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BS11001-Biomolecules > The Periodic Table, Atoms and Ions > Flashcards

The Periodic Table, Atoms and Ions Flashcards

1
Q

How are elements ordered in the periodic table?

A

Elements are listed in order of increasing atomic number

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2
Q

Where are elements with similar properties placed in a periodic table?

A

Elements with similar properties are placed in the same column(Group)

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3
Q

What is the Atomic Number?

A

The Atomic Number is the number of protons in the nucleus

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4
Q

What is the Atomic Mass?

A

The Atomic Mass is the number of protons and neutrons in the nucleus

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5
Q

What does a Chemical element consist of?

A

A chemical element consists of atoms with the same number of protons

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6
Q

What is an isotope?

A

Isotopes are forms of an element that have the same atomic number but different number of neutrons

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7
Q

How many elements are required for a human to conduct a healthy life?

A

Humans need 25 elements to conduct a healthy life

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8
Q

What is periodicity?

A

Periodicity is the name given to the gradual change of physical and chemical properties in elements in the same group

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9
Q

What is an element?

A

An element is a single substance that cannot be split into any separate substances by chemical means

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10
Q

What is the smallest unit an element can exist in?

A

The smallest unit an element can exist in is an atom

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11
Q

What is an atom?

A

An atom is defined as the smallest particle into which an element can be divided

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12
Q

What are the subatomic particles?

A

The subatomic particles are; Protons, Neutrons and Electrons

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13
Q

What charge does a proton carry?

A

A proton carries a single positive charge

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14
Q

What charge does an electron carry?

A

An electron carries a single negative charge

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15
Q

What charge does a neutron carry?

A

A neutron carries no charge

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16
Q

What happens if the number of electrons is different from the number of protons?

A

If the number of electrons is different to the number of protons, a charged ion is formed

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17
Q

What happens if an ion gains one or more electrons?

A

If an atom gains one or more electrons, it becomes a negative ion, known as an Anion

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18
Q

What happens if an atom loses one or more electrons?

A

If an atom loses one or more electrons, it becomes a positive ion, known as a Cation

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19
Q

What does an elements ionization energy tell us?

A

An elements ionisation energy tells us how readily the element will lose an electron to become a positively charged ion

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20
Q

Elements on the left of the periodic table have what type of ionization energy?

A

Elements on the left side of the periodic table have relatively low ionization energies, and readily form positively charged ions

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21
Q

Elements on the right of the periodic table have what type of ionization energy?

A

Elements on the right side of the periodic table have relatively high ionization energies, and are very unlikely to form positively charged ions. Instead, they readily form negatively charged ions by accepting an electron

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22
Q

What is the difference between isotopes of the same element?

A

Different isotopes of the same element have different mass numbers but retain the same atomic number

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23
Q

What is an elements relative atomic mass?

A

An elements relative atomic mass is a measure of the average mass of an atom of that element

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24
Q

What types of atomic orbital are there?

A

There are 4 different types of atomic orbitals:
S orbitals
P orbitals
D orbitals
F orbitals

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25
Q

What are orbitals grouped into?

A

Orbitals are grouped into shells

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26
Q

What are equivalent orbitals occupying the same shell grouped into?

A

Equivalent orbitals occupying the same shell are grouped into subshells

27
Q

What happens when the electrons in the atom are further away form the nucleus?

A

Electrons have progressively higher energy as the distance from the nucleus of the shell they occupy increases

28
Q

What orbitals are filled first? Low energy or High Energy?

A

Low energy orbitals become filled with electrons before high-energy orbitals

29
Q

What are degenerate orbitals?

A

Degenerate orbitals are orbitals that have the same energy levels

30
Q

How are degenerate orbitals filled?

A

Each degenerate orbital in a subshell must be occupied by one electron before any one of the orbitals becomes completely filled

31
Q

What is the valence shell?

A

The valence shell is the shell furthest from the nucleus

32
Q

What are electrons contained in the valence shell called?

A

Electrons held in the valence shell are known as valence electrons

33
Q

What do the elements from the same group have in common?

A

Elements from the same group in the periodic table have the same number of Valence Electrons

34
Q

What can happen when an atom absorbs energy?

