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Organic and Inorganic Chemistry > Chapter 1- Atomic structure and chemical bonding > Flashcards

Chapter 1- Atomic structure and chemical bonding Flashcards

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1
Q

A subatomic particle, symbol p or p+, with a positive electric charge of +1 elementary charge and a mass slightly less than that of a neutron.

A

Proton

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2
Q

A subatomic particle, symbol n or n0, with no net electric charge and a mass slightly larger than that of a proton.

A

Neutron

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3
Q

It plays as an essential role in numerous physical phenomena, such as electricity, magnetism, chemistry and thermal conductivity, and they also participate in gravitational, electromagnetic and weak interactions.

A

Electron

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4
Q

It represents the number of protons in the nucleus of an atom.

A

Atomic number

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5
Q

The total number of protons and neutrons in the nucleus of an atom.

A

Mass number

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6
Q

Atoms of the same element having the same atomic number but different atomic masses.

A

Isotopes

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7
Q

Atoms of different elements having the same mass number but different atomic numbers.

A

Isobars

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8
Q

Atoms of different elements having the same number of neutrons but differ in atomic numbers and mass numbers.

A

Isotones

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9
Q

It is the space around the nucleus in which the electron is found with a probability of 90%.

A

Orbital

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10
Q

The number of electrons in an atom are arranged in shells or ‘energy levels’ around the nucleus

A

Shells

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11
Q

Electrons are those seen in the previous noble gas and any completed transition series. They fill all the lower energy levels of an atom.

A

Inner (core) electrons

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12
Q

Are those in the highest energy level (highest n value). They spend most of their time farthest from the nucleus.

A

Outer electrons

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13
Q

Involved in forming compounds. Among the main group elements, the valence electrons are the outer electrons.

A

Valence electrons

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14
Q

It is a region of space within an electron shell that contains electrons that have the same energy.

A

Subshell

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15
Q

Describes the size of orbitals and relative distance of the electrons from the nucleus.

A

Principal quantum number

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16
Q

This refers to the shape of the orbitals.

A

Angular momentum quantum number

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17
Q

Refers to the orientation of the orbitals in space around the nucleus.

A

Magnetic quantum number

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18
Q

Describes the spin of electrons in an orbital which is opposite direction to differentiate one electron from the other in the same orbital.

A

Spin quantum number

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19
Q

The distribution of electrons in the energy levels and sublevels of an atom

A

Electron configuration

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20
Q

The number of different states of equal energy.

A

Degree of degeneracy or degeneracy

21
Q

Electron orbitals that have the same energy levels.

A

Degenerate orbitals

22
Q

A property of a substance to be slightly attracted to a magnetic field. It is exhibited by substances that contain one or more unpaired electrons.

A

Paramagnetism

23
Q

A property of a substance to be slightly repelled by a magnetic field. It is exhibited by substances whose electrons are all paired.

A

Diamagnetism

24
Q

Electrons first occupy the lowest energy orbitals available to them; only when the lower-energy orbitals are filled that they enter higher–energy orbitals.

A

Aufbau (building–up) principle

25
Q

Only two electrons having opposite spins can occupy an orbital. The third electron will eventually be repelled.

A

Pauli’s exclusion principle

26
Q

Electrons distribute singly before pairing.

A

Hund’s rule

27
Q

These gases have complete e- configuration of ns2np6 except for He making them difficult to either gain or loss electrons.

A

Electron configuration of noble gases

28
Q

The arrangement of electrons around the nucleus of an atom with lower energy levels.

A

The ground state

29
Q

Any state other than the ground state of an atom or molecule; a state that has higher energy than the ground state.

A

Excited state-

30
Q

An elevation in energy level above an arbitrary baseline energy state.

A

Excitation

31
Q

The electrostatic force which holds the atoms in a compound or molecule. This results from the gain and loss of electrons, or from the sharing of electrons between atoms.

A

Chemical bond-

32
Q

The ability of an atom to form bonds.

A

Valance.

33
Q

States that atoms are most stable when they have a full shell of electrons in the outside electron shell.

A

Octet rule

34
Q

It is a chemical bond resulting from the mutual attraction of oppositely charged ions.

A

Ionic bonding

35
Q

Formed from the force of electrostatic attraction between oppositely charged ions (cations and anions).

A

Ionic bonding

36
Q

It is an electrically charged atom of an element or group of atoms that carries an electrical charge.

A

Ion

37
Q

It is a positively charged atom of an element. It is formed when an atom loses electron (s).

A

Cation

38
Q

A negatively charged atom of an element. It is produced when an atom gains electron(s).

A

Anion

39
Q

Formed when atoms share a pair of electrons to form covalent molecules.

A

Covalent

40
Q

Bond formed when the combining atoms have a big difference in their electronegativity values, and that the sharing of the electrons is not equal.

A

Polar covelant bond

41
Q

This type of bond is formed from the combination of atoms of the same element or atoms whose electronegativity values are very close.

A

Non-polar covalent bond

42
Q

A type of covalent bond where the two electrons in the bond are only donated by a single atom.

A

Coordinate covalent bond

43
Q

Shows the valence electrons in an element.

A

Lewis structure

44
Q

States that the bond energy is inversely related to the bond length (r), and so factors which influence a bond’s strength influence its length.

A

Coulomb’s law

45
Q

The number of electrons that an atom will lose or gain in order to get stable electronic configuration in forming ionic bond.

A

Electrovalency

46
Q

The number of electrons that an atom can share to get a stable electronic configuration.

A

Covalency:

47
Q

The energy required to remove an electron from a neutral atom.

A

Ionization potential

48
Q

The energy released when an atom gains one electron to the element.

A

Electron affinity

49
Q

A measure of the ability of an atom in a molecule to attract electrons to itself.

A

Electronegativity

Organic and Inorganic Chemistry (4 decks)

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