Periodic Trends Flashcards: Atomic Radius, Ionization Energy & Electronegativity
Review 88 concise cards on atomic and ionic radius, shielding, effective nuclear charge, ionization energy, electron affinity, electronegativity, metallic character, exceptions, and comparisons.
O tej talii
Periodic Trends Flashcards: Atomic Radius, Ionization Energy & Electronegativity
Study the core periodic trends with 88 independently written English flashcards for high-school and introductory-college chemistry. The deck separates broad patterns from the reasons behind them and uses generally where real configurations create exceptions.
What the cards practice
The sequence covers four useful recall paths: term to definition; table movement to a general property direction; cause to effect through shell number, shielding, distance, and effective nuclear charge; and a concrete pair or isoelectronic set to the expected comparison. Atomic and ionic radius, first and successive ionization energies, electron affinity, electronegativity, metallic character, and selected reactivity links are all included.
The course-level exceptions are deliberately small: Be versus B, Mg versus Al, N versus O, P versus S, and Cl versus F electron affinity. Electron-affinity wording distinguishes a favorable electron gain from the sign convention used by a source. Electronegativity stays tied to bonded atoms, and ionic-radius comparisons state when an isoelectronic rule applies.
Learning order
Definitions and table structure come first. General directions follow, then causal models, ion-size rules, successive-ionization reasoning, limited exceptions, and applied comparisons. Related prompts are spaced apart in a fixed order; the review scheduler handles longer-term interleaving after installation.
Scope
This deck teaches qualitative periodic-trend reasoning. It excludes exact numerical property tables, memorizing values for all 118 elements, advanced transition-metal irregularities, diagonal relationships, melting and boiling trends, broad group trivia, and copied examination or competitor material. It supports chemistry practice but does not replace calculation, laboratory, or full-course problem solving.
Sources and license
Core trends and explanations were checked against OpenStax Chemistry: Atoms First 2e, section 3.5 and its electronegativity discussion in section 4.2. Terminology was cross-checked against the IUPAC Gold Book entries for ionization energy, electron affinity, and electronegativity.
The prompts, answers, examples, organization, metadata, and generated cover were created independently from common chemistry knowledge and original work. No protected cards, textbook prose, source figures, exact property tables, logos, or third-party media were copied.
The Common knowledge · CC0 1.0 label applies only to the original prompts, answers, examples, organization, metadata, and cover, to the extent applicable rights exist. It does not claim ownership of scientific facts or third-party material.
Source review date: August 29, 2026.
Karty w tej talii
Karta 1
Pytanie
What is a periodic trend?
Odpowiedź
A recurring pattern in element properties as atomic number increases across periods and down groups.
Karta 2
Pytanie
What does covalent radius measure?
Odpowiedź
Half the distance between the nuclei of two identical atoms joined by a covalent bond.
Karta 3
Pytanie
What is first ionization energy?
Odpowiedź
The minimum energy needed to remove the most loosely bound electron from an isolated gaseous atom in its ground state.
Karta 4
Pytanie
What is electronegativity?
Odpowiedź
An atom's ability to attract shared electrons toward itself in a chemical bond.
Karta 5
Pytanie
What is a period on the periodic table?
Odpowiedź
A horizontal row. For main-group elements, moving across a period fills orbitals in the same principal electron shell.
Karta 6
Pytanie
What is ionic radius?
Odpowiedź
A measure of an ion's size, usually inferred from distances between ions in crystals.
Karta 7
Pytanie
What does electron affinity describe?
Odpowiedź
The energy change when an electron is added to an isolated gaseous atom to form a gaseous anion.
Karta 8
Pytanie
What does metallic character describe?
Odpowiedź
How readily an element shows metallic behavior, especially losing valence electrons and forming cations.
Karta 9
Pytanie
What is a group on the periodic table?
Odpowiedź
A vertical column. Main-group elements in one group usually share a valence-electron pattern and similar chemistry.
Karta 10
Pytanie
What is effective nuclear charge?
Odpowiedź
The net positive pull an electron feels from the nucleus after shielding and electron–electron repulsion are taken into account.
Karta 11
Pytanie
What are successive ionization energies?
Odpowiedź
The energies needed to remove electrons one after another from the same atom, then from its increasingly positive ions.
Karta 12
Pytanie
How does electronegativity difference relate to bond polarity?
Odpowiedź
A larger difference generally produces a more uneven electron distribution and a more polar bond.
Karta 13
Pytanie
Why do main-group elements in one group often behave similarly?
Odpowiedź
They have the same general number and arrangement of valence electrons, which drive much of their bonding and reactivity.
