUM SUBGROUP
- Cr, Mo, W
19
Q
VIIB
A
Manganese Subgroup
- Mn, Tc, Re
20
Q
VIIIB
A
IRON TRIAD
1st triad: Fe, Co, Ni
2nd triad: Ru, Rh, Pd
3rd triad: Os, Ir, Pt
21
Q
The _______ of a metal in a biological environment depends on the concentration present in the living organism.
Some metal ions are essential for life.
- Concentrations too high can be highly toxic
- Concentrations too low can lead to ________ resulting in disturbed biological processes.
A
toxicity
- disturbed
22
Q
__________: visualizes the relationship between the physiological response and the metal concentration.
A
Bertrand diagram
23
Q
Why use metal-based drugs?
Metal complexes exhibit unique properties, which allow metal ions to interact with biomolecules, and allow scientists to safely administer even toxic metal ions to the human body.
The ability to be involved in __________________ has led to the use of metal complexes in _______________.
In particular, _________ are able to coordinate to electron-rich biomolecules such as DNA. This can lead to the deformation of DNA and ultimately to _______. Therefore, transition metals are under scrutiny as potential ________.
A
- redox oxidation reactions
- photodynamic therapy (PDT)
- transition metals
- cell death
- anticancer agents
24
Q
- Metals that display a magnetic moment can be used as imaging reagents in ___________.
- Many metals have radioactive isotopes, which can be used as so-called __________ for therapy and imaging.
A
- magnetic resonance imaging (MRI)
- radiopharmaceutical
25
- Formation of ionic species due to transfer of electrons between atoms.
- Forming an anion (negatively charged) and a cation (positively charged), which form a strong bond based on ___________.
bond
- electrostatic attraction
26
The bonding situation in ________ bonded molecules was described as a sharing of valence electrons.
Nowadays, chemical bonding is mainly explained by the application of wave mechanics and described either by the valence bond (VB) or molecular orbital (MO) theory.
- covalently
27
__________: defined as an attraction between atoms, which leads to the formation of chemical substances containing two or more atoms.
__________: a result of the electrostatic attraction between opposite charges, such as electrons or nuclei or dipole attraction.
The forces behind this attraction are ___________ of varying degrees, ranging from weak dipole interactions to strong attraction between opposite charges. Strong bonds are ionic bonds and covalent bonds, whilst weak chemical bonding can be observed where _________ and _________ is seen.
- chemical bond
- bond
- electrostatic forces
- dipole interaction and hydrogen bonding
28
_________: used to simply describe how valence electrons are arranged in molecules and how they are involved in chemical bonds.
* Dots are used to visualize the number of valence electrons
* Elemental symbol represents the nuclei.
* Electrons should be ruled. Paired electrons are sometimes also represented by a line, which can be interpreted as a single covalent bond.
* An element with a single electron represents a radical.
* Electron pairs not contributing to any bonds are called lone pairs
Lewis structures
29
___________: rules are a set of rules used to predict the shape of a molecule.
The basic principle is that valence electrons around the center atom repel each other and therefore will form an arrangement in which they are situated furthest from each other.
VSEPR (Valence Shell Electron Pair Repulsion)
30
Double and triple bonds are seen the same as single bonds.
The resulting geometry depends on the number of binding and nonbinding electron pairs, which can be summarized as the _________
- B represents a covalent bond atom or group.
- _______ occupy slightly more space than binding electron pairs, which explains the smaller angle in water of ______ rather than the standard tetrahedral angle of 108.90.
steric number
- Lone pairs
- 104.9°
31
__________: this type of binding is very important for biological actions of various elements.
- defined as a chemical bond that is based on the sharing of electrons
- Often, this leads to full outer shells for the binding partner to obtain the noble gas configuration.
covalent bond
32
- Within homonuclear species (chemical bond occurs between two atoms of _______ element), the binding electron pair is evenly distributed between the two partners.
- In a heteronuclear species (chemical bond occurs between two atoms of ________ elements), the electrons are more attracted/polarized to one partner than the other, depending on the so-called ____________
- same
- different
- electronegativity (EN).
33
describes the tendency of an atom to attract electrons or electron density towards itself.
Electronegativity
34
________: describes the formation of a covalent bond as the overlapping of two half-filled valence (Atomic Orbitals) AOS from each binding partner, which contains one electron each.
The simplest example is: Hydrogen, has only one valence electron (1s1), and therefore two hydrogen 1s orbitals filled with one electron (1s1), can overlap and form a chemical bond
The VB theory
35
_________: approaches chemical binding from a more advanced point of view, where MOS are formed covering the whole molecule.
molecular orbital theory
36
- strong bonds based on the ________ of electrons between the atoms and the resulting electrostatic attraction between the negatively and positively charged bond partners
ionic bond
- transfer
37
The term _____ is used for atoms or molecules in which the total number of electrons is different from the number of protons and therefore carries a ________ charge.
An anion has a negative charge, a cation has a positive charge.
- ion
-
38
_________: strong but short-range bonds
- have no defined direction in space
- they are 'only' the result of electrostatic attraction
- these attractions are not only limited to one directional partner each but also with each ion around them.
- As a result, a whole network of ions will be formed with anions and cations occupying specified spaces.
- The result is called a ________, which typically have high melting points
- lonic bonds
- specified spaces
39
_________: most commonly described as a type of chemical bond where the metal atom donates its valence electrons to a 'pool' of electrons that surrounds the network of metal atoms.
Electrons are NOT anymore identified with one particular atom but are seen as DELOCALIZED over a wide range.
This is a VERY STRONG type of chemical bond.
Electrical and thermal conductivity as well as malleability of metals can be explained using this model.
metallic bond
40
After discussing intramolecular forces (_____________ molecules) such as covalent bonding, it is also important to be aware of the interactions between molecules, the so-called __________.
These forces are much _______ than any of the types of binding discussed previously.
Intermolecular Forces
- intermolecular force
- weaker
1. van der waals force
2. dipole-dipole interaction
3. hydrogen bonding
41
__________: weakest forces occurring between molecules.
- found between molecules that do not have a ___________.
- Electrons are not static but move around, and therefore moments occur when the electron distribution is not even, leading to the formation of _____________
- these dipoles cause a ___________ in the neighboring molecules.
As a result, molecules are (weakly) attracted to each other.
van der Waals force
- permanent dipole
- temporary dipoles
- polarization
42
__________: an electrostatic interaction of permanent dipoles.
In ________ molecules, a polarization of the bond is caused by the difference in electronegativity between the two atoms forming the _________ bond.
This leaves a partially positive charge (6+) on the less electronegative partner and, formally, a partially negative charge (8-) on the more electronegative partner.
These molecules are attracted to each other as they can align in such way that opposite charges are next to each other, leading to ___________ forces between the molecules
Dipole-dipole interaction
- heteronuclear
- covalent
- intramolecular
43
__________: strongest of the intermolecular forces and seen as the particularly strong electrostatic interactions occurring between molecules of the type H-X.
X is an electronegative atom such as F, O or N.
O and N have also the advantage of possessing lone-pair orbitals.
- can be seen as a strong and specialized form of ___________ and is the reason for the high boiling point of water
Hydrogen bonding
- dipole-dipole interaction