A

When an atom absorbs energy, electrons can jump between orbitals of different energy

35
Q

What is the energy of electromagnetic radiation determined by?

A

The energy of electromagnetic radiation is determined by its wavelength

36
Q

What wavelength does high-energy radiation have?

A

High-energy radiation has a short wavelength

37
Q

What wavelength does low-energy radiation have?

A

Low-energy radiation has a long wavelength

38
Q

What is the bond length?

A

The bond length is the sum of the atomic radii of two covalently bonded atoms

39
Q

What is the atomic radius

A

The atomic radius is half the distance between the nuclei of two identical atoms, when joined by a single covalent bond

40
Q

What does VSEPR Theory stand for?

A

Valence Shell Electron Pair Repulsion

41
Q

How do you use the VSEPR Theory?

A

To use VSEPR theory, we count the number of pairs of bonding electrons plus the number of non-bonding pairs around the central atom

42
Q

What type of bond does a single bond contain?

A

A single bond contains 1 sigma bond

43
Q

What type of bonds does a double bond contain?

A

A double bond contains 1 sigma bond and 1 pi bond

44
Q

What type of bonds does a triple bond contain?

A

A triple bond contains 1 sigma bond and 2 pi bonds

45
Q

What do we need to consider when using VSEPR theory to predict molecular shape in compounds containing double and triple bonds?

A

We only need to consider the number of valence electrons occupying single bonds

46
Q

What does the arrangement of Valence Electrons predicted by VSEPR theory occur from a result of?

A

The arrangement of Valence Electrons predicted by VSEPR theory occurs as a result of the hybridization of atomic orbitals to form hybrid orbitals

47
Q

What undergoes overlap to form single covalent bonds?

A

It is the Hybrid Orbitals that undergo overlap to form single covalent bonds

48
Q

The number of hybrid orbitals formed after hybridization is equal to what?

A

The number of atomic orbitals undergoing hybridization

49
Q

What happens when one s and three p orbitals undergo sp^3 hybridization?

A

They form four sp^3 hybrid orbitals with tetrahedral geometry; They can participate in 4 sigma bonds

50
Q

What happens when one s and two p orbitals undergo sp^3 hybridization?

A

They form three sp^3 hybrid orbitals with typical planar geometry; They can participate in 3 sigma bonds

51
Q

What happens when one s and one p orbitals undergo sp^3 hybridization?

A

They form two sp^3 orbitals with linear geometry; They can participate in 2 sigma bonds

52
Q

What undergoes overlap to form pi bonds?

A

Unhybridized orbitals overlap to form pi bonds

53
Q

What can be treated as being equivalent when atomic orbitals hybridize

A

Non-bonding pairs of valence electrons and bonding pairs of valence electrons(sigma bonds) can be treated as being equivalent

54
Q

What does a molecules configuration describe?

A

A molecules configuration describes how its composite atoms are joined together, and is fixed

55
Q

What does a molecules conformation describe?

A

A molecules conformation describes how its composite atoms are arranged at particular moments in time, and is variable

56
Q

Where is rotation not possible?

A

Rotation is not possible about double or triple bonds, or where delocalization occurs

57
Q

What is steric hindrance?

A

Steric Hindrance is the restriction of movement due to a lack of space between neighbouring atoms

58
Q

What shape are Porphyrins?

A

Porphyrins are ring-shaped

59
Q

What can pigments derived from porphyrins be called?

A

Porphyrin-derived pigments can be called the “colours of life”.
In the sense that these rings are necessary to sustain key activities in nearly all organisms

60
Q

What enzyme is the last enzyme before a major breaking point in the synthesis of the “rings of life”

A

Protoporphyrin oxidase

61
Q

Where is protoporphyrin oxidase bound to in Animal cells?

A

In Animal cells, protoporphyrin oxidase is bound to the inner membrane of mitochondria

62
Q

What do non-bonding pairs do to a greater extent that bonding pairs?

A

Non-bonding pairs repel neighbouring valence electrons to a greater extent than bonding pairs, making bond angles smaller than we would otherwise expect for a given geometry

63
Q
A

BS11001-Biomolecules (5 decks)

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