Karta 14
Pytanie
What is electron shielding?
Odpowiedź
The reduction in nuclear attraction felt by an electron because other electrons lie between it and the nucleus and repel it.
Karta 15
Pytanie
Why does the definition of ionization energy specify a gaseous atom?
Odpowiedź
It isolates the atom from bonding and intermolecular effects, so the energy reflects electron removal from that species itself.
Karta 16
Pytanie
Where are metals and nonmetals generally found on the periodic table?
Odpowiedź
Metals occupy the left and center; nonmetals cluster toward the upper right, with metalloids near the boundary.
Karta 17
Pytanie
What changes in the electron arrangement across a main-group period?
Odpowiedź
Electrons are added to the same principal shell while the nucleus gains one proton from one element to the next.
Karta 18
Pytanie
How does atomic radius generally change from left to right across a period?
Odpowiedź
It decreases.
Karta 19
Pytanie
How does first ionization energy generally change from left to right across a period?
Odpowiedź
It increases, although a few recurring subshell and electron-pairing exceptions interrupt the rise.
Karta 20
Pytanie
How does electronegativity generally change from left to right across a period?
Odpowiedź
It increases for the elements normally assigned electronegativity values.
Karta 21
Pytanie
What changes in the electron arrangement down a main-group group?
Odpowiedź
Each step adds a higher principal electron shell while preserving a similar valence-electron pattern.
Karta 22
Pytanie
How does atomic radius generally change down a group?
Odpowiedź
It increases.
Karta 23
Pytanie
How does first ionization energy generally change down a group?
Odpowiedź
It decreases.
Karta 24
Pytanie
How does electronegativity generally change down a group?
Odpowiedź
It decreases.
Karta 25
Pytanie
How does effective nuclear charge generally change across a main-group period?
Odpowiedź
It increases because nuclear charge rises while added electrons enter the same principal shell and do not fully shield one another.
Karta 26
Pytanie
How does a cation's radius compare with its neutral parent atom?
Odpowiedź
The cation is smaller.
Karta 27
Pytanie
How does electron addition generally change across a period?
Odpowiedź
It generally becomes more energetically favorable toward the right, but electron affinity has substantial exceptions and depends on the sign convention used.
Karta 28
Pytanie
How does metallic character generally change from left to right across a period?
Odpowiedź
It decreases.
Karta 29
Pytanie
Why are valence electrons generally farther from the nucleus down a group?
Odpowiedź
They occupy shells with higher principal quantum numbers, so the electron cloud extends farther outward.
Karta 30
Pytanie
How does an anion's radius compare with its neutral parent atom?
Odpowiedź
The anion is larger.
Karta 31
Pytanie
How does favorable electron addition generally change down a group?
Odpowiedź
It generally becomes less favorable as the added electron enters a larger, more shielded shell, though electron-affinity irregularities are common.
Karta 32
Pytanie
How does metallic character generally change down a group?
Odpowiedź
It increases.
Karta 33
Pytanie
Why does shielding change less than nuclear charge across a main-group period?
Odpowiedź
The added electrons enter the same principal shell, so they do not shield one another as effectively as inner-shell electrons do.
Karta 34
Pytanie
Which has the larger atomic radius, Li or Na?
Odpowiedź
Na. It lies below Li and has an additional occupied electron shell.
Karta 35
Pytanie
Which has the larger atomic radius, Na or Mg?
Odpowiedź
Na. Atomic radius generally decreases from left to right across Period 3.
Karta 36
Pytanie
How does greater electron–nucleus distance affect electrostatic attraction?
Odpowiedź
It weakens the attraction, all else being equal.
Karta 37
Pytanie
How do successive ionization energies for one element compare?
Odpowiedź
Each successive ionization energy is higher than the one before it because an electron is removed from an increasingly positive species.
Karta 38
Pytanie
Which has the higher first ionization energy, Li or Na?
Odpowiedź
Li. Its valence electron is closer to the nucleus and less shielded.
Karta 39
Pytanie
Which has the higher first ionization energy, Na or Mg?
Odpowiedź
Mg. Its greater effective nuclear charge holds the valence electrons more tightly.
Karta 40
Pytanie
Why does forming a cation usually shrink an atom?
Odpowiedź
Electron loss reduces electron–electron repulsion and increases the nuclear pull per remaining electron; losing the outer shell can shrink it sharply.
Karta 41
Pytanie
Which element is most electronegative on the Pauling scale?
Odpowiedź
Fluorine.
Karta 42
Pytanie
Which is more electronegative, Li or Na?
