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Sem1 > Gen chem F > Flashcards

Gen chem F Flashcards

I love how warm she is

1
Q
  • Energy needed to remove an electron from an atom or ion in its ground state.
  • During the removal of electrons, one electron is removed from the atom at a time.
  • Energy needed to remove the first valence electron from an atom is called the first ionization energy
A

Ionization energy

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2
Q

A model of the atom that derives from the Schrödinger wave equation and deals with probabilities. wave function: Give only the probability of finding an electron at a given point around the nucleus.

A

The quantum mechanic model

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3
Q
  • Ability of an atom in a chemical bond to attract electrons toward itself and is usually measured in electron volt (ev).
  • The higher the Ea, the greater the ability of an atom to pick up electrons
A

Electronegativity(EN)

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4
Q
  • Also called azimuthal quantum number.
  • Describes the shape of the orbital
  • Orbitals have shapes that are best described as spherical (I = 0), dumb bell (I = 1), or cloverleaf (I = 2). They can even take on more complex shapes as the value of the ??? number becomes larger.
  • Each value of / indicates a specific s, p, d, f subshell (each unique in shape.) The value of (/)is dependent on the principal quantum number.
A

Angular quantum number (/)

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5
Q

distance of the electron from the nucleus

A

principal

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6
Q

Consists of the s- and p-block elements.These elements are under Groups 1, 2, 13, 14, 15, 16, 17, and 18.

A

Representative elements (or main group elements)

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7
Q
  • Described values of quantities of a quantum system* An important aspect of quantum mechanics is the quantization of observable quantities, which is possible through ??? since they are discrete set of integers and half-integers.
A

Quantum numbers

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8
Q

Energy level or shell

A

principal quantum number

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9
Q
  • Composed of Representative Elements and Noble Gas Family.
    *The name comes from the fact that these elements are unreactive towards other elements or compounds. (8 electrons in the outer shell)
  • It is called representative elements because the number of an element represents or is equal to the number of valence electron
A

Group A (IA-VIIA)

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10
Q

In 1926, said that electron is a wave and tries to describe the regions in space, or orbitals, where electrons are most likely to be found.

A

Erwin Schrodinger

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11
Q

The f-block elements that are in Period 6 are called, ??? (since these elements are found after lanthanum in the periodic table), while those in Period 7 are called ???, as they come after actinium

A

lanthanides and actinides

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12
Q

orientation of the electron spin

A

spin

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13
Q

Consists of elements arranged in order of increasing atomic number

A

Periodic table

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14
Q

increases from left to right across a period, and decreases from top to bottom within a group

A

electron affinity

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15
Q
  • Refers to the change in energy when an atom in its ground state gains an electron forming an anion.
  • Nonmetals always form an anion because they have high electron affinity.
A

Electron affinity

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16
Q

Elements belonging to the d-block are called ???. It consists of elements under Groups 3 to 12

A

transition elements

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17
Q

■ The electrons in an atoms have energy levels that can be described by four types of quantum numbers.
The four types of quantum numbers.

A
  1. Principal quantum number
  2. Angular quantum number
  3. Magnetic quantum number
  4. Electron spin quantum number
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18
Q

increases from left to right across a period, and decreases from top to bottom within a group

A

Electronegativity

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19
Q

Orbital must be filled in first by a single electron before pairing up

A

Hund’s Rule

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20
Q

*The periodic number of an element (horizontal arrangement) corresponds to the highest energy level occupied by an element’s electron.
* A horizontal row of elements.
* Have varying physical and chemical properties

A

PERIOD or SERIES

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21
Q
  • A vertical column of elements.
  • Elements in the same group often have similar chemical and physical properties
A

Group or family

22
Q

shape of the orbital

A

angular

23
Q

subshell

A

angular quantum number

24
Q

discovered the existence of electrons in 1897 and proposed the plum pudding model, through which he suggested that electrons are randomly distributed throughout the atom.

A

J.J thomson

25
Q

first few main energy level act as a shield of valence electrons from the nuclear force

A

shielding effect

26
Q

In 1913, stated that the nucleus is surrounded by electrons in defined orbits as shown in Bohr Model.