Odpowiedź
Li. Electronegativity generally decreases down Group 1.
Karta 43
Pytanie
Which is more electronegative, Na or Mg?
Odpowiedź
Mg. Electronegativity generally increases across Period 3.
Karta 44
Pytanie
What does a large jump between successive ionization energies reveal?
Odpowiedź
The next electron would come from a lower, core shell; the number removed before the jump indicates the valence-electron count for a main-group atom.
Karta 45
Pytanie
Why is Cl⁻ larger than neutral Cl?
Odpowiedź
The added electron increases repulsion within the valence shell while the nuclear charge stays the same.
Karta 46
Pytanie
How do you compare the radii of isoelectronic species?
Odpowiedź
The species with more protons is smaller because the same number of electrons feels a stronger nuclear attraction.
Karta 47
Pytanie
Why does an atom have no single sharp physical radius?
Odpowiedź
Its electron cloud has no hard edge, so atomic size depends on a defined measurement such as covalent, metallic, or van der Waals radius.
Karta 48
Pytanie
Why are noble-gas electronegativities often omitted in introductory tables?
Odpowiedź
Electronegativity describes attraction in a bond, and many noble gases form too few ordinary bonds for a standard value to be useful on common scales.
Karta 49
Pytanie
Why does forming an anion usually expand an atom?
Odpowiedź
The extra electron increases electron–electron repulsion and lowers the nuclear pull available per electron.
Karta 50
Pytanie
Order O²⁻, F⁻, and Ne from largest to smallest radius.
Odpowiedź
O²⁻ > F⁻ > Ne. All have 10 electrons, and increasing proton count pulls that electron cloud inward.
Karta 51
Pytanie
After which removal does Na show its first large ionization-energy jump?
Odpowiedź
After the first electron. Removing one valence electron leaves a stable core, so the second removal reaches that core.
Karta 52
Pytanie
Does electronegativity difference create a universal ionic-versus-covalent cutoff?
Odpowiedź
No. A larger difference usually means more bond polarity, but bonding lies on a continuum and context matters.
Karta 53
Pytanie
How do noble gases generally differ from halogens in electron affinity?
Odpowiedź
Adding an electron to a noble gas is generally unfavorable because it must begin a higher-energy shell; halogens usually gain one much more favorably.
Karta 54
Pytanie
Which is smaller, Na⁺ or Mg²⁺?
Odpowiedź
Mg²⁺. Both have 10 electrons, but Mg²⁺ has one more proton.
Karta 55
Pytanie
After which removal does Mg show its first large ionization-energy jump?
Odpowiedź
After the second electron. Mg has two valence electrons, so the third removal reaches a core shell.
Karta 56
Pytanie
How does electronegativity differ from electron affinity?
Odpowiedź
Electronegativity is a relative measure of attraction for shared electrons in a bond; electron affinity is an energy change for adding an electron to an isolated gaseous species.
Karta 57
Pytanie
How are atomic radius and first ionization energy generally related?
Odpowiedź
A larger radius usually means a lower first ionization energy because the valence electron is farther from the nucleus and easier to remove.
Karta 58
Pytanie
Which has the more exothermic first electron affinity, F or Cl?
Odpowiedź
Cl. Fluorine's very compact 2p shell creates stronger electron–electron repulsion for the incoming electron, so this pair breaks the simple down-group expectation.
Karta 59
Pytanie
Which has the higher first ionization energy, Be or B?
Odpowiedź
Be. B loses a higher-energy 2p electron, while Be loses a more penetrating 2s electron from a filled 2s subshell.
Karta 60
Pytanie
Why does Group 1 metal reactivity generally increase down the group?
Odpowiedź
The valence electron is farther out and more shielded, so its first ionization energy falls and electron loss becomes easier.
Karta 61
Pytanie
How are atomic radius and electronegativity generally related?
Odpowiedź
Smaller atoms usually attract bonding electrons more strongly, so electronegativity tends to rise as radius falls.
Karta 62
Pytanie
Why is Na⁺ much smaller than neutral Na?
Odpowiedź
Na loses its entire third-shell valence level, leaving the smaller neon-like electron configuration.
Karta 63
Pytanie
Which has the higher first ionization energy, Mg or Al?
Odpowiedź
Mg. Al's removed electron is a higher-energy 3p electron, while Mg loses a more penetrating 3s electron from a filled 3s subshell.
Karta 64
Pytanie
Why does halogen reactivity generally decrease down Group 17?
Odpowiedź
Larger radius and greater shielding weaken attraction for an incoming electron, so oxidizing ability generally falls. Particular reactions still depend on bond energies and conditions.
Karta 65
Pytanie
Why do Groups 2 and 15 often interrupt the simple electron-affinity trend?
Odpowiedź
Group 2 has a filled s subshell and Group 15 has a half-filled p subshell, so an added electron enters a less favorable arrangement.
Karta 66
Pytanie
Can ion charge alone rank two unrelated ionic radii?
Odpowiedź
No. Shell number, electron count, proton count, oxidation state, and crystal environment can all matter; the isoelectronic rule needs the same electron count.
Karta 67
Pytanie
Which has the higher first ionization energy, N or O?
Odpowiedź
N. Its half-filled 2p subshell is relatively stable; O has one paired 2p orbital, and repulsion makes one electron easier to remove.
Karta 68
Pytanie
In which direction does nonmetallic character generally increase?
Odpowiedź
Up and to the right, opposite the general trend in metallic character.
Karta 69
Pytanie
Within the same principal shell, which penetrates closer to the nucleus: an s or p orbital?
Odpowiedź
An s orbital. Greater penetration means its electrons are less shielded and usually lower in energy than p electrons in the same shell.
Karta 70
Pytanie
How do same-charge ion radii generally change down a group?
Odpowiedź
They increase as occupied electron shells are added.
Karta 71
Pytanie
Which has the higher first ionization energy, P or S?
Odpowiedź
P. Its half-filled 3p subshell is relatively stable; S contains a paired 3p orbital that increases repulsion and eases removal.
Karta 72
Pytanie
Why should simple periodic-direction rules be used cautiously for transition metals?
Odpowiedź
d-electron filling, shielding, oxidation state, and contraction effects make their property changes less regular than main-group trends.
Karta 73
Pytanie
Why do periodic-trend statements usually say “generally”?
Odpowiedź
Subshell energies, electron pairing, radius definitions, and element-specific configurations create real exceptions to the broad patterns.
Karta 74
Pytanie
Which has the larger atomic radius, K or Br?
Odpowiedź
K. Both are in Period 4, and atomic radius generally decreases from left to right.
Karta 75
Pytanie
Which has the higher first ionization energy, Mg or Cl?
Odpowiedź
Cl. Its valence electrons experience greater effective nuclear charge and are held more tightly.
Karta 76
Pytanie
Which is more electronegative, Al or Si?
Odpowiedź
Si. Electronegativity generally increases across Period 3.
Karta 77
Pytanie
Which has the larger atomic radius, O or F?
Odpowiedź
O. Atomic radius generally decreases across Period 2.
Karta 78
Pytanie
Which has the higher first ionization energy, K or Br?
Odpowiedź
Br. First ionization energy generally increases across Period 4.
Karta 79
Pytanie
Which is more electronegative, Mg or Cl?
Odpowiedź
Cl. It lies farther right in Period 3.
Karta 80
Pytanie
Which has the larger atomic radius, Al or Si?
Odpowiedź
Al. Atomic radius generally decreases across Period 3 as effective nuclear charge rises.
Karta 81
Pytanie
Which has the higher first ionization energy, O or F?
Odpowiedź
F. This pair follows the general increase across Period 2.
Karta 82
Pytanie
Which is more electronegative, K or Br?
Odpowiedź
Br. Electronegativity generally increases across Period 4.
Karta 83
Pytanie
Which has the larger atomic radius, Mg or Cl?
Odpowiedź
Mg. Both are in Period 3, and Mg lies farther left.
Karta 84
Pytanie
Which has the higher first ionization energy, Al or Si?
Odpowiedź
Si. This pair follows the general increase across Period 3.
Karta 85
Pytanie
Which is more electronegative, O or F?
Odpowiedź
F, the most electronegative element on the Pauling scale.
Karta 86
Pytanie
Order Al³⁺, Mg²⁺, Na⁺, Ne, F⁻, and O²⁻ from smallest to largest radius.
Odpowiedź
Al³⁺ < Mg²⁺ < Na⁺ < Ne < F⁻ < O²⁻. All have 10 electrons, so radius grows as proton count falls.
Karta 87
Pytanie
Why do upper-right nonmetals usually hold valence electrons tightly?
Odpowiedź
Their relatively small radii and high effective nuclear charges create strong attraction between the nucleus and valence electrons.
Karta 88
Pytanie
Across a main-group period, what shared cause links smaller radius, higher ionization energy, and higher electronegativity?
Odpowiedź
Increasing effective nuclear charge pulls the same-shell valence electrons inward and holds them more strongly.
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Periodic Trends Flashcards: Atomic Radius, Ionization Energy & Electronegativity
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