A

Neil Bohr

27
Q
  • Also known as electrovalent bond
    *Type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound.
  • Compound formed by ionic or electrovalent bond is called ??? compound
A

ionic bond

28
Q
  • Unlike n, I, and ml, the electron spin quantum number ms does not depend on another quantum number.
  • It designates the direction of the electron spin and may have a spin of +1/2, represented by (arrow up) or -1/2 represented by (arrow down) This means that when ms is positive the electron has an upward spin, which can be referred to as “spin up.” When it is negative, the electron has a downward spin, so it is “spin down.”
A

Electron spin quantum number(ms)

29
Q
  • Group VIIIA (group O) are the most stable atoms in the periodic table.
  • They comply with the ??? rule (except He)
  • This rule states that atoms tend to combine in such way that they each have eight electrons
A

octet rule (Gilbert Lewis)

30
Q

It describes the properties of molecules and atoms, particularly the electrons, protons, neutrons and their esoteric particles.

A

quantum mechanics

31
Q
  • This describes the orientation of the electron cloud. The value of m_{l} depends on the value of /. the range of m_{l} values range form -/ to +/. Therefore, it can be a negative integer, zero or a positive integer
A

Magnetic quantum number (mj)

32
Q

Electrons mus occupy the lowest available subshell first.

A

Aufbau’s principle

33
Q

In 1927, proposed the ??? uncertainty principle which states that it is not possible to predict the position and momentum of a particle given at a time

A

Werner Heisenberg

34
Q
  • Includes transition metals, Lanthanides, and Actinides.
  • Lanthanides - atomic numbers 57 to 71.
  • Actinides - atomic numbers 89 to 103
  • Transition Metals - connect the left and right sides of the periodic table.
A

Group B (IB-VIIIB, Lanthanides, Actinides)

35
Q

➤States that no two identical electrons may occupy the same quantum state in an atom simultaneously. Thus, no two electrons in an atom can have exactly the same set of quantum numbers.

A

Pauli’s exclusion principle

36
Q

??? elements are those that can loose electrons and form positive ions (cation). Increases from top to bottom, and decreases from right to left

A

mentallic characters

37
Q

*Represents the distance of the electrons from the nucleus, and hence, the atomic size.
*It is denoted by the symbol n and takes positive integer values only
*a.k.a “shell”
*A higher n-value indicates a large atom

A

Principal quantum number (n)

38
Q

orientation of the orbital

A

magnetic

39
Q

f,d,p,s electrons?

A

f14,d10,p6,s2

40
Q

It is a science that deals with the processes that affect the behavior of matter and light in atomic and subatomic scales

A

quantum mechanics

41
Q

Elements arranged vertically in the periodic table fall into two big groups, namely, group A and group B.

A

S and P block group A and D block in groub B

42
Q

value of / in designated orbital/subshell

A

s0,p1,d2,f3

43
Q

tends to increase from bottom to the top, and increase from left to right

A

Ionization energy

44
Q

While some elements are classified as either metals or nonmetals, there are some with both metallic and nonmetallic properties; these are called metalloids or semimetals. The periodic table on the right shows which among the elements are metals, nonmetals, and metalloids. Note that metalloids serve as boundaries for metals and nonmetals. Note that hydrogen is the only nonmetal positioned together with the metals

A

metallic properties

45
Q

The current periodic table is based on the arrangement proposed by ???, a Russian chemist. Modifying pre-existing arrangement of elements based on similarities in properties, ??? clustering of elements was able to predict properties of elements that were discovered later on.

A

Dmitri Mendeleev

46
Q

??? elements that can gain electrons and form negative ions (anion). Increases from bottom to the top, and increases from left to right.

A

Non-metallic character

47
Q

discovered the nucleus in 1911 using gold foil experiment

A

Ernest Rutherford

48
Q
  1. lose electrons to form cation and 2. gain electrons to form anion
A

1.metals 2.nonmetals

49
Q
  • A useful way to illustrate the octet rule.
  • Represents the number of electrons in the outermost shell of the atom using dots.
A

The Lewis structure

50
Q

name of s,p,d,f

A

sharp
principal
diffuse
fundamental

51
Q

The elements in the periodic table are also clustered based on their metallic properties— ductile, malleable, relatively high melting point, good conductor of heat and electric current, etc

A

Metallic Properties

52
Q

orientation of the subshell

A

spin of the electron

Sem1 (12 decks)

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